If you increase the number of moles of gas in a fixed volume container kept as a constant temperature. What happens?
Reason it out.
The ideal gas law is
PV = nRT
If you keep V, R and T constant, then P is proportional to n so larger n values will increase P.
When you increase the number of moles of gas in a fixed volume container kept at a constant temperature, the pressure of the gas increases. This is described by the ideal gas law.
The ideal gas law is given by the equation PV = nRT, where P represents pressure, V represents volume, n represents the number of moles of gas, R is the ideal gas constant, and T represents temperature.
At a constant temperature (T), if the volume (V) remains constant, then the product of pressure (P) and the number of moles (n) is constant as well. This means that if you increase the number of moles of gas, the pressure of the gas must also increase.
To explain this further, let's consider a scenario where you have a fixed volume container with a certain amount of gas. Each gas molecule contributes to the overall pressure in the container by colliding with the container walls. When you increase the number of gas molecules (moles) by adding more gas to the container, there are now more molecules colliding with the walls, resulting in an increase in pressure.
This relationship between the number of moles and pressure is known as Boyle's Law, which states that at a constant temperature, the pressure of a gas is inversely proportional to its volume. Therefore, if the volume is constant, an increase in the number of moles will cause an increase in pressure.
In summary, when you increase the number of moles of gas in a fixed volume container at a constant temperature, the pressure of the gas will increase.