How many liters of gas is 10.8 grams of nitrogen at 780 mmHg and 38.0 °C?
A)10.1 L
B)1.17 L
C)9.59 L
D)269 L
E)0.353 L

Question

Quizplus · Accepted Answer

We need to use the ideal gas law equation: PV = nRT
where P = pressure, V = volume, n = number of moles, R = gas constant, and T = temperature in Kelvin.

First, we need to convert the temperature to Kelvin: 
T = 38.0 + 273.15 = 311.15 K

Next, we need to calculate the number of moles of nitrogen: 
n = mass/molar mass = 10.8 g / 28.01 g/mol = 0.385 mol

Now we can rearrange the ideal gas law equation to solve for volume: 
V = nRT/P = (0.385 mol)(0.0821 L*atm/mol*K)(311.15 K)/(780 mmHg)(1 atm/760 mmHg) = 9.59 L

Therefore, the answer is C) 9.59 L.

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