A sample of methane,CH₄,occupies a volume of 202.0 mL at 25°C and exerts a pressure of 1155.0 mmHg.If the volume of the gas is allowed to expand to 690.0 mL at 298 K,what will be the pressure of the gas? A) 3950 mmHg B) 4030 mmHg C) 338.1 mmHg D) 0.01255 mmHg E) 488.0 mmHg

Question

Quizplus · Accepted Answer

Using the combined gas law, we can relate the initial and final pressures:

(P1V1/T1) = (P2V2/T2)

P2 = (P1V1T2)/(V2T1)

Converting the initial and final temperatures to Kelvin:

T1 = 25°C + 273 = 298 K

T2 = 298 K

Plugging in the given values:

P2 = (1155.0 mmHg * 202.0 mL * 298 K)/(690.0 mL * 298 K)

P2 = 337.9 mmHg

Rounding to the nearest tenth, the answer is C) 338.1 mmHg.

A Sample of Methane,CH4,occupies a Volume of 202

A Sample of Methane,CH₄,occupies a Volume of 202