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a 2.1 l flask contains 4.65 g of gas at 1 atm and 27oc, what is the density and molar mass of the gas?

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The ideal gas law, also known as the general gas equation, is an equation of the state of a hypothetical ideal gas.

The ideal gas law states that the product of the pressure and the volume of one gram molecule of an ideal gas is equal to the product of the absolute temperature of the gas and the universal gas constant.

How to calculate molar mass of the gas?

Ideal Gas Equation:

PV = nRT

Knowing that moles, n = m/M, where m is the mass of the gas, and M is the molar mass. We can plug this into the Ideal Gas Equation:

PV=( m / M) RT

Finally, putting the equation in terms of molar mass, we have:

M = mRT / PV

This derivation of the Ideal Gas Equation is useful in determining the molar mass of an unknown gas.

Given:

m = 4.65 g

P = 1 atm

R = 0.0821 L. atm/k. mol

V =2.1 L

T = 270C = 27 + 273 = 300 K

Putting these values in above formula, we get

Hence, M = (4.65 g X 0.0821 L. atm/k. mol X 300 K) / (1 atm x 2.1 L)

              = 114.5295 / 2.1

              = 54.54 g/ mol

Hence molar mass of a gas = 54.54 g/ mol

To know more about ideal gas equation, click on https://brainly.com/question/20348074

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