Multiple Choice
What pressure would a gas mixture in a 10.0 L tank exert if it were composed of 48.5 g of He and 94.6 g of CO2 at 398 K, assuming ideal gas behavior?
7. Gases
The Ideal Gas Law
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What is the pressure of a 75.0 g sample of N2O in a 4.12 L vessel at 298 K, assuming ideal gas behavior? (R = 0.0821 L·atm/mol·K)
A
7.89 atm
B
2.34 atm
C
5.67 atm
D
3.45 atm
Verified step by step guidance1
First, determine the molar mass of N2O. The molar mass is calculated by adding the atomic masses of nitrogen (N) and oxygen (O). N2O has two nitrogen atoms and one oxygen atom.
Convert the mass of N2O from grams to moles using the formula: \( \text{moles} = \frac{\text{mass}}{\text{molar mass}} \). Use the molar mass calculated in the previous step.
Use the ideal gas law equation \( PV = nRT \) to solve for pressure (P). Rearrange the equation to \( P = \frac{nRT}{V} \), where n is the number of moles, R is the ideal gas constant, T is the temperature in Kelvin, and V is the volume in liters.
Substitute the known values into the rearranged ideal gas law equation: n (moles of N2O), R (0.0821 L·atm/mol·K), T (298 K), and V (4.12 L).
Calculate the pressure by performing the arithmetic operations in the equation \( P = \frac{nRT}{V} \) to find the pressure in atmospheres.
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