What is the density of nitrogen gas at 740 Torr and-12 $\circ$ C?

Question

Quizplus · Accepted Answer

To solve this problem, we can use the ideal gas law:
PV = nRT
Where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature. Rearranging this equation gives us:
n/V = P/RT
To find the density, we need to divide the number of moles by the volume. The molar mass of nitrogen gas (N2) is 28.02 g/mol, so we can use this to convert between moles and grams. We also need to convert the temperature from Celsius to Kelvin by adding 273.15. Plugging in the values and solving for density gives us:
density = (P * 28.02 g/mol) / (0.08206 L·atm/mol·K * (273.15°C + 1°C))
density = 1.27 g/L
Since the units of the answer choices are given in grams/L, we can see that the correct answer is choice C.

What Is the Density of Nitrogen Gas at 740 Torr ∘\circ∘

What Is the Density of Nitrogen Gas at 740 Torr $\circ$