If 4 moles of a gas at a pressure of 5.4 atm have a volume of 230 liters, what is the temperature?

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It is given that 4 moles of the gas at a pressure of 5.4 atm has a volume of 230 liters. It can be assumed that the gas behaves as an ideal gas and as a result the ideal gas law is applicable. This gives P*V = n*R*T where n...

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It is given that 4 moles of the gas at a pressure of 5.4 atm has a volume of 230 liters. It can be assumed that the gas behaves as an ideal gas and as a result the ideal gas law is applicable. This gives P*V = n*R*T where n represents the number of moles of the gas, T represents the temperature, P is the pressure of the gas, V is the volume of the gas and R is a constant equal to 0.082057 L*atm/(K*mole).

Substituting the values given in the question:

5.4*230 = 4*0.082057*T

=> T = 3783 K

The temperature of the gas is 3783 K

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