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.

PV=nRT

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

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What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the The Ideal Gas Law concept. You can view video lessons to learn The Ideal Gas Law. Or if you need more The Ideal Gas Law practice, you can also practice The Ideal Gas Law practice problems.

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Based on our data, we think this problem is relevant for Professor Maxwell's class at UCF.