The unknown gas has a molar mass of 27.94 g/mol.
<h3>Steps</h3>
Use Graham's Law, which states that the rate of effusion of a gas is proportional to its molar mass squared.
Two different gases, (a) and (b), are compared in the following equation, which expresses this:
(R(a)/R(b)^2 = M(b)/M (a)
The effusion rate is R.
M, the molar mass
If gas (a) is the unknown gas and Xe(M = 131 g/mol) is the second gas, then the answer to your question is:
Square both sides, and you get:
(2.165)² = 131 g/mol/ M (a)
M(a)(2.165)² = 131
M(a) is equal to 131/(2.165)² = 27.94 g/mol.
Thus, the unknown gas has a molar mass of 27.94 g/mol.
<h3>How is molar mass determined?</h3>
Divide each element's atomic weight (found in the periodic table) by the quantity of that element's atoms in the compound. Add up the totals, and then follow the number with the units of grams/mole.
Learn more about Graham's law of effusion here brainly.com/question/22359712
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