Multiple Choice
What is the pressure in mm of Hg of a gas mixture that contains 1g of H2 and 8.0g of Ar in a 3.0 L container at 27°C?
7. Gases
The Ideal Gas Law Applications
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Using the Ideal Gas Law, what is the pressure exerted by a 75.0 g sample of dinitrogen monoxide (N2O) gas in a 4.21 L vessel at 298 K?
A
1.50 atm
B
1.02 atm
C
0.85 atm
D
0.65 atm
Verified step by step guidance1
First, identify the variables given in the problem: the mass of N2O is 75.0 g, the volume of the vessel is 4.21 L, and the temperature is 298 K. We need to find the pressure exerted by the gas.
Convert the mass of N2O to moles using its molar mass. The molar mass of N2O is calculated by adding the atomic masses of nitrogen (14.01 g/mol) and oxygen (16.00 g/mol): Molar mass of N2O = 2(14.01) + 16.00 g/mol.
Use the Ideal Gas Law equation: \( PV = nRT \), where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant (0.0821 L·atm/mol·K), and T is the temperature in Kelvin.
Rearrange the Ideal Gas Law equation to solve for pressure (P): \( P = \frac{nRT}{V} \).
Substitute the values for n (moles of N2O), R (0.0821 L·atm/mol·K), T (298 K), and V (4.21 L) into the equation to calculate the pressure exerted by the gas.
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