According to the equation below, how many moles of oxygen are produced by decomposing 36.8 g of hydrogen peroxide(molar mass = 34.0 g/mol)?
2H2O2->2H2O+O2
a. 1.082 mol oxygen
b. 626 mol oxygen
c. 0.541 mol oxygen
d. 2.16 mol oxygen
e. None of these
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To find the number of moles of oxygen produced, we need to use stoichiometry.
The balanced equation shows that 2 moles of hydrogen peroxide decompose to produce 1 mole of oxygen.
First, let's find the number of moles of hydrogen peroxide.
The molar mass of hydrogen peroxide is 34.0 g/mol.
Therefore, 36.8 g of hydrogen peroxide is equal to:
36.8 g * (1 mol/34.0 g) = 1.082 mol
Since the ratio of moles of hydrogen peroxide to moles of oxygen is 2:1, the number of moles of oxygen produced will be half the number of moles of hydrogen peroxide.
So, the number of moles of oxygen produced is:
1.082 mol * (1/2) = 0.541 mol
Therefore, the answer is c. 0.541 mol oxygen.
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