Question

For a particular sample of an ideal gas, suppose that the pressure is increased. Which of the following is a possible direct result?

Answer 1

1) The number of moles of the gas will increase.
2) The volume of the gas will increase.
3) The universal gas constant will increase.
4) The temperature of the gas will increase.

Answer 2

So think about PV=nRT if you increase pressure which variables will increase and which variables will decrease to keep a constant?

Answer 3

Boyle's law states that the pressure of a gas tends to decrease as volume decreases.
The number of moles of the gas is an independent variable. In other words, pressure would increases if the number of moles of the gas in a container increased as more collision on the walls of the container will produce. If the temperature of a gas increases, gas particles speed up colliding more often with the inner walls of the container.

Answer 4

changing the pressure isn't going to change the number of molecules of the gas you have. that rules out 1. Similarly, the universal gas constant wouldn't be a universal constant if changing the pressure made it change, so that rules out 3.

So, we've established that \[PV = nRT\]and that \(n\) and \(R\) are constant for this problem. If \(P\) increases and \(V\) stays constant, \(T\) must increase. If \(P\) increases and \(V\) increases, \(T\) must increase as well. Only one of those options matches your answer choices.