An ideal gas is at a pressure 1.00 times 10^5 N/m^2 in a container of volume 2.0

Question

An ideal gas is at a pressure 1.00 times 10^5 N/m^2 in a container of volume 2.00 m^3. a. If the gas is compressed to a volume of 1.00 m^3, while the temperature remains constant, what will be the new pressure in the gas? b. The gas is then transferred to a new closed container that cannot expand where the pressure is 1.00 times 10^5 N/m^2 at a temperature of 20 degree C. What is the pressure in the gas if its temperature is increased to 60.0 degree C? c. If the gas is then transferred to a closed container of volume 2.00 m^3 and the pressure is 1.00 times 10^5 N/m^2 at a temperature of 20 degree C. Find the number of moles of the ideal gas.

Explanation / Answer

(A) P V = constant

if V is halved then P will be doubled.

P = 2 x 10^5 N/m^2

(B) P / T = constant

1 x 10^5 / (273 + 20) = P / (273 + 60)

P = 1.14 x 10^5 N/m^2

(C) P V = n R T

(1 x 10^5) (2) = n (8.314)(273 + 20)

n = 82.1 mol

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