The density of nitric oxide (NO)gas at 0.970 atm and 34.9 °C is ________ g/L.
A)0.0384
B)0.869
C)1.15
D)0.339
E)10.2

Question

Quizplus · Accepted Answer

We can use the ideal gas law to solve for density:
PV = nRT
n/V = P/RT
density = (P/RT) * molar mass
First, we need to convert the temperature to Kelvin:
34.9 °C + 273.15 = 308.05 K
Next, we can use the molar mass of NO, which is 30.01 g/mol.
Plugging in the values and solving for density:
density = (0.970 atm / (0.08206 L*atm/mol*K * 308.05 K)) * 30.01 g/mol
density = 1.15 g/L

The Density of Nitric Oxide (NO)gas at 0