# 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?
1
2013-05-14T12:01:04-0400
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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