Suppose that 0.84 g of water at 25 °C condenses on the surface of a 51 g block of aluminum that is initially at 25 °C. If the heat released during condensation goes only toward heating the metal, what is the final temperature (in °C) of the metal block? (The specific heat capacity of aluminum is 0.903 J/g °C; enthalpy of vaporization of water is 44.0kJ/mol at at 25 °C. Also, remember that the heat reuired to increase the temperature of a substance by ΔT is given as Q=mCsΔT, where m is the mass of the substance, and Cs its specific heat).
The final temperature of the metal block : t=69.5 °C
Further explanationGiven
0.84 g water
Aluminum block = 51 g
Required
The final temperature
Solution
Enthalpy of vaporization of water is 44.0kJ/mol = 2.44 kJ/g=2440 J/g
Q out=Q in
Q releases = Q absorbed
Q water = Q Aluminum
m.Lf = m.cs.ΔT
0.84 x 2440 J/g = 51 x 0.903 J/g C x (t-25)
2049.6=46.053(t-25)
t=69.5 °C
.
A drawing.Short description, A drawing.,Long description,
The drawing shows a wave of water moving to the right in a container. As the wave moves, the distance between the peak and trough of the wave gets shorter, but the distance between the peaks of the waves remains the same.
Question
What does the drawing show about the energy of the wave as it moves?
Answer options with 4 options
A.
The energy of the wave increases as shown by the increasing frequency.
B.
The energy of the wave decreases as shown by the decreasing amplitude.
C.
The energy of the wave remains the same as shown by the same wavelength.
D.
The energy of the wave regularly increases and decreases as shown by the peaks and troughs.
the picture is this:
Answer:
wow 15 points is alot
Explanation:
Question 3 (1 point)
Consider the following unbalanced chemical equation representing the combustion of methane, yielding carbon dioxide and water.
CH4 + O2 --> CO2 + H20
If you had burned 800 g of methane, how many moles of Carbon dioxide would be produced?
a
b
Ос
122.22
8
2200
100
670
f
750
50
Answer:
50 mol
Explanation:
Mass of methane = 800 g
Number of moles of CO₂ produced = ?
Solution:
Chemical equation:
CH₄ + 2O₂ → CO₂ + 2H₂O
Number of moles of methane:
Number of moles = mass/molar mass
Number of moles = 800 g/ 16 g/mol
Number of moles = 50 mol
Now we will compare the moles of methane and carbon dioxide from balanced chemical equation.
CH₄ : CO₂
1 : 1
50 : 50
The activation energy for a reaction is changed from 184 kJ/mol to 59.0 kJ/mol at 600. K by the introduction of a catalyst. If the uncatalyzed reaction takes about 6900 years to occur, about how long will the catalyzed reaction take
Answer:
The catalyzed reaction will take 2.85 seconds to occur.
Explanation:
The activation energy of a reaction is given by:
[tex] k = Ae^{-\frac{E_{a}}{RT}} [/tex]
For the reaction without catalyst we have:
[tex] k_{1} = Ae^{-\frac{E_{a_{1}}}{RT}} [/tex] (1)
And for the reaction with the catalyst:
[tex] k_{2} = Ae^{-\frac{E_{a_{2}}}{RT}} [/tex] (2)
Assuming that frequency factor (A) and the temperature (T) are constant, by dividing equation (1) with equation (2) we have:
[tex] \frac{k_{1}}{k_{2}} = \frac{Ae^{-\frac{E_{a_{1}}}{RT}}}{Ae^{-\frac{E_{a_{2}}}{RT}}} [/tex]
[tex] \frac{k_{1}}{k_{2}} = e^{\frac{E_{a_{2}} - E_{a_{1}}}{RT} [/tex]
[tex] \frac{k_{1}}{k_{2}} = e^{\frac{59.0 \cdot 10^{3}J/mol - 184 \cdot 10^{3} J/mol}{8.314 J/Kmol*600 K} = 1.31 \cdot 10^{-11} [/tex]
Since the reaction rate is related to the time as follow:
[tex] k = \frac{\Delta [R]}{t} [/tex]
And assuming that the initial concentrations ([R]) are the same, we have:
[tex] \frac{k_{1}}{k_{2}} = \frac{\Delta [R]/t_{1}}{\Delta [R]/t_{2}} [/tex]
[tex]\frac{k_{1}}{k_{2}} = \frac{t_{2}}{t_{1}}[/tex]
[tex] t_{2} = t_{1}\frac{k_{1}}{k_{2}} = 6900 y*1.31 \cdot 10^{-11} = 9.04 \cdot 10^{-8} y*\frac{365 d}{1 y}*\frac{24 h}{1 d}*\frac{3600 s}{1 h} = 2.85 s [/tex]
Therefore, the catalyzed reaction will take 2.85 seconds to occur.
I hope it helps you!
What is the common name for the slow reaction between oxygen and iron?
A. explosion
B. rust
C. rain
Identify the most common reaction conditions for the dehydration of 2,3-dimethyl-2-pentanol. A line-angle structure of 2,3-dimethyl-2-pentanol shows a chain of the following sequence:
a. A line terminus, a segment of three vertices, and a line terminus.
b. A CH3 group is attached to the first (from left to right) and the second vertices.
c. An OH group is attached to the first vertex.
Answer:
1) Acid
2) heat
Explanation:
Dehydration is a type of chemical reaction in which water is removed from an alkanol to yield one or more alkenes.
The reaction normally commences with a protonation of the -OH group by a proton from the acid. Water is always a good leaving group so it quickly departs creating a carbocation. The removal of a proton yields the alkene.
The major product is the one in which there is greater substitution around the C=C double bond.
Someone help me with these questions 15 and 16. You can do 17 if you’d like
Answer:
For question 15, we use cloths, heat-resistant gloves. (From what I know, I am just a 7th grader. Forgive me.)
For question 16, we use bowls to drink soup, metal cans which we use to drink soda from, we use lunch boxes which are insulated or thermos can be used for bringing to school to eat lunch and keeping food warm, we use aluminium foil containers to keep food warm.
For question 17, I think it's related to chart above question 15 and etc, if it isn't then I don't think I may be able to help.
During the phosphatase experiment you will use a 1% w/v of phenolphthalein di-phosphate (PPP). How much PPP do you need to make 750ml of the solution if you only have 25g and you know that the MW of PPP is 478 g/mole
Answer:
Explanation:
1 % w/v of phenolphthalein di-phosphate (PPP)
will contain 1 gram of phenolphthalein di-phosphate (PPP) in 100 mL of solution
750 mL solution will contain 7.5 g of PPP
750 mL solution will contain 7.5 / 478 moles of PPP
750 mL solution will contain .0157 moles of PPP
So 7.5 g of PPP or .0157 mole of PPP will be needed .
Container A holds 717 mL of an ideal gas at 2.80 atm. Container B holds 174 mL of a different ideal gas at 4.30 atm. Container A and container B are glass spheres connnected by a tube with a stopcock. Container A is larger than container B. If the gases are allowed to mix together, what is the resulting pressure
Answer:
3.09 atm
Explanation:
Given that:
Volume of container A = 717 mL
Pressure of container A = 2.80 atm
Volume of container B = 174 mL
Pressure of container B = 4.30 atm
Now, if the valve are being removed and the gases are allowed to mix together; then
The total final pressure can be calculated by using the formula:
[tex]P_f = \dfrac{P_AVA+P_BV_B}{V_A+V_B}[/tex]
[tex]P_f = \dfrac{2.80*717+4.30*174}{717+174}[/tex]
[tex]P_f = \dfrac{2007.6+748.2}{891}[/tex]
[tex]P_f = \dfrac{2755.8}{891}[/tex]
[tex]\mathbf{P_f =3.09 \ atm}[/tex]
The absence of the intermolecular attraction between the atoms or molecules is called an ideal gas. The pressure of the resultant mixture is 3.09 atm.
What is the relation between pressure and volume?The relationship between the pressure and the volume of the gas is given by Boyle's law which states the inverse proportionality relation with the volume.
Given,
The volume of container A = 717 mL
The volume of container B = 174 mL
The pressure of container A = 2.80 atm
The pressure of container B = 4.30 atm
The total final pressure of the ideal gas of the mixture is calculated by:
[tex]\begin{aligned} \rm P_{f} &= \rm \dfrac{P_{A}V_{A}+ P_{B}V_{B}}{V_{A}+V_{B}}\\\\&= \dfrac{2007.6 +748.2}{891}\\\\&= 3.09 \;\rm atm\end{aligned}[/tex]
Therefore, the total pressure of the mixture is 3.09 atm.
Learn more about pressure here:
https://brainly.com/question/13534890
How many grams of IRON are
contained in a 245 gram sample
of Fe2O3?
Answer:
[tex]m_{Fe}=171.7gFe[/tex]
Explanation:
Hello!
In this case, since we have 245 of iron (III) oxide, we first need to compute the moles contained there:
[tex]n_{Fe_2O_3}=245gFe_2O_3*\frac{1molFe_2O_3}{159.7gFe_2O_3} =1.54molFe_2O_3[/tex]
Now, as 1 mole of iron (III) oxide is related to 2 moles of iron, due to iron's subscript in the molecule, we get the moles of iron itself:
[tex]n_{Fe}=1.54molFe_2O_3*\frac{2molFe}{1molFe_2O_3} =3.08molFe[/tex]
And the mass is computed based on the atomic mass of iron:
[tex]m_{Fe}=3.08molFe*\frac{55.8gFe}{1molFe} \\\\m_{Fe}=171.7gFe[/tex]
Best regards!
I need help ASAP!! Giving brainliest!
The passenger airship Hindenberg exploded in 1937 while attempting to dock in New Jersey. Its 16 hydrogen filled cells were filled with a total of 200,000 cubic meters of hydrogen gas. Given a density of 0.0824 grams per liter, how many kilograms of hydrogen gas was used to fill the airship?
Answer:
16480 Kg
Explanation:
From the question given above, the following data were obtained:
Volume of Hydrogen = 200000 m³
Density of Hydrogen = 0.0824 g/L
Mass of Hydrogen (in Kg) =?
Next, we shall convert 200000 m³ to L. This can be obtained as follow:
1 m³ = 1000 L
Therefore,
200000 m³ = 200000 m³ × 1000 L / 1 m³
200000 m³ = 2×10⁸ L
Thus, 200000 m³ is equivalent to 2×10⁸ L.
Next, we shall determine the mass of Hydrogen. This can be obtained as follow:
Volume of Hydrogen = 2×10⁸ L
Density of Hydrogen = 0.0824 g/L
Mass of Hydrogen =?
Density = mass /volume
0.0824 = mass of Hydrogen / 2×10⁸
Cross multiply
Mass of Hydrogen = 0.0824 × 2×10⁸
Mass of Hydrogen = 16480000 g
Finally, we shall convert 16480000 g to kg in order to obtain the desired result. This can be obtained as follow:
1000 g = 1 kg
Therefore,
16480000 g = 16480000 g × 1 kg / 1000 g
16480000 g = 16480 Kg
Thus, the mass of Hydrogen used to fill the airship was 16480 Kg
A 2.912 g sample of a compounds containing only C, H, and O was completely oxidized in a reaction that yielded 3.123 g of water and 7.691 g of carbon dioxide. Determine the empirical formula and molecular formula of the compound if it has a molar mass of 100.1 g/mol.
Answer:
Explanation:
18 gram of water contains 2 g of hydrogen
3.123 gram of water will contain 2 x 3.123 / 18 = .347 g of hydrogen .
44 gram of carbon dioxide contains 12 g of carbon
7.691 gram of carbon dioxide will contain 12 x 7.691 / 44 = 2.1 g of carbon .
So the sample will contain 2.912 - ( .347 + 2.1 ) g of oxygen .
= .465 g of oxygen .
moles of Carbon = 2.1 / 12 = .175
moles of hydrogen = .347 / 1 = .347
moles of oxygen = .465 / 16 = .029
Ratio of moles of carbon , oxygen and hydrogen ( C,O,H )
= 0.175 : 0.029 : 0.347
= .175/ .029 : 1 : .347 / .029
= 6 : 1 : 12
So empirical formula = C₆H₁₂O
Let the molecular formula be [tex](C_6H_{12}O)_n[/tex]
molecular weight = n ( 6 x 12 + 12x 1 + 16)
= 100 n
Given 100 n = 100.1
n = 1
Molecular formula = C₆H₁₂O.
In the explosion of a hydrogen-filled balloon, 0.10 g of hydrogen reacted with 0.80 g of oxygen to form how many grams of water vapor? (Water vapor is the only product.)
Express your answer using two significant figures.
Mass of water vapor produced : 0.90 g
Further explanationGiven
0.10 g of hydrogen reacted with 0.80 g of oxygen
Required
mass of water vapor produced
Solution
Reaction
2H₂ + O ⇒ 2H₂O
If we refer to the law of conservation of mass which states that the mass before and after the reaction is the same, then the mass of water vapor formed as a product is:
mass reactants = mass products
mass of Hydrogen + mass of Oxygen = mass of water vapor
0.1 g + 0.8 g = 0.90 g
Or we can also solve by using stochiometry (using the concept of moles) to find the mass of water vapor
compared to sodium, sulfur is more-
A. conductive
B. shiny
C. dull
D. malleable
What must be changed, temperature or heat energy, during condensation explain in 2-3 sentences
Answer:
Change occur in heat energy.
Explanation:
Change occur in the heat energy of molecules during condensation process. The molecules of gas releases its heat energy and converted into liquid state. With this heat energy, they are active and escape from each other but when the heat energy is removed from them, the attractive forces between these gas molecules are formed which convert them into liquid state so change in heat energy occur in the condensation process.
A car is traveling at 8km per hour for 3 hours. What is the distance? 33 km 22 km 24 km 30 km
Answer:24
Explanation:
How many grams of Li3N are produced when 4.7 X 10(23) atoms of lithium react?
Answer:
[tex]m_{Li_3N}=9.06gLi_3N[/tex]
Explanation:
Hello!
In this case, since the reaction between nitrogen and lithium to obtain lithium nitride is:
[tex]6Li+N_2\rightarrow 2Li_3N[/tex]
Starting by that amount of atoms of lithium, we first need to compute the moles of lithium via the Avogadro's number:
[tex]n_{Li}=4.7x10^{23}atoms*\frac{1molLi}{6.022x10^{23}atoms}=0.78molLi[/tex]
Now, by using the 6:2 mole ratio between lithium and lithium nitride and the molar mass of this product (34.83 g/mol), we can compute the required grams as shown below:
[tex]m_{Li_3N}=0.78molLi*\frac{2molLi_3N}{6molLi}*\frac{34.83gLi_3N}{1molLi_3N} \\\\m_{Li_3N}=9.06gLi_3N[/tex]
Best regards!
PLEASE HELP:(((
What kind of reaction is used for electroplating?
O A. A nonspontaneous redox reaction
B. A spontaneous redox reaction
C. A precipitation reaction
D. A decomposition reaction
Explanation:
B.Electroplating involves passing an electric current through a solution called an electrolyte. A redox reaction is spontaneous if the standard electrode potential for the redox reaction is positive
The yttrium- nuclide radioactively decays by electron capture. Write a balanced nuclear chemical equation that describes this process.
Answer:
See explanation and image attached
Explanation:
Yttrium has many isotopes, the lowest mass number of Yttrium is 89Y.
Recall that electron capture converts an electron into a proton and then into a neutron with a consequent emission of a neutrino (v).
In electron capture, the mass number of the daughter nucleus remains the same as that of the parent nucleus while the atomic number of the daughter nucleus is less than that of the parent by one unit.
8. In a blast furnace, iron (III) oxide is used to produce iron by the following (unbalanced) reaction:
Fe2O3 (s) + CO (g) -----> Fe (s) + CO2 (g)
If 4.00 kg Fe2O3 is available to react, how many moles of CO are needed?
How many moles of each product are formed?
Answer:
6
Explanation:
I really need an answer please help
Answer:
56g the time to convey he must take care of the full stops and then try to combine the two sentences that the time to convey
state mandeelev's periodic law explain mandeelev's periodic table with its limitation
Answer: Mendeleev's periodic law : The properties of element are a periodic function of the atomic masses . Limitations:-(1)positions of hydrogen is not correctly placed. (2) The positions of isotopes could not be explained . For ex:- cl35 are cl37 are placed in the same group.
Explanation:
Which property is shared between liquids that are used in thermometers.
Answer:
the property that is shared between liquids us called thermometric property your welcome
Question 4 of 10
Which of the following describes a chemical reaction?
A. Atoms in substances react with each other.
B. Molecules interact without bonds breaking.
C. Substances change shape but not properties.
D. Molecules mix without interacting.
SIR
Answer:
B.
Explanation:
Because one or more substances,the reactants are converted into one or more Different substances,the products. Hope this helps
Sodium Phosphate reacts with calcium nitrate according to the following equation:
2 Na3PO4 + 3 Ca(NO3)2 - Ca3(PO4), + 6 NaNO3
-
If 49.33 grams of sodium phosphate reacts, how many grams of Calcium Phosphate is
produced?
Answer:
Mass = 46.52 g
Explanation:
Given data:
Mass of sodium phosphate react = 49.33 g
Mass of calcium phosphate produced = ?
Solution:
Chemical equation:
2Na₃PO₄ + 3Ca(NO₃)₂ → Ca₃(PO₄)₂ + 6NaNO₃
Number of moles of Na₃PO₄:
Number of moles = mass/molar mass
Number of moles = 49.33 g/ 163.94 g/mol
Number of moles = 0.300 mol
now we will compare the moles of Na₃PO₄ and Ca₃(PO₄)₂
Na₃PO₄ : Ca₃(PO₄)₂
2 : 1
0.300 : 1/2×0.300 = 0.15
Mass of Ca₃(PO₄)₂:
Mass = number of moles × molar mass
Mass = 0.15 mol × 310.14 g/mol
Mass = 46.52 g
Identify each described physical separation technique.
A. A solid mixture is heated. One component transitions directly between solid and gas.
B. A liquid is carefully poured out, leaving the solid behind in the container.
C. A solvent is added to dissolve only one mixture component and then the liquids are separated.
D. A solid is caught on paper or a membrane while the liquid passes through.
Answer:
A. A solid mixture is heated. One component transitions directly between solid and gas ---> Sublimation
B. A liquid is carefully poured out, leaving the solid behind in the container ----> Decantation
C. A solvent is added to dissolve only one mixture component and then the liquids are separated ----> solvent extraction
D. A solid is caught on paper or a membrane while the liquid passes through ---> Filtration using filter paper
Explanation:
A. Sublimation is a process of separating solids which sublimes (solids turning directly to gases) from a a mixture of other solids which do not sublime. When the mixture is heated, the solids which sublime are separated and those which do not are left behind. examples of solids which sublime are naphthalene, Iodine crystals, etc.
B. Decantation is the process of carefully pouring out a liquid from a mixture of it with a solid, leaving the solid behind. Example, a mixture of sand and water where water can be easily decanted, leaving the sand behind.
C. In the process of solvent extraction, a mixture of solids which are soluble in different solvent, one of the components is dissolved in a solvent in which it is soluble while the others are not. The solution is then filtered out and the solid is then separated from the solvent by evaporation.
D. In filtration using a filter paper, the solid-liquid mixture is passed through a filter paper which has pores the size through which liquids can pass through but the solid can not. therefore, the solid remains behind on the paper while the liquid passes through.
A is sublimation, B is decantation, C is solvent extraction, and D is filtration.
Separation of mixturesChemical mixtures are separated in different ways.
A mixture in which one of the components can sublime may be separated using sublimation. The sublime-able component transition from solid straight into gas.A mixture of a liquid plus solid can be decanted if the solid is allowed to settle below the liquid. The liquid can then be decanted off.Solvent extraction has to do with the recovery of a component of a liquid mixture. A solvent is poured into the mixture and the component to be recovered dissolves in the solvent. The liquid is then separated.Filtration is used to separate a mixture consisting of soluble and insoluble components. The insoluble component can be filtered off using a filter paper of suitable pore size.More on separation of mixtures can be found here: https://brainly.com/question/863988
What is the maximum amount in moles of P2O5P2O5 that can theoretically be made from 112 gg of O2O2 and excess phosphorus
Answer:
[tex]n_{P_2O_5}^{max}=1.4molP_2O_5[/tex]
Explanation:
Hello!
In this case, since the reaction between phosphorous and oxygen to form diphosphorous pentoxide is:
[tex]2P+\frac{5}{2}O_2\rightarrow P_2O_5[/tex]
Thus, since phosphorous is in excess and oxygen and diphosphorous pentoxide are in a 5/2:1 mole ratio, we can compute the maximum moles of product as shown below:
[tex]n_{P_2O_5}^{max}=112 gO_2*\frac{1molO_2}{32.00gO_2}*\frac{1molP_2O_5}{5/2molO_2}\\\\ n_{P_2O_5}^{max}=1.4molP_2O_5[/tex]
Best regards!
A mixture of Mg and Zn with a combined mass of 1.0875 g was burned in oxygen producing MgO and ZnO with a combined mass of 1.4090 g. How many grams of zinc was in original mixture
Answer:
0.9537g is the original mass of Zn in the mixture
Explanation:
We can solve this question using the molar mass of each compound involved:
Mg = 24.305g/mol
MgO = 40.304g/mol
Zn = 65.38g/mol
ZnO = 81.38g/mol
Mg-Zn:
1.0875g = 24.305X + 65.38Y (1)
Where X are moles of Mg and Y moles of Zn
MgO-ZnO:
1.4090g = 40.304X + 81.38Y (2)
(1.4090g - 81.38Y) / 40.304 = X
0.03496 - 2.0192Y = X
Replacing (2) in (1)
1.0875g = 24.305(0.03496 - 2.0192Y) + 65.38Y
1.0875 = 0.8497 - 49.077Y + 65.38Y
0.2378 = 16.303Y
0.01459 moles of Zn = Y
And the mass is:
0.01459 moles of Zn * (65.38g/mol) =
0.9537g is the original mass of Zn in the mixtureWrite the quantum numbers of the last electron of Neptunium.
Answer:
Explanation:
quantum number of neptunium is
6
[tex]L_{11/2}[/tex]
