Asked by md.

I would really like help for this question ASAP! pleasee! I thank you ahead of time.

The question refers to an experiment using equal volumes of O2 gas and three other gases "X", "Y", "Z", at the same temperature and pressure. If the respective masses are: 02 = 0.96g X = 1.92g "Y" = 0.90g "Z" = 0.48g. The molecular mass of gas "Z" in g is:

a. 1.0
b. 16
c. 32
d. 44
e. 121

Gas "Y" could be which of the following?

a. butane (C4H10)
b. oxygen
c. NO
d. Nitrogen
e. SO2
Answered by DrBob222
Look at PV = nRT
If all of the gases have the same P, V, R, and T, then moles must bae equal. So how many moles oxygen do you have. At STP that is 0.96/32 = 0.03
So 0.03 x molar mass = grams of gas.
Solve for molar mass of each gas.
For Y, calculate the molar mass of each of the answers to see which agrees with the molar mass of gas Y.
There are no AI answers yet. The ability to request AI answers is coming soon!