Multiple Choice
What is the total pressure in a 6.00-L flask which contains 0.127 mol of H2(g) and 0.288 mol of N2(g) at 20.0°C, assuming ideal gas behavior?
7. Gases
The Ideal Gas Law
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What is the volume of total gas at STP (273.15 K and 1 atm) that is produced from the combustion of 1.00 mole of methane gas? Give your answer in liters (L).
A
22.4 L
B
11.2 L
C
44.8 L
D
33.6 L
Verified step by step guidance1
Write the balanced chemical equation for the combustion of methane: CH₄ + 2O₂ → CO₂ + 2H₂O.
Identify the stoichiometry of the reaction: 1 mole of CH₄ produces 1 mole of CO₂ and 2 moles of H₂O, totaling 3 moles of gas products.
Recall that at STP (Standard Temperature and Pressure), 1 mole of an ideal gas occupies 22.4 liters.
Calculate the total volume of gas produced by multiplying the total moles of gas by the volume occupied by 1 mole at STP: 3 moles × 22.4 L/mole.
Conclude by stating that the total volume of gas produced from the combustion of 1.00 mole of methane at STP is the result of the previous calculation.
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