What volume of oxygen gas is required to react completely

Question

Use the following information to answer the next two questions.

1. Hydrogen cyanide is extremely toxic and has been used in chemical warfare. Its main industrial applications are in the mining and refining of gold and silver. Hydrogen cyanide gas can be produced by the following reaction:

2CH₄(g) + 2NH₃(g) + 3O₂(g) → 2HCN(g) + 6H₂O(g)

a) What volume of oxygen gas is required to react completely to produce 340 L of hydrogen cyanide? Assume all reactant and product volumes are measured at 300 kPa and 1200^oC

b) What volume of water vapour will be produced during the production 136 L of hydrogen cyanide? Assume all reactant and product volumes are measured at 300 kPa and 1200^oC.

2. Hydrogen fuel cells are seen as a new, efficient, and clean energy source. Hydrogen combusts according to the reaction:

2H₂(g) + O2(g) → 2H2O(g)

If 60 L of hydrogen reacts with 30 L of oxygen, then the volume of water produced is ________.

3. Hydrogen-powered fuel cells are seen increasingly as “clean” sources of energy and are now used in some vehicles. What volume does a 2.86 mol sample of hydrogen gas occupy at STP?

4. What volume does a 1.26 g sample of chlorine gas occupy at SATP?

5. What mass of helium gas occupies 12.1 L at STP?

6. What volume will 3.51 mol of methane gas occupy at 25.0oC and 111.0 kPa?

7. What is the mass of a 34.3 L sample of carbon dioxide gas at a temperature of 30.0oC and a pressure of 109 kPa?

8. What volume will a 33 g sample of butane gas, C4H10(g), occupy at a temperature of 45.0oC and a pressure of 711 mm Hg?

9. To what temperature, in o C ,must a 20.2 g sample of hydrogen gas be heated to, at 128 kPa, to occupy a volume of 222 L?

10. During a lab experiment, an unknown gas was observed reacting violently when it caused heated steel wool to burst into flames. To help identify the unknown gas, one student suggested they try to determine its molar mass. A 0.5750 g sample of the gas was measured as having a volume of 327.9 mL at 106.3 kPa and 24.00oC . Use this information to calculate the molar mass of the gas. Record your answer to two decimal places.