The Ideal Gas Law Video Lessons

Concept: Boyle's Law

# Problem: A 250.0-mL sample of ammonia, NH 3(g), exerts a pressure of 833 torr at 42.4 °C. What mass of ammonia is in the container?A. 0.0787 g B. 0.187 g C. 0.804 g D. 17.0 g E. 0.0106 g

###### FREE Expert Solution

We’re being asked to determine the mass of the ammonia gas.

First, we have to calculate the amount of gas in moles using the ideal gas equation.

$\overline{){\mathbf{P}}{\mathbf{V}}{\mathbf{=}}{\mathbf{n}}{\mathbf{R}}{\mathbf{T}}}$

P = pressure, atm
V = volume, L
n = moles, mol
R = gas constant = 0.08206 (L·atm)/(mol·K)
T = temperature, K

Isolate n (number of moles of gas):

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###### Problem Details

A 250.0-mL sample of ammonia, NH 3(g), exerts a pressure of 833 torr at 42.4 °C. What mass of ammonia is in the container?

A. 0.0787 g

B. 0.187 g

C. 0.804 g

D. 17.0 g

E. 0.0106 g