A 250.0-mL sample of ammonia, NH_3(g), exerts a pressure of 833 torr at 42.4 deg

Question

A 250.0-mL sample of ammonia, NH_3(g), exerts a pressure of 833 torr at 42.4 degree C. What mass of ammonia is in the container? What is the pressure in a 7.50-L flask if 0.15 mol of carbon dioxide is added to 0.33 mol of oxygen? The temperature of the mixture is 48.0 degree C. If 0.750 L. of argon at 1.50 atm and 177 degree C and 0.235 L of sulfur dioxide at 95.0 kPa and 63.0 degree C are added to a 1.00-L flask and the flask's temperature is adjusted to 25.0 degree C, what is the resulting pressure in the flask? A gas mixture consists of equal masses of methane (molecular weight 16.0) and argon (atomic weight 40.0). If the partial pressure of argon is 200. torr, what is the pressure of methane, in torr?

Explanation / Answer

34. For this problem we'll use the gas eqution

PV = nRT or n = PV/RT

n = mass/molecular weight of ammonia = m /(17gm/mol)

P = pressure of the gas = 833 torr = 1.09605 atmosphere

V = 250ml = .25 liters

R = gas constant = .0821

T = temperature in kelvins = 42.4 degree C = 42.4+273 = 315.4 Kelvins

=> n = PV/RT
m/17 = PV/RT
m = (17*1.09605*.25)/(.0821*315.4) = .1799 grams or .180 grams <==== mass of ammonia in the container

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