A gas contained in a steel tank has a pressure of 1.5atm at a temperature of 320K. What will be the gas pressure when the temperature changes to 450K at a constant amount of gas and volume?

2.109 atm

Explanation:

This is Gay-Lussac's Law when the temperature of a sample of gas in a rigid container is increased, the pressure of the gas increases as well. The increase in kinetic energy results in the molecules of gas striking the walls of the container with more force, resulting in a greater pressure. Gay-Lussac's Law states that the pressure of a given mass of gas varies directly with the absolute temperature of the gas, when the volume is kept constant. Gay-Lussac's Law is very similar to Charles's Law, with the only difference being the type of container.

So for this one:

Rearrange it to

P2= (P1 x T2)/T1

P2= (450 x 1.5)/320 = 2.109 atm

chemistry sucks a**

explanation: