What is the density of NO(g) at 25.0°C and 783 mmHg?

Question

Quizplus · Accepted Answer

To find the density of NO(g) at 25.0°C and 783 mmHg, we can use the ideal gas law in the form of the density equation: $\rho = \frac{PM}{RT}$, where $\rho$ is the density, $P$ is the pressure in atm, $M$ is the molar mass in g/mol, $R$ is the ideal gas constant (0.0821 L·atm/K·mol), and $T$ is the temperature in Kelvin. First, convert 25.0°C to Kelvin (25 + 273.15 = 298.15 K) and 783 mmHg to atm (783 mmHg * 1 atm/760 mmHg = 1.03 atm). The molar mass of NO is 14.01 (N) + 16.00 (O) = 30.01 g/mol. Plugging these values into the equation gives a density of approximately 1.26 g/L.

What Is the Density of NO(g) at 25