A 1.5 L sample of CCl2F2 (g) is held at 56 torr and 23.5 degrees Celsius.?

Question

If the pressure is increased to 150 torr (temp stays the same), what is the new volume of gas?

In the above system, how many grams of CCl2F2 are in the system?

I figured that the new volume of gas is 0.9 L but since the system changes in pressure, I'm not sure how to solve the second question of the problem.

Roger the Mole · Accepted Answer

(1.5 L) x (56 torr / 150 torr) = 0.56 L
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n = PV / RT = (56 torr) x (1.5 L) / ((62.36367 L torr/K mol) x (23.5 + 273.15) K) = 0.0045405 mol 
(0.0045405 mol) x (120.9135 g CCl2F2/mol) = 0.549 g CCl2F2

DavidB · Answer

the mass of the gas does not change, use the ideal gas equation to find the moles of gas at the original pressure. Then calculate the mass from the moles.

PV = nRT so n = PV/RT

A 1.5 L sample of CCl2F2 (g) is held at 56 torr and 23.5 degrees Celsius.?

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