A student collected a sample of a gas in a 165 mL gas bulb until it’s pressure was 765 mm Hg at a temperature of 27.0 Degrees C. If the sample had a mass of 0.452 g, what is the molar mass of the gas?

The ideal gas law can be described as an equation of the state of a hypothetical perfect gas. This equation can be represented as the product of the volume and pressure of one-mole perfect gas is equal to the product of the universal gas constant and absolute temperature of that gas.

The mathematically, ideal gas equation can be written as follows:

PV = nRT

Where n is the moles of gas, P is the pressure, V is the volume of the gas, and R is the gas constant.

Given, the volume of collected gas, V = 165 ml = 0.165 L

The temperature of the gas, T = 27° C = 273 + 27 = 300 K,

The pressure of gas, P = 765 mmHg = 0.99 atm

The value of the gas constant, R = 0.082 atm L /K mol

Substituting the values V, R, P, and T in the equation, we get:

The number of moles of the gas, n = PV/RT

n = 0.99 ×0.165/(0.082 × 300)

n = 0.0066 mol

The molar mass of the gas = 0.452/ 0.0066 =68.48 g/mol

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