The density of ammonia gas in a 4.32 L container at 837 torr and 45.0 °C is ________ g/L. A)3.86 B)0.719 C)0.432 D)0.194 E)4.22 × 10^-2

Question

Quizplus · Accepted Answer

We can use the ideal gas law to solve for the density of ammonia gas in the given conditions:

PV = nRT

First, we need to convert the pressure to atm:

837 torr = 1.1 atm

Next, we can calculate the number of moles of ammonia using the molar volume:

V = nRT/P

n = PV/RT

n = (1.1 atm)(4.32 L)/(0.0821 L·atm/mol·K)(318 K)

n = 0.179 mol

Finally, we can calculate the density:

density = mass/volume

mass = n × M

where M is the molar mass of ammonia (17.03 g/mol)

mass = (0.179 mol)(17.03 g/mol)

mass = 3.05 g

density = 3.05 g/4.32 L

density = 0.707 g/L

Therefore, the answer is B, 0.719 g/L (rounded to three significant figures).

The Density of Ammonia Gas in a 4