Under which set of circumstances will the pressure of a gas definitely increase? a) increasing the moles and increasing the volume of the gas. b) raising the temperature and reducing the volume of the gas. c) lowering the temperature and reducing the volume of the gas. d) raising the temperature and increasing the volume of the gas.

Option (B) is the correct answer.

Explanation:

According to the ideal gas equation, pressure times volume equals n times R times temperature.

Mathematically,        PV = nRT

where       P = pressure

                 V = volume

                n = number of moles

                R = gas constant

                T = temperature

Therefore, we can see that pressure is directly proportional to temperature and inversely proportional to volume.

Thus, we can conclude that by raising the temperature and reducing the volume of the gas, the pressure of a gas DEFINITELY increase.

a) the event horizon, singularity, and the chute located between the two.

if i write it on a piece of paper and submit it to you would that be okay

explanation: