Suppose a gas is kept in a closed rigid container if the temperature of the gas increased what happens to its pressure on the container?

Answer 1

Generally, the gas will expand and the pressure will go up. For this question we can refer to the ideal gas law and you can combine it with some thermodynamics later on for things like adiabatic expansions.

The law simply states that pV=nRT

breaking down the terms:

P= pressure in atmospheres

V= volume in L

n= number of moles of the gas that is present

R= 8,314 462 1 joules per kelvin and mole; the units of this are important

T= the temperature in kelvin (add 273,16 to the temperature in degrees Celsius to get this figure)

so rearrange our equation so we can look at pressure

p=nRT/v

plug in the figures for two different temperatures and then you will see the exact change in pressure for your idealised gas.

Answer 2

Since the container cannot expand, the pressure will increase because the increase in temperature increases the kinetic energy of the gas particles, resulting in the particles hitting the inside walls of the container more frequently.

Answer 3

If the temperature of the gas is increased, the average kinetic energy of its molecules also increases, leading to a greater frequency and force of collisions with the container walls. This results in an increase in pressure on the container due to the increased momentum transfer from the gas molecules to the walls.

Answer 4

The pressure will increase.

Answer 5

It goes up.