Chemistry Volume-Volume Relationships Quiz

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Questions and Answers

What is the volume of 1.25 moles of CO2 produced from 1.25 moles of methane at STP?

50 dm-3

22.4 dm-3

34.4 dm-3

28 dm-3 (correct)

How many moles of oxygen are required for the complete combustion of 2 moles of carbon disulphide (CS2)?

6 moles (correct)

4 moles

2 moles

3 moles

If 900 dm-3 of H2S is completely combusted, what is the volume of SO2 produced?

900 dm-3 (correct)

1350 dm-3

450 dm-3

1800 dm-3

What is the volume of oxygen gas required at STP for burning 900 dm-3 of H2S?

1350 dm-3 Signup and view all the answers

How much volume does 25 moles of CO2 occupy at room temperature and pressure (RTP)?

600 dm-3 Signup and view all the answers

What is the volume of SO2 produced from burning 900 dm-3 of H2S?

900 dm-3 Signup and view all the answers

For the combustion of 25 moles of methane, how many moles of CO2 are produced?

25 moles Signup and view all the answers

What does the mole ratio in a chemical reaction represent?

The number of moles of reactants to products Signup and view all the answers

What is the theoretical yield of SiC when 100 kg of sand is reacted?

66.66 kg Signup and view all the answers

What is the percentage yield of SiC when 51.4 kg is produced?

77.17% Signup and view all the answers

Which of the following separation techniques can lead to a decrease in actual yield if not performed properly?

Filtration Signup and view all the answers

How much SiC can theoretically be produced from 100 kg of sand in the reaction?

60 kg Signup and view all the answers

How many moles of oxygen are present in a volume of 50 dm³ at STP?

2.0 moles Signup and view all the answers

How many moles of oxygen are consumed when 3.5 moles of methanol are burned?

5.25 moles Signup and view all the answers

How many moles of water are produced from the combustion of 3.5 moles of methanol?

4 moles Signup and view all the answers

What is the purpose of determining the empirical formula of a compound?

To determine the combining ratio of atoms Signup and view all the answers

What is the atomic mass contribution of Carbon in glucose (C6H12O6)?

72 g/mol Signup and view all the answers

In the context of determining the empirical formula, which step follows after calculating the percentage of each element?

Mole ratios using atomic masses Signup and view all the answers

If an organic compound yielded 3.002 g of CO2 upon combustion, what is the mass of carbon in that CO2?

1.076 g Signup and view all the answers

What is the percentage of hydrogen in glucose based on its molecular formula?

6.6% Signup and view all the answers

What is represented by the molecular formula of a compound?

The actual number and types of atoms in a molecule Signup and view all the answers

Which step in determining the empirical formula involves dividing by the least number?

Atomic ratios Signup and view all the answers

What is the percentage of oxygen in the compound calculated as 100 − [% of C + % of H]?

46.75% Signup and view all the answers

What is the empirical formula obtained from the mole ratio 2:5:1?

C2H5O Signup and view all the answers

Given a molecular mass of 110.15 g/mol and an empirical formula mass of 55.05 g/mol, what is the value of n used to derive the molecular formula?

2 Signup and view all the answers

In the reaction of hydrogen and oxygen to produce water, what is the limiting reactant when 2 moles of H2 and 1 mole of O2 are present?

H2 Signup and view all the answers

If the empirical formula is C3H3O, what is the molecular formula when n is determined to be 2?

C6H6O2 Signup and view all the answers

Which element is present in the highest percentage in the initial combustion analysis?

Carbon Signup and view all the answers

What is the empirical formula mass calculated for the empirical formula C3H3O?

55.05 g/mol Signup and view all the answers

In the balanced equation 2H2 + O2 → 2H2O, how many grams of water are produced from 2 moles of hydrogen?

18 g Signup and view all the answers

What is the limiting reactant when 20g of Al and 30g of S are used in the reaction 2Al + 3S → Al2S3?

S Signup and view all the answers

How many moles of Al2S3 can be produced from 30g of S?

0.28 Signup and view all the answers

If 0.313 moles of Al are unreacted, what is the mass of Al left after the reaction?

8.45g Signup and view all the answers

What is the mass of the excess reactant Al after the reaction with S?

8.45g Signup and view all the answers

In the reaction 2Al + 6HBr → 2AlBr3 + 3H2, how many moles of Al would react with 9.92 moles of HBr?

2.96 moles Signup and view all the answers

How many moles of Al remain unreacted when 6.44 moles of Al are mixed with HBr?

2.62 moles Signup and view all the answers

What is the molar mass of Al2S3, given the atomic masses of Al=27 and S=32?

150 g/mol Signup and view all the answers

What is the total mass of the product Al2S3 produced when 20g of Al reacts completely?

42g Signup and view all the answers

Study Notes

Volume-Volume Relationship at STP

1 mole of any gas at Standard Temperature and Pressure (STP) occupies 22.4 dm³
Volume of any gas at STP is directly proportional to the number of moles
CO₂ produced by complete combustion of 1.25 moles of CH₄ is 28 dm³

Combustion of Carbon Disulphide

1 mole of CS₂ reacts with 3 moles of O₂ at STP
2 moles of CS₂ reacts with 6 moles of O₂ at STP
The volume of 6 moles of O₂ at STP is 134.4 dm³

Combustion of Hydrogen Sulphide

2 dm³ of H₂S reacts with 3 dm³ of O₂ at STP
900 dm³ of H₂S will react with 1350 dm³ of O₂ at STP
2 dm³ of H₂S produces 2 dm³ of SO₂ at STP
900 dm³ of H₂S will produce 900 dm³ of SO₂ at STP

Combustion of Methane at RTP

1 mole of any gas at Room Temperature and Pressure (RTP) occupies 24 L (dm³)
25 moles of CH₄ combust to produce 25 moles of CO₂
The volume of 25 moles of CO₂ at RTP is 600 dm³

Mole Ratio

Mole ratio indicates the number of moles of reactants and products in a balanced chemical equation
2 moles of CH₃OH react with 3 moles of O₂ to produce 2 moles of CO₂ and 4 moles of H₂O
When 3.5 moles of methanol are burned, 5.25 moles of oxygen are consumed and 7 moles of water are produced

Percentage Composition

Percentage by mass of an element in a compound is calculated by dividing the atomic mass of the element by the molecular mass of the compound and then multiplying by 100
Percentage composition of C₆H₁₂O₆ is 40% for C, 6.6% for H, and 53% for O

Empirical and Molecular Formula

Empirical formula: Simplest whole-number ratio of atoms in a molecule
Molecular formula: Actual number and types of atoms present in a molecule
5 steps for determining empirical formula:
- Element detection
- Mass of each element
- Percentage of each element
- Mole ratio of each element (percentage divided by atomic mass)
- Atomic ratio (mole ratio divided by the smallest mole ratio)

Empirical and Molecular Formula of an Organic Compound

Combustion analysis of an organic compound containing C, H, and O yielded 3.002g CO₂ and 1.640g H₂O
The empirical formula is C₂H₅O
The molecular mass of the compound is 110.15 g/mol, leading to a molecular formula of C₆H₆O₂

Limiting Reagent

Limiting reagent: Reactant that produces the least amount of product and therefore controls the amount of the product formed.
2 moles of H₂ react with 1 mole of O₂ to produce 2 moles of H₂O
In the reaction of 20g Al with 30g S to form Al₂S₃, Sulphur is the limiting reagent
Excess reactant is the reactant present in an amount greater than that required to react completely with the limiting reagent

Percentage Yield

Actual yield: Amount of product obtained in a reaction
Theoretical yield: Amount of product expected to be formed based on the stoichiometry of the reaction
Percentage yield is the ratio of actual yield to theoretical yield multiplied by 100

Thermal Decomposition of KClO₃

The thermal decomposition of 490g of KClO₃ produces 0.223 moles of O₂
The number of molecules of O₂ produced is 1.34 * 10²³ molecules.

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Description

Test your understanding of volume-volume relationships at Standard Temperature and Pressure (STP) in chemical reactions. This quiz encompasses the combustion of various gases including methane, carbon disulphide, and hydrogen sulphide. Evaluate your knowledge on how volumes of gases relate to moles in these reactions.