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

Explanation:

According to the ideal gas equation, PV = nRT.

where,               P = pressure,                  V = volume

                         n = number of moles,     R = gas constant

                         T = temperature

Since, pressure is inversely proportional to volume. As container B is half in size as compared to container A. Therefore, pressure will increase when gas is added to container B.

Also, there will be more number of collisions between the molecules. Due to this there will be increase in rate of collisions.

Thus, we can conclude that for the given situation if the temperature and moles of gas stay constant during transfer, the rate of collisions will increase and the pressure will also increase.