Question

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?

Answer 1

Answer: The pressure of gas will be 1328 Joules

Explanation:

Combined gas law is the combination of Boyle's law, Charles's law and Gay-Lussac's law.

The combined gas equation is,

`(P_1V_1)/(T_1)=(P_2V_2)/(T_2)` (for same value of n)

where,

`P_1` = initial pressure of gas = 1245 J

`P_2` = final pressure of gas = ?

`V_1` = initial volume of gas = 2 L

`V_2` = final volume of gas = 2.5L

`T_1` = initial temperature of gas = 300K

`T_2` = final temperature of gas = 400K

Now put all the given values in the above equation, we get the final pressure of gas.

`(1245* 2)/(300K)=(P_2* 2.5)/(400)`

`P_2=1328J`

Therefore, the final pressure of gas will be 1328 Joules.