The absolute temperature of a gas is increased four times while maintaining a constant volume. What happens to the pressure of the gas?

1 Answer
Mar 28, 2017

Answer:

The pressure of the gas also increases by a factor of #4#.

Explanation:

Since there is constant volume, we can use Gay-Lussac's Law:

#P_1/T_1 = P_2/T_2#

The problem tells us that the temperature of the gas is increased by a factor of 4. So, we can make the substitution:

#T_2 = 4T_1#

Now, use this substitution to find #P_2# in terms of #P_1#.

#P_1/T_1 = P_2/T_2#

#P_1/T_1 = P_2/(4T_1) color(white)"XXXX"# substitute #4T_1# for #T_2#

#4P_1 = P_2 color(white)"XXXXX"# multiply both sides by #4T_1#

This means that #P_2# is #4# times #P_1#, so we can say that when the temperature of a gas increases by a factor of #4#, the pressure of the gas also increases by a factor of #4#.

Final Answer