Assume that you have a cylinder with a movable piston. What would happen to the gas volume of the cylinder if you were to do the following? (a) Halve the Kelvin temperature while holding the pressure constant

Question

Accepted Answer

Hello everyone today. We were being given the falling problem. Consider a cylinder with a movable piston. How will the volume of the gas in the cylinder change if the temperature in kelvin is doubled at the same time keeping the pressure constant. So the first thing that we want to do is you want to recall our ideal gas law when we have our pressure times. Our volume is equal to the number of moles that we have times of gas constant, R times r temperature. And so according to the problem, our pressure is constant. So we can knock that variable out and we can also assume that the number of moles and the gas constant itself will remain constant, meaning that we are left with our volume equaling our temperature. And so this relationship, what we want to note is that our volume is directly proportional to our temperature, meaning if we have an increase in our volume, we will also have an increase in our temperature. And so we can formulate what that would look like. So, according to the problem, our temperature doubled. This would directly lead to our volume also doubling. And so our final answer will be volume is doubled as well. And with that we have answered the question overall. I hope that this helped and until next time

Assume that you have a cylinder with a movable piston. What would happen to the gas volume of the cylinder if you were to do the following? (a) Halve the Kelvin temperature while holding the pressure constant

Verified Solution

Key Concepts

Ideal Gas Law

Charles's Law

Absolute Temperature