If a sample of a gas at 25.2oC has a volume of 536 mL at 0.838 atm, what will its volume be if the pressure is increased to 0.937 atm? A) 477.78 mL B) 563.21 mL C) 503.88 mL D) 613.52 mL

Answers

Answer 1

Answer:

Final answer:

The volume of the gas sample would be 477.78 mL.

Explanation:

The student is asking about the change in volume of a gas sample when the pressure is increased. This can be solved using Boyle's law, which states that the pressure and volume of a gas are inversely proportional at constant temperature. The equation for Boyle's law is: P1 * V1 = P2 * V2

We are given the initial conditions: T1 = 25.2°C, V1 = 536 mL, and P1 = 0.838 atm. We need to find V2 when P2 = 0.937 atm. Using the Boyle's law equation, the volume can be calculated as: V2 = (P1 * V1) / P2

Plugging in the values, we get: V2 = (0.838 atm * 536 mL) / 0.937 atm = 477.78 mL

Therefore, the volume of the gas sample would be 477.78 mL (Option A) when the pressure is increased to 0.937 atm.

Learn more about Boyle's law here:

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Answers

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Answers

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Answers

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Explanation:

Answer:

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Answers

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Answers

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