A gas occupies 600 mL at a pressure of 900 mmHg. What will be its volume when the pressure is reduced to 750 mmHg, assuming temperature remains constant?

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BlackTom AI · Accepted Answer

We start by identifying the governing principle for this problem: Boyle's Law, which states that for a fixed amount of gas at constant temperature, pressure times volume is constant (P1V1 = P2V2).

Option 1: 720 mL
This value satisfies Boyle's Law with P1 = 900 mmHg, V1 = 600 mL, P2 = 750 mmHg. Calculating V2 = (P1V1)/P2 = (900×600)/750 = 540000/750 = 720 mL. Therefore, this option is numerically correct.

Option 2: 560 mL
If V2 were 560 mL, then P2V2 would be 750×560 = 420,000. But P1V1 equals 540,000, not matching P2V2, so this would violate P1V1 = P2V2. This demonstrates a misapplication or miscalculation of Boyle's Law.

Option 3: 480 mL
A volume of 480 mL would yield P2V2 = 750×480 = 360,000, which again does not equal the initial product 540,000. This shows an inconsistency with the constant-temperature gas law and indicates incorrect use of the relationship.

Option 4: 680 mL
With 680 mL, P2V2 = 750×680 = 510,000, still not matching P1V1 = 540,000. This option fails to satisfy the fundamental equality P1V1 = P2V2 under constant temperature, so it is incorrect.

Overall, only the 720 mL result preserves the product P×V across the pressure change, in accordance with Boyle's Law. The other volumes do not maintain P1V1 = P2V2 and thus are incorrect interpretations.

2254 CHEM 0101 SEC2010 HW 9

A gas occupies 600 mL at a pressure of 900 mmHg. What will be its volume when the pressure is reduced to 750 mmHg, assuming temperature remains constant?

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