The density of nitric oxide (NO)gas at 1.21 atm and 46.2°C is __________ g/L.
A)0.0462
B)0.722
C)1.39
D)0.319
E)9.6

Question

Quizplus · Accepted Answer

We can use the ideal gas law, PV=nRT, to solve for the density of NO gas.

First, we need to calculate the number of moles of NO:

PV = nRT

n = PV/RT

n = (1.21 atm)(V) / [(0.0821 L atm/mol K)(46.2°C + 273.15)]

n = (1.21 atm)(V) / (0.0821 L atm/mol K)(319.35 K)

n = 0.0486V

Next, we can calculate the density (d) of NO gas:

d = mass / volume

We can use the molar mass of NO (30.01 g/mol) to relate moles to mass:

mass = n x molar mass

mass = (0.0486V) x (30.01 g/mol)

mass = 1.461V g

Now we can substitute these expressions into the density formula:

d = (1.461V g) / V L

d = 1.461 g/L

Rounded to two decimal places, the answer is 1.39 g/L, which corresponds to choice C.

The Density of Nitric Oxide (NO)gas at 1