Question

The chemistry teacher asked George to transfer an ideal gas from container A to container B. Container B is half the size of container A. If the temperature and moles of gas stay constant during transfer, the rate of collisions will _______________ and the pressure will _______________. A) stay the same; increase B) increase; increase C) increase; decrease Eliminate D) decrease; decrease
Ok because i'm just so dumb at USATESTPREP i'll give 21 points if you help me here. (Brainlyest)

Answer 1

The answer is B) increase, increase

You can work this out mathematically with the equation PV = nRT.
Because volume is halved, the pressure will double, which increases rate of reactions as well.

Answer 2

Answer:The correct answer is option B.

Explanation:

At constant temperature and moles of gas, the pressure exerted by the ideal gas is inversely proportional to the volume occupied by the gas that is Boyle's law.

$Pressure\propto \frac{1}{Volume}$

So, when George transfers an ideal gas from container A to container B with half the volume of container A. With decrease in volume of the container the pressure exerted by an ideal gas will increase as per as Boyle's Law.

And in with increase in pressure the rate of collisions among the particles and with the walls of container will also increase.

If the temperature and moles of gas stay constant during transfer, the rate of collisions will increase and the pressure will increase.