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# Answer to Question #30027 in Inorganic Chemistry for Ali

Question #30027
if 10.0 g of hydrogen and 75.0 g of oxygen are exploded together in a reaction tube, how much water is produced? What other gas is found in the reaction tube (besides water vapor) after the reaction, and how much of this gas remains?
First, we write the equation for the reaction:

2H2 + O2 = 2H2O
We find the amount of substance of oxygen and hydrogen:
n(H2) = m(H2) / M(H2)
n(H2) = 10g/2g/mol = 5 mol
n(O2) = 75g/32g/mol = 2.34 mol
As seen in excess hydrogen:
the amount of unreacted substance hydrogen = 5 - (2 * 2.34) = 0.3125 mol
m(H2O) = n(H2O) * M(H2O)
Because of a lack of oxygen, it is selected for the calculations:
n(H2O) = 2.34 mol * 2 = 4.68 mol
M(H2O) = 18 g / mol
m(H2O) = 18 g / mol * 4.68 mol = 84.24 g
After reaction, the hydrogen will be:
m(H2) excess = 0.3125 mol * 2 g / vol = 0.625 g

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