Multiple Choice
At what temperature (in K) would 2.10 moles of N_2 gas exert a pressure of 1.25 atm in a 25.0 L tank? (Use R = 0.0821 L·atm·mol^{-1}·K^{-1})
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7. Gases
The Ideal Gas Law Applications
Multiple Choice
A 6.00 L tank contains 20.0 grams of nitrogen gas (N_2) at a temperature of 385 K. What is the pressure inside the tank? (Use R = 0.0821 L·atm·mol^{-1}·K^{-1})
A
2.60 atm
B
0.98 atm
C
4.10 atm
D
1.85 atm
Verified step by step guidance1
Identify the known quantities: volume (V) = 6.00 L, mass of nitrogen gas (m) = 20.0 g, temperature (T) = 385 K, and the gas constant (R) = 0.0821 L\(\cdot\) atm\(\cdot\) mol^{-1}\(\cdot\) K^{-1}.
Calculate the number of moles (n) of nitrogen gas using its molar mass. The molar mass of N_2 is approximately 28.0 g/mol. Use the formula: \(n = \frac{m}{\text{molar mass}}\).
Apply the ideal gas law equation to find the pressure: \(P V = n R T\). Rearrange to solve for pressure: \(P = \frac{n R T}{V}\).
Substitute the values of n, R, T, and V into the equation to express the pressure in atm.
Perform the calculation to find the pressure inside the tank.
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