A sample of methane,CH₄,occupies a volume of 318.0 mL at 25°C and exerts a pressure of 1010.0 mmHg.If the volume of the gas is allowed to expand to 770.0 mL at 298 K,what will be the pressure of the gas? A)2440 mmHg B)4970 mmHg C)417.1 mmHg D)0.01727 mmHg E)452 mmHg

Question

Quizplus · Accepted Answer

First, we need to use the ideal gas law formula to find the initial number of moles of methane:

PV = nRT

n = PV/RT

n = (1010.0 mmHg)(318.0 mL)/(62.36 L mmHg K^-1 mol^-1)(298 K)

n = 0.0400 mol

Now, we can use the same formula with the new volume and the same number of moles to find the new pressure:

PV = nRT

P = nRT/V

P = (0.0400 mol)(62.36 L mmHg K^-1 mol^-1)(298 K)/(770.0 mL)

P = 417.1 mmHg

Therefore, the answer is C) 417.1 mmHg.

A Sample of Methane,CH4,occupies a Volume of 318

A Sample of Methane,CH₄,occupies a Volume of 318