Directions: Using the ideal gas law and stoichiometry, solve the following problems.
PV = nRT
P stands for pressure in atmospheres
V stands for volume in liters
n stands for the number of moles
R stands for the Universal Gas Constant (0.0821 L atm / mol K)
T stands for temperature in Kelvin
K = ºC + 273
760 torr = 760 mmHg = 101.3 kPa = 1 atm
Use the following reaction to answer the questions below:
CH4 (l) + 2 O2 (g) → CO2 (g) + 2 H2O (g)
Problem 1
If 8.00 moles of CH4 are burned, what volume of oxygen is needed if the pressure is 0.957 atm, and the temperature is 68.0°C?
Answer: ________________
Problem 2
How many grams of water would be produced if 16.8 liters of oxygen were burned at a temperature of -31.0°C and a pressure of 1.51 atm?
Answer: ________________
Problem 3
If you burned one gallon of CH4 (approximately 1760 grams), how many liters of carbon dioxide would be produced at a temperature of 15.3°C and a pressure of 1.21 atm?
Answer: ________________
Problem 4
How many liters of oxygen would be needed to produced 26.0 liters of carbon dioxide if the temperature and pressure for both are 37.0°C and 1.99 atm?
Answer: ________________
