What is the density of nitrogen dioxide gas (g/L)contained in a 4.77 L pressure tank at 738.4 mm Hg and 45.0 °C?
A)1.71
B)1300
C)12.1
D)0.0169
E)8.17

Question

Quizplus · Accepted Answer

To find the density of nitrogen dioxide (NO2) gas under the given conditions, we can use the ideal gas law equation rearranged to solve for density ($ \rho $):$$ \rho = \frac{PM}{RT} $$where:- $ P $ is the pressure in atmospheres (atm),- $ M $ is the molar mass of the gas in grams per mole (g/mol),- $ R $ is the ideal gas constant, 0.0821 L·atm/(K·mol),- $ T $ is the temperature in Kelvin (K).First, convert the given pressure from mm Hg to atm:$$ 738.4 \, \text{mm Hg} \times \frac{1 \, \text{atm}}{760 \, \text{mm Hg}} = 0.9716 \, \text{atm} $$Convert the temperature from °C to K:$$ 45.0 \, °C + 273.15 = 318.15 \, K $$The molar mass of NO2 (14.01 g/mol for N + 2 × 16.00 g/mol for O) = 46.01 g/mol.Now, plug the values into the density equation:$$ \rho = \frac{(0.9716 \, \text{atm}) \times (46.01 \, \text{g/mol})}{(0.0821 \, \text{L·atm/(K·mol)}) \times (318.15 \, \text{K})} $$$$ \rho = \frac{44.69 \, \text{g/mol}}{26.11 \, \text{L/mol}} = 1.71 \, \text{g/L} $$Therefore, the density of nitrogen dioxide gas under the given conditions is 1.71 g/L.

What Is the Density of Nitrogen Dioxide Gas (G/L)contained in a 4.77