The absolute temperature of a gas is increased four times while maintaining a constant volume. What happens to the pressure
of the gas?
It decreases by a factor of four.
It increases by a factor of four.
It decreases by a factor of eight.
It increases by a factor of eight.

It increases by a factor of four.

Explanation:

To answer this question, we can use the pressure's law, which states that:

"For a constant mass of an ideal gas kept at constant volume, the pressure of the gas is directly proportional to the absolute temperature of the gas"

Mathematically:

where

p is the pressure of the gas

T is its absolute temperature

The equation can be rewritten as

In this problem we have:

, since the absolute temperature of the gas is increased by 4 times

Here we want to find p2; solving for it, we find:

So, the pressure

It increases by a factor of four.

why do the isotopes of a particular element behave differently in nuclear reactions but the same in chemical reactions? chemical reactions involve changes to electrons in an atom; isotopes do not differ in electrons, and so they react the same way during chemical changes.