The pressure, P, of a gas varies directly with its temperature, T, and inversely with its volume, V, according to the equation P=nRT/V, where n is the number of molar units and R is the universal gas constant. One molar unit of gas has a pressure of about 1,245 joules at a temperature of 300 degrees Kelvin and a volume of 2 liters. What is the pressure of the same number of molar units of the gas at a temperature of 400 degrees Kelvin and a volume of 2.5 liters?

Question

Harper Ellis

Mathematics

29 September, 12:52

The pressure, P, of a gas varies directly with its temperature, T, and inversely with its volume, V, according to the equation P=nRT/V, where n is the number of molar units and R is the universal gas constant. One molar unit of gas has a pressure of about 1,245 joules at a temperature of 300 degrees Kelvin and a volume of 2 liters. What is the pressure of the same number of molar units of the gas at a temperature of 400 degrees Kelvin and a volume of 2.5 liters?

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Answers (1)

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Brylee Irwin · Answer 1

To solve this one. let use the formula of the Ideal Gas Law which is P=nRT/V.

Given:

n = 1,245 joules

T = 400 degrees Kelvin

V = 2.5 liters

R = constant

P=?

P=nRT/V

P = (1,245 J) (0.082057 Latm/Kmol) (400K)

2.5 liters

= 40864.386

2.5

= 16345.7544