A sample of nitrogen gas is contaminated with a gas (gas A) of unknown molar mass. The partial pressure of each gas is known to be 200 torr at 25°C. The gases are allowed to effuse through a pinhole, and it is found that gas A escapes 2.65 times the rate of nitrogen gas. What is the molar mass of gas A?
Thank you for posting your question here at brainly. I hope the answer will help you. Feel free to ask more questions.r(A)/r(N2) = 3 = sqrt(28/x)
so, x = 28/9 = 3.1 approx.
The gas can be H2 (mass = 2), D2 (Mass = 4) or He (Mass =4)
Answer:
Molar mass of gas A is 4.00 g/mol
Explanation:
Rate of effusion (r) is inversely proportional to molecular mass of the gas (M).
Therefore,
\(r \propto \sqrt{\frac{1}{M} } \\or,\ \frac{r_1}{r_2} =\frac{M_2}{M_1}\)
r1 = Rate of effusion of gas A
r2 = Rate of effusion of nitrogen gas
M1 = Molecular formula of gas A
M2 = Molecular formula of nitrogen gas = 28 g/mol
Given:
\(\frac{r_1}{r_2} =2.65\)
substitute the value in the formula,
\(2.65=\sqrt{\frac{28}{M_1}} \\(2.65)^2=\frac{28}{M_1} \\M_1=\frac{28}{7.0025} =3.998 \approx 4.00\ g/mol\)
Molar mass of gas A is 4.00 g/mol