Final answer:
Using Boyle's Law, convert the initial pressure to atm, then calculate the final volume (V2) by dividing the product of the initial pressure and volume (P1 * V1) by the final pressure (P2). The gas will occupy a volume of 2.81 L when the pressure is increased to 1.88 atm at constant temperature.
Step-by-step explanation:
The question involves the use of Boyle's Law, which describes the relationship between pressure and volume of a gas at constant temperature. In this case, we are given that a gas at 22°C exhibits a pressure of 754 torr and occupies a volume of 5.32 L. Boyle's Law states that P1 * V1 = P2 * V2, where P1 and V1 are the initial pressure and volume, and P2 and V2 are the final pressure and volume, respectively.
First, we need to convert the pressure from torr to atm since 1 atm = 760 torr. Hence, P1 = 754 torr / 760 torr/atm = 0.992 atm.
Given the final pressure P2 = 1.88 atm, we can rearrange Boyle's Law to solve for the final volume V2: V2 = (P1 * V1) / P2 = (0.992 atm * 5.32 L) / 1.88 atm.
Performing the calculation yields: V2 = 2.81 L. So, when the pressure is increased to 1.88 atm while temperature is held constant, the volume the gas will occupy is 2.81 L.