The decomposition of hydrogen peroxide is represented by the equation: 2H2O(l) + O2(g) what mass of hydrogen peroxide would be required to produce 22.4dm³ of oxygen at s.t.p? (H = 1, O = 16, molar volume of a gas at s.t.p. = 22.4dm³)
A. 18 g
B. 34 g
C. 36 g
D. 64 g
E. 68 g
Correct Answer:
Option E – 68 g
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![A compound contains 40.0% carbon, 6.7% hydrogen and 53.3% oxygen. If the molar mass of the compound is 180. Find the molecular formula. [H = 1, C = 12, O = 16]](https://erudites.ng/wp-content/plugins/contextual-related-posts/default.png "A compound contains 40.0% carbon, 6.7% hydrogen and 53.3% oxygen. If the molar mass of the compound is 180. Find the molecular formula. [H = 1, C = 12, O = 16]")