Most modern automobiles are equipped with air bags which are very effective in reducing the number of traffic fatalities. During a front-end collision, the air bag sensor sends an electric signal that triggers the rapid decomposition of an unknown compound X which releases a large amount of a certain gas. Within a very short period of time, the air bag inflates to protect the driver and passengers from frontal impact.
A 1.00 g sample of X is decomposed to release 507 mL (110 kPa, 18 C) of gas A, which is one of the components of air. The reaction also yields a solid residue. Treatment of the residue with an excess of water produces 172 mL (S.T.P.) of gas B. Determine X.
Attempt:
X
a A
+ b Y
Y + c H
2O
d B
+ e Z
n
A=0.0231mol
n
B=0.0077mol
I also assumed that d=1, so n
y=n
B therefore the molar ration of A and Y produced by the decomposition of X is 3:1. Here I am stuck. What to do now?