MHTCET 23 Apr 2025 Shift 1 Paper

Concept:Boyle's law states that at constant temperature, the pressure of a gas is inversely proportional to its volume.Explanation:Since the volume of the gas is reduced by 5%, we can write:$$V_2 = V_1 - \frac{5}{100}V_1 = \frac{95}{100}V_1 = \frac{19}{20}V_1$$At constant temperature, Boyle's law gives:$$P_1V_1 = P_2V_2$$Substituting the expression for $V_2$ into the equation:$$P_1V_1 = P_2 \times \frac{19}{20}V_1$$Cancelling $V_1$ from both sides of the equation:$$P_1 = \frac{19}{20}P_2$$Solving for $P_2$:$$P_2 = \frac{20}{19}P_1 \approx 1.0526P_1$$The increase in pressure is calculated as:$$P_2 - P_1 = 1.0526P_1 - P_1 = 0.0526P_1$$Thus, the pressure must be increased by 5.26% of the original pressure.Answer:The required increase in pressure is 5.26%.The correct option is C. 5.26%.