The pressure of a sample of CH₄ gas (6.022 g)in a 30.0 L vessel at 402 K is ________ atm.

Question

Quizplus · Accepted Answer

To find the pressure of the gas, we can use the ideal gas law equation: PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant (0.0821 L·atm/(mol·K)), and T is the temperature in Kelvin. First, we need to calculate the number of moles of CH4 gas. The molar mass of CH4 (C = 12.01 g/mol, H = 1.008 g/mol × 4 = 4.032 g/mol) is 16.042 g/mol. The number of moles of CH4 in 6.022 g is 6.022 g / 16.042 g/mol = 0.375 moles. Using the ideal gas law: P = (nRT)/V = (0.375 mol × 0.0821 L·atm/(mol·K) × 402 K) / 30.0 L = 0.413 atm.

The Pressure of a Sample of CH4 Gas (6

The Pressure of a Sample of CH₄ Gas (6