At standard temperature and pressure, 1 mole of an ideal gas occupies how many liters?

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Prepare for the ACS Organic Chemistry Test with multiple choice questions and comprehensive explanations. Utilize flashcards for quick learning and gain confidence for your exam day!

Multiple Choice

At standard temperature and pressure, 1 mole of an ideal gas occupies how many liters?

Explanation:
The concept here is the molar volume of an ideal gas at standard conditions. For one mole at standard temperature and pressure (P = 1 atm, T = 0°C = 273.15 K), the ideal gas law gives V = nRT/P. Using R = 0.082057 L·atm/mol·K, V = (1 mol)(0.082057)(273.15 K) / (1 atm) ≈ 22.4 L. So one mole of an ideal gas at STP occupies about 22.4 liters. (At room temperature, 25°C, the molar volume is around 24.0 L because the temperature is higher.)

The concept here is the molar volume of an ideal gas at standard conditions. For one mole at standard temperature and pressure (P = 1 atm, T = 0°C = 273.15 K), the ideal gas law gives V = nRT/P. Using R = 0.082057 L·atm/mol·K, V = (1 mol)(0.082057)(273.15 K) / (1 atm) ≈ 22.4 L. So one mole of an ideal gas at STP occupies about 22.4 liters. (At room temperature, 25°C, the molar volume is around 24.0 L because the temperature is higher.)

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