Enter your answer in the provided box. Crystalline silicon has a cubic structure. The unit cell edge length is 543 pm. The density of the solid is 2.33 g/cm3. Calculate the number of Si atoms in one unit cell. atoms/cell

Answer:

Explanation:

Organic ChemistryOrganic Chemistry It is often known as the 'Chemistry of Life' that deals with the structure, properties and reactions of organic compounds. A study of Organic Chemistry helps students to identify and classify the various naturally occurring compounds and to create one with desired properties and functions.

The branch of chemistry that deals with the structure and properties of naturally occurring molecules is Organic Chemistry.

Chemistry is divided into several branches in which we learn inorganic chemistry, Physical chemistry, analytical chemistry and also organic chemistry. Organic chemistry deals with natural compounds in which we learn about chemical and physical properties of natural compounds and then the structures of organic compounds as well. We study about the formation of different organic compounds and which kind of compounds will be useful in which field.

For example- Alcohols can be used in vehicles, as solvents, it can be used to form many other organic compounds as well.

Aldehydes, Ketones are the organic compounds which has medicinal use and helps in forming other compounds as well.

Therefore, The branch of chemistry that deals with the structure and properties of naturally occurring molecules is Organic Chemistry.

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MgSo4 will be formed

Answer:

223 g O₂

Explanation:

To find the mass of oxygen gas needed, you need to (1) convert moles Al to moles O₂ (via the mole-to-mole ratio from reaction coefficients) and then (2) convert moles O₂ to grams O₂ (via the molar mass). When writing your ratios/conversions, the desired unit should be in the numerator in order to allow for the cancellation of the previous unit. The final answer should have 3 sig figs because the given value (9.30 moles) has 3 sig figs.

4 Al + 3 O₂ ----> 2 Al₂O₃
^         ^

Molar Mass (O₂): 32.0 g/mol

9.3 moles Al          3 moles O₂              32.0 g
-------------------  x  ---------------------  x  --------------------  =  223 g O₂
                              4 moles Al               1 mole

0.139 moles of plutonium are present in a sample containing 8.4 x 10²² atoms of Pt.

The number of moles of a substance can be calculated using the following expression:

no of moles = no of molecules ÷ 6.02 × 10²³

According to this question, 8.4 × 10²² atoms of plutonium are present in the molecule of plutonium.

no of moles = 8.4 × 10²² = 6.02 × 10²³

no of moles = 1.39 × 10-¹

no of moles = 0.139moles

Therefore, 0.139 moles of plutonium are present in a sample containing 8.4 x 10²² atoms of Pt.

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Answer:

Since Beryllium has a larger atomic radius than Sulphur its electrons are not strongly attracted to the nucleus hence lost easily. But Sulphur has a small atomic radius hence electrons are more closely attracted to the nucleus.

What is the empirical formula for the molecular formula given? Molecular formula: C5H12O

The empirical formula for the given molecular formula C₅H₁₂O. As the molecular formula cannot be reduced into simplest ratio, therefore, the empirical formula and the molecular formula are the same.

The empirical formula can be described as the simplest ratio of the number of different atoms present in a compound. The molecular formula of the compound can be described as the actual number of each different atom in a molecule. This formula is generally used and is also a multiple of the empirical formula of a compound.

The empirical formula provides the ratio of the number of atoms of a chemical in a given compound. The percentage composition directly gives the empirical formula of the compound.

The molecular formula can be reduced into the empirical formula of the compound by dividing the subscripts with a number that can provide the smallest ratio of the elements in the compound.

For the given molecular formula, the further simplest or most reduced ratio cannot be possible. Therefore, the empirical formula of the compound will be the same as the molecular formula. Therefore empirical formula of the compound is C₅H₁₂O.

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Answer:

The electron moved up to an energy level and has an energy of 21.72 x 10−19 J.

Explanation:

i know

Answer:

D) The electron moved up to an energy level and has an energy of 21.72 x 10−19 J.

Explanation:

I took the test and got it right.

did anyone able to look up this question

the ratio for the H is 3.9901

Considering the definition of molar mass, the moles of gas used are 10.625 moles.

The molar mass of substance is a property defined as its mass per unit quantity of substance, in other words, molar mass is the amount of mass that a substance contains in one mole.

Natural gas has a molar mass of 16.0 g/mole.

You started out the day with a tank containing 200.0 g of natural gas.  So, you can apply the following rule of three: If by definition of molar mass 16 grams are contained in 1 mole, 200 grams are contained in how many moles?

[tex]amount of moles at the beginning=\frac{200 gramsx1 mole}{16 grams}[/tex]

amount of moles at the beginning= 12.5 moles

At the end of the day, your tank contains 30.0 g of natural gas. So, you can apply the following rule of three: If by definition of molar mass 16 grams are contained in 1 mole, 30 grams are contained in how many moles?

[tex]amount of moles at the end=\frac{30 gramsx1 mole}{16 grams}[/tex]

amount of moles at the end= 1.875 moles

The number of moles used will be the difference between the number of moles used initially and the contents at the end of the day.

moles used= amount of moles at the beginning - amount of moles at the end

moles used= 12.5 moles - 1.875 moles

moles used= 10.625 moles

Finally, the moles of gas used are 10.625 moles.

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Answer:

1. Oxygen - 46.1%

2. Silicon - 28.2%

3. Aluminium - 8.23%

4. Iron - 5.63%

5. Calcium - 4.15%

6. Sodium - 2.36%

7. Magnesium - 2.33%

8. Potassium - 2.09%

9. Titanium - 0.565%

10.Hydrogen -0.140%

Explanation:

please mark me brainlist

Blocks on the periodic table will not list a mass number of elements in this scenario.

This table comprises of elements in order of their atomic number which determines their chemical properties.

It contains the atomic number but however doesn't contain the mass number of the elements.

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Answer:

chemical reactions In our daily environment are

1) Cooking food

2) Photosynthesis

3) rusting

4) painting

5) respiration

6) combustion

7) Electrochemistry (including chemical batteries)

8)Digestion

9)Soap and detergent reactions

10)Acid-base reactions

11) fermentation

12) oxidation

13 ) burning of paper

14) riping of fruits

15) frying egg

16) souring of milk

17) baking

18) heating sugar

19) burning wood

20) rising bread

267.14 gm grams[tex]Fe_2O_3[/tex] would be required to make 187 g Fe.

A balanced equation is an equation for a chemical reaction in which the number of atoms for each element in the reaction and the total charge is the same for both the reactants and the products.

The balanced equation:

Fe₂O₃ + 3 CO ⟶ 3 CO₂ + 2 Fe

We know that the molecular mass of iron-oxide = 160 g/mole.

We know that the molecular mass of iron = 56 g/mole.

From the above reaction, we can say that

1 mole of iron -oxide produces 2 moles of iron

160 gm of iron oxide produce 112 gm of iron

So,

1 gm of iron required 160÷112 =1.42 gram of iron oxide

Therefore,

187 gm of iron required 1.42 x 187 =265.54 of iron oxide.

Therefore 187 gm of iron required 267.14 iron oxide.

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[tex]\quad \huge \quad \quad \boxed{ \tt \:Answer }[/tex]

[tex]\qquad \tt \rightarrow \:2.8 × {10}^{-5}[/tex]

____________________________________

[tex] \large \tt Solution \: : [/tex]

[tex]\qquad \tt \rightarrow \: \dfrac{2.36 \times 10 {}^{ - 2} }{8.4 \times {10}^{2} } [/tex]

[tex]\qquad \tt \rightarrow \: \dfrac{2.36 }{8.4 } \times \cfrac{10 {}^{ - 2} }{10 {}^{2} } [/tex]

[tex]\qquad \tt \rightarrow \: 0.28 \times 10 {}^{ - 2 - 2} [/tex]

[tex]\qquad \tt \rightarrow \: 0.28 \times 10 {}^{ - 4} [/tex]

[tex]\qquad \tt \rightarrow \: 2.8 \times 10 {}^{ - 5} [/tex]

Answered by : ❝ AǫᴜᴀWɪᴢ ❞

Answer:

=> 11. d. Moon

The moon is not a light source because it does not emit its own light.

=> 12. b. The light is refracted.

13. What is the substance produced by a chemical reaction called?

=> b. Product

Answer:

Season 5 lol

Explanation:

Answer:

season 1

Explanation:

the man was shot rip

The earth's mantle will not change in the future because this region is safe from the intervention of human beings.

The transfer of heat and material in the mantle helps us to determine the landscape of Earth. Activity in the mantle moves the plate tectonics, that contributes to volcanoes, seafloor spreading, earthquakes, and building of mountains.

So we can conclude that the earth's mantle will not change in the future because this region is safe from the intervention of human beings.

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Answer:

a) Black

b) Non-magnetic

c) No reaction with carbon disulphide.

d) i don't know sry

But i had to go through my 6th grade notes for this .____.

Mass of hydrate + crucible = 47.29 g

Mass of anhydrous salt = 2.7 g

Molar mass of anhydrous salt CuSO4 = 159.5 g

Given,

mass of empty crucible = 42.45 g

mass of hydrate salt= 4.84 g

mass of crucible after first heating = 46.1 g

mass of crucible after second heating= 45.153 g

mass of crucible after third heating= 45.15 g

so, as per the question we need to find...

Mass of hydrate + crucible = ? g

Mass of anhydrous salt = ? g

Molar mass of anhydrous salt CuSO4 = ? g

∴Mass of hydrate + crucible = 42.45 + 4.48 = 47.29 g

The given salt is in hydrate form, to remove water from this molecule we need to perform heating .

So we are taking the substance into the crucible as it is in less quantity.

Here, we performed heating 3 times and note the weight after every heating.

After this, assume that the water is totally evaporated and the remaining salt is in anhydrous form,

∴ Mass of anhydrous salt = 45.15 - 42.45 = 2.7 g

To find the molar mass of anhydrous salt of CuSO4,

atomic weight of Cu = 63.5 g

atomic weight of S = 32 g

atomic weight of O =16 g

∴ molar mass of anhydrous salt of CuSO4 = 63.5 + 32 + (16 ×3)

                                                                   =159.5 gm

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The enthalpy of combustion of 1 mole of acetylene for the reaction using the information in the table (attached as figure) is - 1,256 kJ/mol

The enthalpy of combustion of a substance is defined as the heat energy given out when one mole of a substance burns completely in oxygen.

Hence, The enthalpy of combustion of 1 mole of acetylene for the reaction using the information in the table is - 1,256 kJ/mol

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Answer: Are people happier if they have more spare time?

Explanation:

Happiness cannot be measured quantitatively.

Answer:

0

Explanation:

they cancel each other out (ex: 1 positive and 1 negative cancels, making it neutral or a charge of 0)

The vapour pressure in the water flask is 23.686 torr.

The pressure of [tex]H_2[/tex] in the flask was 713.514  torr.

Pressure is the [tex]H_2[/tex] exerting in the flask is 688.314 torr

Vapour pressure is a measure of the tendency of a material to change into the gaseous or vapour state, and it increases with temperature.

a.The vapour pressure of water is given by:

[tex]Log_{10} P =A- \frac{B}{C+T}[/tex], where T is in degree Celcius, P is in torr.

For 0-100 degree celcius, A=8.07131, B=1730.63, C=233.426

[tex]Log_{10} P = 8.07131 - \frac{1730.63}{233.426+25} =1.3745[/tex]

As T =25 degree celcius

[tex]P = 10^{1.3745} torr[/tex] =23.686 torr

b.We know that [tex]P_{total} =P_{H_2} + P_{H_2O}[/tex]

[tex]P_{total}[/tex] = Atmospheric pressure

[tex]737.2 torr = P_{H_2} +23.686 torr[/tex]

[tex]P_{H_2} = 713.514 torr[/tex]

c.After there is a leak in the gas collection tube, the amount at pressure due to water vapour remains unchanged as it is a quantity dependent on temperature.

[tex]P_{total} =P_{H_2} + P_{H_2O} + P_{leaking \;air}[/tex]

[tex]737.2 torr = P_{H_2} + 23.686 torr + 25.2 torr[/tex]

[tex]P_{H_2} =688.314 torr[/tex]

For calculating molar mass of any gas:

M= Density X (RT ÷ P)

M= 0.714 g X ([tex]8.314 J mol^{-1}K^{-1}[/tex]273 K ÷ 101325 Pa)

M= 15.994 g/mol = 16 g/mol.

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Answer:

(b)  19.9 moles

Explanation:

To convert from moles Al to moles O₂, you need to multiply the given value by the mole-to-mole ratio of each component. This ratio is constructed via the coefficients in the balanced reaction. The desired unit (moles O₂) should be placed in the numerator to allow for the cancellation of units.

2 Al₂O₃ ----> 4 Al + 3 O₂
                    ^         ^            

26.5 moles Al           3 moles O₂
---------------------  x  ----------------------  =  19.9 moles O₂
                                 4 moles Al

Answer:

alcohol

Explanation:

alcohol thus, C2H5OH

Answer:

'An ion has a non-zero electric charge. A radical has an atom with unfilled electron shells and so is very reactive, but is electrically neutral.'

'Atoms are single neutral particles. Molecules are neutral particles made of two or more atoms bonded together.'

'The primary difference that lies between these organic compounds and inorganic compounds is that organic compounds always have a carbon atom while most of the inorganic compounds do not contain the carbon atom in them.'

Organic and inorganic compounds:

Similarities:::---

1) In both organic and inorganic compound, the elements joining in making compound complete their octet.

2) Organic compound shows isomerism (R/S , E/Z , cis/trans, enantiomers, diastereomers, etc), just as inorganic compound do (Δ/Λ, enantiomers, R/S enantiomers, cis/trans, fac/mer isomers, etc).

3) Organic compound and inorganic compounds can be very active in chemical reactions, e.g. organolithium reagents could be flammable or even pyrophoric (generally stored under 10°C), while inorganic reagents like in this paper are quite rapid...

Differences:::---

1) Organic compound are very long in size so they can make polymer but inorganic compound are not very long but its structure might me complex.

2) The boiling,melting point of organic compound is lass than inorganic compound.

3) Organic compound always contains carbon but inorganic compounds might not.

4) Organic compound

_____________________________

Ion and Radical Atoms:

In some sense they are a bit similar. The main difference is that a neutral radical has no charge imbalance between the protons and electrons, but the cation or anion does.

Ions are written with an explicit charge because of that charge imbalance, but radicals may or may not have an imbalance of charge. Just because a molecule is a radical doesn't mean it's neutral.

For example, if you shoot 2-pentanone with an electron beam for Electron "Impact" Mass Spectroscopy, where you essentially study molecules whose structures break into smaller pieces as a result of interacting with stray electrons to identify the molecules, you get a cationic radical (middle, or far right of the following diagram).

Considering the Charles's law, the sample of carbon dioxide gas will occupy 308.72 mL.

Charles's law establishes the relationship between the temperature and the volume of a gas when the pressure is constant. This law says that the volume is directly proportional to the temperature of the gas: for a given sum of gas at constant pressure, as the temperature increases, the volume of the gas increases and as the temperature decreases, the volume of the gas decreases.

Mathematically, Charles's law states that the ratio between volume and temperature will always have the same value:

[tex]\frac{V}{T} =k[/tex]

Considering an initial state 1 and a final state 2, it is fulfilled:

[tex]\frac{V1}{T1} =\frac{V2}{T2}[/tex]

In this case, you know:

Replacing in Charles's law:

[tex]\frac{250 mL}{298 K} =\frac{V2}{368 K}[/tex]

Solving:

[tex]V2=368 K\frac{250 mL}{298 K}[/tex]

V2= 308.72 mL

Finally, the sample of carbon dioxide gas will occupy 308.72 mL.

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Answer:

310mL

Explanation:

A sample of carbon dioxide gas occupies a volume of 250 mL at 25°C. What volume will it occupy at 95°C?

Use the formula:

V1

T1

=

V2

T2

Temperature conversion: __°C + 273 K