The mole fraction of methanol is 0.100 in a 78.0-g 78.0-g aqueous solution of methanol, ch4o, ch 4 o. Is the mass of methanol in the solution is 7.809 g and the mass of water is 39.425 g.
The mole fraction of methanol (CH4O) in the solution is 0.100, which means that 10% of the moles of the solution are methanol. We can use this information, along with the total mass of the solution, to determine the mass of each component.
The total moles of the solution can be calculated by dividing the total mass of the solution by its molar mass. Methanol has a molar mass of 32.04 g/mol, so we have:
total moles of solution = 78.0 g / 32.04 g/mol = 2.434 mol
Now we can calculate the moles of methanol:
moles of methanol = 0.100 x 2.434 mol = 0.2434 mol
The remaining moles are water:
moles of water = 2.434 mol - 0.2434 mol = 2.1906 mol
To calculate the mass of each component, we can use their respective molar masses:
mass of methanol = 0.2434 mol x 32.04 g/mol = 7.809 g
mass of water = 2.1906 mol x 18.02 g/mol = 39.425 g
Therefore, the mass of methanol in the solution is 7.809 g and the mass of water is 39.425 g.
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What is the process of separating a mixture into its individual components called?
Answer:
separation
Explanation:
The process of separating a mixture into its individual components is called separation. This can be achieved through various methods such as physical separation techniques, such as filtration, centrifugation, and evaporation, or chemical separation techniques, such as extraction and distillation. The specific method used depends on the type of mixture and the properties of the components. The goal of separation is to isolate the individual components of the mixture in their pure form.
ALLEN
A student measures the mass of a solution before and after a chemical reaction takes place. In both cases the student measures the mass to be 50.25 g on an electronic balance with an uncertainty of 0.05 g. The student realizes that the ranges of uncertainty for each measurement overlap exactly. Which claim can the student make?
(a) The mass definitely stayed the same because the ranges of uncertainty overlap exactly.
(b) We can't know for sure whether or not the mass changed, but it seems reasonable to claim that the mass did not change, given that the ranges of uncertainity overlap.
(c) The mass definitely stayed the same because the measurement of 50.25 g was obtained each time.
The correct option is (b) We can't know for sure whether or not the mass changed, but it seems reasonable to claim that the mass did not change, given that the ranges of uncertainty overlap.
The overlap of the ranges of uncertainty for each measurement indicates that the masses of the solution before and after the reaction are consistent with each other. However, this does not provide definite proof that the mass did not change, as there is still some uncertainty associated with the measurements. The student's conclusion is reasonable, given the information provided, but further investigation is needed to determine if the mass did actually stay the same.
In scientific experiments, it is common to make multiple measurements of a quantity and report the results along with the associated uncertainty. The uncertainty represents the degree of precision with which the measurement was made, and it is typically expressed as a range of values. In this case, the student made two measurements of the mass of the solution with an uncertainty of 0.05 g, and the results were 50.25 g ± 0.05 g for both measurements.
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What is the volume, in liters, of 0.250 mole of oxygen gas at 20.0 C and 0.974 atm of
pressure?
The volume in liters, of 0.250 mole of oxygen gas at 20.0 C and 0.974 atm of pressure is 6.174L.
How to calculate volume?The volume of a substance can be calculated by using Avogadro's law equation as follows:
PV = nRT
Where;
P = pressureV = volume n = number of molesR = gas law constantT = temperatureAccording to this question, a 0.250 mole of oxygen gas at 20.0 C and 0.974 atm of pressure. The volume of the gas is calculated as follows:
0.974 × V = 0.250 × 293 × 0.0821
0.974V = 6.013825
V = 6.174L
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What would you observe if benzene was shaken with bromine water? Does this support or oppose Kekulé’s model of benzenes structure. Explain your answer.
Answer:
If benzene was shaken with bromine water, you would observe a slow reaction, as bromine water is a weak oxidizing agent. The reaction would result in the formation of bromobenzene, which is a yellow or reddish-brown solution.
This observation supports Kekulé's model of benzene's structure, as Kekulé proposed that benzene had alternating double bonds in its ring. This allows for the slow reaction with bromine water as the electrons in the double bonds can participate in the reaction to form bromobenzene. In contrast, if benzene had a structure with only single bonds, the reaction would occur more rapidly.
Explanation:
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an ionic compound will dissolve when the attraction between the ______ molecules and the ions is greater than the attraction between the _____ themselves
An ionic compound will dissolve when the attraction between the polar molecules and the ions is greater than the attraction between the ions themselves.
Polar motes A polar patch is generally formed when the one end of the patch is said to retain more positive charges and whereas the contrary end of the patch has negative charges, creating an electrical pole. When a patch is said to have a polar bond, also the centre of the negative charge will be on one side, whereas the centre of positive charge will be in the different side. The entire patch will be a polar patch.
Ion, any snippet or group of tittles that bears one or further positive or negative electrical charges. appreciatively charged ions are called cations; negatively charged ions, anions. Ions are formed by the addition of electrons to, or the junking of electrons from, neutral tittles or motes or other ions.
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15.6g potassium (K). How many moles of potassium oxide would be produced assuming you had unlimited oxygen? ____ K + ____ O2 → _____ K2O
15.6g of potassium would produce 1 mole of potassium oxide 15.6g K + 0.8 mol O2 → 1.2 mol K2O.
What is potassium?Potassium is an essential mineral that plays an important role in a number of bodily functions. It is a type of electrolyte that helps regulate the body's water balance, acid-base balance, and heart rate. It also helps to maintain healthy muscle and nerve function, as well as normal blood pressure. Potassium can be found in many foods, including fruits, dairy products, legumes, nuts, and leafy green vegetables.
Assuming you had unlimited oxygen, 15.6g of potassium would produce 1 mole of potassium oxide (K2O). This is because the molar mass of potassium oxide is 94.2 g/mol and there are 2 moles of oxygen for every 1 mole of potassium in the reaction equation: K + O2 → K2O.
Therefore, 15.6g of potassium would produce 1 mole of potassium oxide, which can be calculated as follows:
15.6g K / (39.1g K/mol) = 0.4 mol K
0.4 mol K x (2 mol O2/1 mol K) = 0.8 mol O2
0.4 mol K + 0.8 mol O2 = 1.2 mol K2O
Therefore, the answer is:
15.6g K + 0.8 mol O2 → 1.2 mol K2O
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the table above provides the values for some physical properties of h2s and h2o . approximately, how many moles of h2s must be condensed to release as much heat as would be released when 1 mole of h2o is condensed? responses
In order to generate the same amount of heat as 1 mole of H2O, approximately 2 moles of H2S must be condensed.
A colourless gas noted for its strong "rotten egg" smell at low concentrations is hydrogen sulphide. It is exceedingly poisonous and combustible.
Compared to hydrogen sulphide, one mole of water requires about 40.7 kJ/mol of enthalpy to vaporise.
To produce the same amount of heat, more hydrogen sulphide must condense into water. Because water has a higher enthalpy of vaporisation than hydrogen sulphide, this happens.
Hence, around two moles of hydrogen sulphide will give the heat produced as one mole of water produces.
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The complete question is-
the table above provides the values for some physical properties of h2s and h2o . approximately, how many moles of h2s must be condensed to release as much heat as would be released when 1 mole of h2o is condensed? responses
chlorine gas (cl2) reacts with phosphorus (p) to produce phosphorus trichloride (pcl3). how many grams of pcl3 can be produced (what is the theoretical yield of pcl3) when 62.54 g of cl2 are reacted with 12.39 g of p?
The theoretical yield of PCl₃ produced from the reaction of 62.54 g of Cl₂ with 12.39 g of P is 54.93 g.
To determine the theoretical yield of PCl₃ produced from the reaction of 62.54 g of Cl₂ with 12.39 g of P, we first need to write a balanced chemical equation for the reaction:
P + 3Cl₂ → PCl₃
From the balanced equation, we can see that 1 mole of P reacts with 3 moles of Cl₂ to produce 1 mole of PCl₃. Therefore, we need to convert the given masses of Cl₂ and P into moles using their respective molar masses:
Molar mass of Cl₂ = 35.45 g/mol
Molar mass of P = 30.97 g/mol
Number of moles of Cl₂ = 62.54 g / 35.45 g/mol = 1.764 mol
Number of moles of P = 12.39 g / 30.97 g/mol = 0.400 mol
The limiting reactant in this reaction is P, since it produces less moles of product than Cl₂. Therefore, we will use the number of moles of P to determine the theoretical yield of PCl₃:
Number of moles of PCl₃ = 0.400 mol
To convert the number of moles of PCl₃ to grams, we use its molar mass:
Molar mass of PCl₃ = 137.33 g/mol
The theoretical yield of PCl₃ produced is:
Theoretical yield of PCl₃ = 0.400 mol × 137.33 g/mol = 54.93 g
Therefore, the theoretical yield of PCl₃ produced from the reaction of 62.54 g of Cl₂ with 12.39 g of P is 54.93 g.
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An unknown amount of a radioactive isotope with a half-life of 2.0 h was observed for 6.0 h. If the amount of the isotope remaining after 6.0 h was 24 g, what would the original amount have been?
A.3 g
B.4 g
C.144 g
D.192 g
The original amount of of the isotope remaining after 6.0 h was 24 g would have been 144g.
Thus, the correct answer is D.
To solve this problem, we need to use the formula for radioactive decay:
A = A0 * (1/2)^(t/t1/2)
Where A is the amount of the radioactive isotope remaining after time t, A0 is the original amount of the isotope, t1/2 is the half-life of the isotope, and t is the time elapsed.
In this case, we know that A = 24 g, t1/2 = 2.0 h, and t = 6.0 h. We need to find A0.
Plugging in the known values into the formula, we get:
24 g = A0 * (1/2)^(6.0 h / 2.0 h)
Simplifying the equation, we get:
24 g = A0 * (1/2)^3
24 g = A0 * (1/8)
Multiplying both sides of the equation by 8, we get:
192 g = A0
Therefore, the original amount of the radioactive isotope was 192 g.
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which process requires more energy: completely vaporizing 1 kg of saturated liquid water at 1 atm pressure of completely vaporizing 1 kg of saturated water at 8 atm pressure? explain by using the property table.
The process requires more energy: is completely vaporizing 1 kg of saturated liquid water at 1 atm pressure.
The The process requires more energy: is completely vaporizing 1 kg of saturated liquid water at 1 atm pressure. This is because from the latent heat of vaporization of the each system. For the system 1, saturated the water at 1 atm, the latent heat of vaporization is equal to 40.7 kJ per mole and for, at 8 atm, the latent heat of vaporization is equal to 36.4 kJ per mole.
Thus, the completely vaporizing 1 kg of saturated liquid water at 1 atm pressure requires the more energy.
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Transcribed image text: Which two rings have approximately the same bond angle in their favored conformations? cyclopropane O cyclobutane O cyclohexane cyclopentane o cycloheptane Which ring(s) sacrifice bond angle to relieve torsional strain? cyclobutane cyclopropane cycloheptane cyclopentane cyclohexane Which strain(s) are a type of steric interaction? O transannular strain O ring strain O torsional strain bond angle strain
The two rings that have approximately the same bond angle in their favored conformations are cyclopropane and cyclopropane. The rings that sacrifice bond angle to relieve torsional strain are cyclopropane and cyclobutane.
Bond angle strain is a type of steric interaction.
A cyclic ring is a closed chain of atoms, typically carbon, that forms a loop or ring structure. Cyclic rings are commonly found in organic molecules, and the properties and behavior of cyclic rings can vary depending on their size, shape, and composition.
Cyclic rings can be classified based on the number of atoms in the ring, with three-membered rings known as cyclopropanes, four-membered rings known as cyclobutanes, five-membered rings known as cyclopentanes, six-membered rings known as cyclohexanes, and so on. The stability and reactivity of cyclic rings can also be affected by the presence of functional groups and the stereochemistry of the ring.
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magnesium has an hcp crystal structure, a c/a ratio of 1.624, and a density of 1.74 g/cm3. compute the atomic radius for mg.
The atomic radius of magnesium is approximately 1.736 Å. This can be calculated using the formula: Atomic Radius = (a / 2) * sqrt(3), where a is the lattice parameter for the hcp crystal structure.
To calculate the atomic radius of magnesium, we can use the following formula:
Density = (2 * Atomic Mass) / [(a²) * (c / a) * Na]
where:
Density is the density of magnesium
Atomic Mass is the atomic mass of magnesium
a is the lattice parameter for the hcp crystal structure
c/a is the ratio of the height of the unit cell to the base length of the unit cell
Na is Avogadro's number
We can rearrange this formula to solve for the atomic radius:
Atomic Radius = (a / 2) * sqrt(3)
where:
a is the lattice parameter for the hcp crystal structure
Now, let's plug in the values given in the problem:
Density = 1.74 g/cm3
c/a = 1.624
Na = 6.022 x 10²³ molecules/mol
The atomic mass of magnesium is 24.305 g/mol.
To find the lattice parameter, we can use the fact that the volume of the unit cell is given by:
Volume = a² * (c / a) * sqrt(3) / 2
The density is also related to the volume and the atomic mass by:
Density = Atomic Mass / Volume
We can combine these two equations and solve for a:
a = (4 * Atomic Mass / (sqrt(3) * Density * c))⁽¹/³⁾
Plugging in the values:
a = (4 * 24.305 g/mol / (sqrt(3) * 1.74 g/cm^3 * 1.624))⁽¹/³⁾
a = 3.209 Å
Now we can calculate the atomic radius:
Atomic Radius = (a / 2) * sqrt(3)
Atomic Radius = (3.209 Å / 2) * sqrt(3)
Atomic Radius = 1.736 Å (rounded to three significant figures)
Therefore, the atomic radius of magnesium is approximately 1.736 Å.
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what is the polarity of slime molecules
Slime is a non-Newtonian fluid and does not have a molecular structure that can be considered polar or non-polar. The term "polarity" typically refers to the distribution of electrical charge within a molecule. In the case of slime, the material is made up of polymer molecules, which are long chains of repeating units. These polymer molecules interact with each other through hydrogen bonding, which gives the material its unique properties such as being a non-Newtonian fluid. However, these interactions are not based on polarity, so it is not appropriate to describe slime as being polar or non-polar.
Answer:
The polarity of slime molecules depends on the specific type of slime. There are many different types of slime, each made up of different types of molecules.
For example, if we consider a typical type of slime made from polyvinyl alcohol (PVA), the polarity of the PVA molecules will depend on their molecular structure and the type of bonding between the atoms. PVA is a synthetic polymer made up of repeating units of vinyl alcohol, which has a polar hydroxyl group (-OH). As a result, PVA is considered to be a polar molecule.
However, the overall polarity of a slime made from PVA will also depend on the other ingredients that are present, such as borax, which is often used as a cross-linking agent to form the slime. The overall polarity of the slime will also depend on the conditions it is in, such as the temperature, pH, and the presence of other substances that could affect the polarity of the slime.
In summary, the polarity of slime molecules can be complex and depends on the specific type of slime, the ingredients that make it up, and the conditions it is in.
Explanation:
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How many moles of oxygen atoms are present in 1 mole of Iron (III)oxide?
The formula for Iron (III) oxide is Fe2O3, which means that there are 2 iron atoms and 3 oxygen atoms in one molecule of Fe2O3.
What do you mean by molecules?
A molecule is a group of two or more atoms held together by chemical bonds. These atoms can be of the same or different types. Molecules are the smallest units of a compound that retain the chemical and physical properties of that compound.
Molecules play a critical role in many chemical reactions and biological processes. They can interact with each other through chemical reactions to form new compounds or release energy. Understanding the structure and behavior of molecules is fundamental to understanding many fields of science, including chemistry, biochemistry, and materials science.
The formula for Iron (III) oxide is Fe2O3, which means that there are 2 iron atoms and 3 oxygen atoms in one molecule of Fe2O3.
To find the number of moles of oxygen atoms in 1 mole of Fe2O3, we need to multiply the number of oxygen atoms per molecule by the Avogadro constant (6.022 x 10^23).
Number of moles of oxygen atoms in 1 mole of Fe2O3 = 3 x (6.022 x 10^23) = 1.8066 x 10^24
Therefore, there are 1.8066 x 10^24 oxygen atoms in 1 mole of Fe2O3.
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15. How many atoms are in a 3.56g sample of Cu?
15. How many atoms are in a 3.56g sample of Cu?
Considering the definition of Avogadro's Number, 7.37×10²² moles of Cu are in a 3.56g sample of Cu?
Definition of molar massThe molar mass of substance is the amount of mass that a substance contains in one mole.
Definition of Avogadro's NumberAvogadro's Number is the number of particles that make up a substance (usually atoms or molecules) in the amount of one mole of the substance. Its value is 6.023×10²³ particles per mole.
Avogadro's number applies to any substance.
Moles of CuThe molar mass of Cu is 63.54 g/mole. The amount of moles of Cu can be calculated as:
amount of moles= 3.56 g÷ 63.54 g/mole
amount of moles= 0.056 moles
Now you can apply the following rule of three: 1 mole of the compound has 6.023×10²³ atoms, 0.056 mole contains how many atoms?
amount of atoms of Cu= (0.056 moles ×6.023×10²³ atoms)÷ 1
amount of atoms of Cu= 7.37×10²²
Finally, 7.37×10²² moles of Cu are present.
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A compound has a molar mass of 123.22 g/mol. what is the molecular formula of a substance that has this molar mass? A. CoH4. B. PSF3
C. SrS
D. ZrO2
A compound which has molar mass 123.22g/mol will have a molecular formula as ZrO₂. so the correct option is D.
We need to know the empirical formula of the compound and the quantity of empirical formula units in the molecular formula in order to determine the molecular formula of a substance with a certain molar mass.
The mass of a certain molecule is its molecular mass, which is expressed in daltons. Because they contain various isotopes of an element, multiple molecules of the same substance can have distinct molecular weights.
A) Co₂H₄:
Co: 2 x 58.93 = 117.86
H: 4 x 1.01 = 4.04
Total: 121.9 g/mol
B) PSF:
P: 1 x 30.97 = 30.97
S: 1 x 32.06 = 32.06
F: 1 x 18.99 = 18.99
Total: 82.02 g/mol
C) SrS₃:
Sr: 1 x 87.62 = 87.62
S: 3 x 32.06 = 96.18
Total: 183.8 g/mol
D) ZrO₂:
Zr: 1 x 91.22 = 91.22
O: 2 x 16.00 = 32.00
Total: 123.22 g/mol
The number of empirical formula units in the molecular formula can now be determined by dividing the supplied molar mass by the empirical formula weight:
A)Co₂H₄: 123.22 / 121.9 = 1.01, meaning that the molecular formula and the empirical formula,Co₂H₄, are nearly identical.
B) PSF: 123.22 divided by 82.02 equals 1.50, which means the molecular formula is 1.5 times the empirical formula and can be rounded to PS3F3PS₃F₃.
CSrS₃: 123.22 / 183.8 = 0.67, which means that the molecular formula is equal to 0.67 times the empirical formula, or SrS₂.
D) ZrZrO₂2: Because the molar mass and empirical formula weight are already equal, the molecular formula, ZrO₂, is also the empirical formula.
Consequently, D) ZrO2rO₂ is the chemical formula for the substance with a molar mass of 123.22 g/mol.
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How many moles of glucose did your body consume if you exhale 100 grams of carbon dioxide?
C6H12O6 + 6O2 = 6CO2 + 6H2O
24 g of pure CO2 are exhaled by the individual. To calculate the number of moles, divide the outcome by the molar mass. As a result, the individual exhales about 0.55 moles of carbon dioxide every hour.
What impact on glucose molecule due to exhale of Co2?During aerobic cellular respiration, the interaction of glucose and oxygen results in the production of ATP that the cell can utilize.
As by-products, water and carbon dioxide are produced. The general formula for aerobic cellular respiration is: During cellular respiration, oxygen and glucose combine to create ATP.
CO2 is converted to glucose during photosynthesis, and H2O is oxidized to produce oxygen. Cellular respiration involves the reduction of oxygen and the oxidation of glucose to produce CO2 and water.
CO2 is carried by the bloodstream to the lungs, where it is eventually exhaled out of the body.
Therefore, Hence Number of moles glucose, C6H12O6 = 100g/180g = 0.55 moles.
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What is molar ratio of Mg reacted to H2 produced? what is the stoichiometric ratio between the mg ribbon reactant and the hydrogen gas product?
The molar ratio of Mg reacted to H2 produced is 1:1. This means that for every mole of Mg that reacts, one mole of H2 is produced. The stoichiometric ratio between the Mg ribbon reactant and the hydrogen gas product is also 1:1.
This ratio is determined by the balanced chemical equation for the reaction between Mg and HCl, which is Mg + 2HCl → MgCl2 + H2. The coefficients in this equation represent the number of moles of each reactant and product that are involved in the reaction. The coefficient for Mg is 1, indicating that one mole of Mg reacts with two moles of HCl to produce one mole of H2 and one mole of MgCl2.
The stoichiometric ratio is important because it allows us to determine the number of reactants or products needed in a reaction. For example, if we know the amount of Mg we have, we can use the stoichiometric ratio to calculate the amount of H2 that will be produced. Similarly, if we know the amount of H2 we need, we can use the stoichiometric ratio to determine how much Mg we need to react with HCl to produce the required amount of H2.
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write a chemical formula of one compound formed by the combination of k ions with one of these ions as water completely evaporates from the seawater sample.
Chemical formula of one compound formed by the combination of K+ ions with one of these ions as water completely evaporates from the seawater sample is KCl( Poassium Chloride).
Potassium chloride is an ionic compound that contains the ions K+ and Cl-. The K+ ions and Cl- ions create an ionic connection when the water evaporates from the saltwater sample. Because the K+ and Cl- ions are attracted to each other, the bond forms when the two ions create a symmetrical configuration.
The process of ionic bonding is a key aspect of seawater chemistry. Several dissolved ions are found in seawater, including K+, Na+, Ca2+, and Mg2+. The dissolved ions get concentrated when the water evaporates and interact with other ions to create compounds. In the case of KCl, the K+ ions will create an ionic connection with the Cl- ions, which is a strong bond that binds the two ions together.
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how much heat is required to evaporate 100.0 g of liquid ammonia, nh3, at its boiling point if its enthalpy of vaporization is 4.8 kj/mol?
The total amount of heat required to evaporate hundred gram of liquid Ammonia at its boiling point is found to be 28 KJ.
The enthalpy of vaporization from liquid ammonia is given to be 4.8 kilo joule per mole.
The mass of the liquid ammonia is 100 grams.
The formula to find the amount of heat required to evaporate this ammonia is given by,
Q = nL
Where, m is the moles of ammonia and L is the latent heat of vaporization.
Putting all the values,
Q = 100/17 x 4.8 KJ/mol
Q = 28 KJ
So, a total of 28 kilo joules of energy will be required to evaporate these ammonia.
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Okay I actually have a question this time can someone please help me with this table and the question? I tried doing it but my teacher said it was wrong so-
The temperature is increasing the three degrees.
Does heat affect enthalpy of reaction?The enthalpy of a reaction, also known as the heat of reaction, can be affected by changes in temperature. Enthalpy is a measure of the total energy in a system, including both heat and internal energy.
In a chemical reaction, the enthalpy change is the heat absorbed or released during the reaction, which can be measured as the temperature change of the system. When the temperature of a reaction increases, the enthalpy of the system will increase, and when the temperature decreases, the enthalpy of the system will decrease.
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An organic compound containing 40% carbon, 6.67% hydrogen and rest of oxygen, has the molecular mass 180g.mol-1. Find out the EF as well as MF of the compound.
Answer:
The EF of the compound is CH2O and the MF is C6H12O6.
Explanation:
To find the empirical formula (EF) of the compound, we need to determine the simplest whole number ratio of the atoms in the compound. We can assume we have 100 g of the compound, which means we have:
40 g of carbon
6.67 g of hydrogen
53.33 g of oxygen (since the rest of the compound is oxygen)
Next, we can convert the masses to moles:
Moles of carbon = 40 g / 12.01 g/mol = 3.33 mol
Moles of hydrogen = 6.67 g / 1.01 g/mol = 6.61 mol
Moles of oxygen = 53.33 g / 16.00 g/mol = 3.33 mol
We then divide each of the mole values by the smallest number of moles, which is 3.33, to get the simplest whole number ratio:
Carbon: 3.33 / 3.33 = 1
Hydrogen: 6.61 / 3.33 = 1.98 (rounded to 2)
Oxygen: 3.33 / 3.33 = 1
So the EF of the compound is CH2O.
To find the molecular formula (MF), we need to know the molecular mass of the EF. The empirical formula mass (EFM) of CH2O is:
EFM = (1 x 12.01 g/mol) + (2 x 1.01 g/mol) + (1 x 16.00 g/mol) = 30.03 g/mol
We can then calculate the molecular formula mass (MFM) by dividing the given molecular mass (180 g/mol) by the EFM:
MFM = 180 g/mol / 30.03 g/mol = 6
This means the MF is 6 times the EF, or C6H12O6. Therefore
The total pressure of gases inside a vessel is 2.07×104 kPa. The partial pressure of oxygen in the tank is 8.27 × 10³ kPa.
What is the percentage of oxygen in the vessel?
21%
25%
40%
90%
The 40% is the percentage of oxygen in the vessel.
What is pressure ?
As force applied per unit area, pressure is defined. P=FA, where F is the force operating perpendicular to the surface area A, gives it mathematical expression. The pascal (Pa), which equates to a newton per square metre (N/m 2), is the accepted unit of pressure.
What is partial pressure ?
The idea of partial pressure arises from the fact that each individual gas contributes a portion of the total pressure, and that portion is the partial pressure of that gas. In order to describe all the pieces, it is essentially like taking a percentage or fraction of the whole.
Therefore, The 40% is the percentage of oxygen in the vessel.
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What type of fault has the geologist found?
Given the following occasion 4p+5O2-> 2P2O5. How many moles of P2O5 are formed from 3.4moles of O2
Answer:
3.4 (2/5) (sorry i dont have a calculator )
Explanation:
3.4 moles of O2 x (2 moles of P2O5/5 moles of O2)
= 3.4 (2/5)
question 3
pls help asap
The molar mass and the mole ratio from the reaction equation B. 305.9 grams Al2O3
What is molar mass?Molar mass is a physical property of a chemical compound, defined as the mass of a given substance divided by the amount of substance measured in moles. It is expressed in g/mol and is numerically equal to the average atomic weight of the atoms in the compound. Molar mass is used to calculate the mass of a given amount of a substance, as well as to determine the relative atomic mass of an element.
The molar mass of aluminum is 26.98 g/mol, and the molar mass of aluminum oxide is 101.96 g/mol. Using the molar mass and the mole ratio from the reaction equation, we can calculate the amount of Al2O3 produced.
6.000 mol Al x (2 mol Al2O3/3 mol Al) x (101.96 g Al2O3/1 mol Al2O3) = 305.9 g Al2O3
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this is a tiny unit of an element that retains the properties of the element. it is called___
The correct answer is Atom is the tiny unit of an element that retains the properties of the element.
An atom is a kind of particle that has an electron cloud surrounding its protons and neutrons-filled nucleus. The atom is the basic building block of the chemical elements, and it is the protons in an atom that allow us to distinguish one chemical element from another. For instance, every atom with 11 protons is sodium, while any atom with 29 protons is copper. The quantity of neutrons in an element determines its isotope.
Atoms are very small, with a diameter of around 100 picometers. An typical human hair has about one million carbon atoms. Standard microscopes cannot observe atoms since this is smaller than the smallest wavelength of the visible light spectrum.
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How many moles are in 5.12 × 10³ F atoms?
Answer in units of mole
The number of moles in 5.12 × 10³ Fluorine(F) atoms is 8.45 × 10 ‐ ²³ moles.
The moles is defined as the measurement of the amount of any substance. Its is the measure of the amount of elementary particles in a substance. One mole is numerically equal to 6.023 × 10²³ which is called Avogadro's number.
From Periodic Table, we can find that Molecular Weight of Fluorine(F) is 19. We know the Molar Weight of any element is numerically equal to its Molecular Weight i.e. numerically, Molecular Weight = Molar Weight of any matter.
The number of moles in 5.12 × 10³ Fluorine(F) atoms will be calculated as: (5.12 × 10³) / (6.023 × 10²³) = 8.45 × 10 ‐ ²³ moles
So, there are approximately 8.45 x 10^-23 moles in 5.12 × 10³ atoms of Fluorine.
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What is the value of electron gain enthalpy of Na+ if the first Ionization enthalpy of Na is 5.1 e.v
The electron gain enthalpy of Na+ is 5.65 eV.
What is electron gain enthalpy?The amount of energy released when an electron is added to a single gaseous atom is known as the electron gain enthalpy. Energy can either be released or absorbed when an electron is added.
The electron gain enthalpy of Na+ can be calculated using the formula below:
Electron gain enthalpy of Na+ = Ionization enthalpy of Na - Electron affinity of Na
The ionization enthalpy of Na is 5.1 eV.
The electron affinity of Na is -0.55 eV.
Therefore, the electron gain enthalpy of Na+ can be calculated as:
Electron gain enthalpy of Na+ = Ionization enthalpy of Na - Electron affinity of Na
Electron gain enthalpy of Na+ = 5.1 eV - (-0.55 eV)
Electron gain enthalpy of Na+ = 5.65 eV
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determine the percent error in the experimentally determined value for the enthalpy of formation of mgo.
From the information provided, the percent error in the experimentally determined value for the enthalpy of formation of MgO is 1.96%
To determine the percent error in the experimentally determined value for the enthalpy of formation of MgO, we need to compare the experimental value to the accepted or theoretical value.
The accepted value for the enthalpy of formation of MgO is: -601.8kJ/mol. Let's assume that the experimentally determined value is -590.0 kJ/mol.
The percent error can be calculated using the following formula:
Percent error = |(Experimental value - Theoretical value) / Theoretical value| x 100%
Substituting the values, we get:
Percent error = |(-590.0 kJ/mol - (-601.8 kJ/mol)) / (-601.8 kJ/mol)| x 100%
Percent error = |(11.8 kJ/mol) / (601.8 kJ/mol)| x 100%
Percent error = 1.96%
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