The molar mass of the given gas is equal to 68.48 g.
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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