0
You visited us 0 times! Enjoying our articles? Unlock Full Access!
Question

2.9 g of gas at 95C occupied the same volume as 0.184 g of dihydrogen at 17C at the same pressure. What is the molar mass of the gas?

Solution
Verified by Toppr

Let M be the molar mass of the gas.
The number of moles of the gas, n=2.9M.
The volume of the gas is V=nRTP.
V=2.9R×368MP
The number of moles of dihydrogen are n=0.1842=0.092
The volume of dihydrogen gas is =0.092×R×290P.
At same pressure P, the volume of gas is equal to volume of dihydrogen.
0.092R×290=2.9R×368M
M=2.9×3680.092×290=40
Thus, the molar mass of the gas is 40g/mol.

Was this answer helpful?
3
Similar Questions
Q1
2.9 g of gas at 95C occupied the same volume as 0.184 g of dihydrogen at 17C at the same pressure. What is the molar mass of the gas?
View Solution
Q2
3.7 g of a gas at 25 C occupies the same volume as 0.184 g of hydrogen at 17 C and at the same pressure. What is the molar mass of the gas in grams (g)?
View Solution
Q3
3.7 g of a gas at 25 occupied the same volume as 0.184 g of hydrogen at 17C and at the same pressure. What is the molecular mass of the gas?
View Solution
Q4
3.7 g of a gas at 25C occupies the same volume as 0.184 g of hydrogen at 17C at the same pressure. What is the molecular mass of the gas (round off to the nearest integer)?

View Solution
Q5
If 3.7 g of a gas at 25C occupies the same volume as 0.184 g of hydrogen at 17C and at the same pressure, then what is the molecular weight (x×10) of the gas.
View Solution