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Problem: Because H2 is completely consumed, it is the limiting reactant. Because some O2 is left over after the reaction is complete, it is the excess reactant. The amount of H2O formed depends on the amount of limiting reactant, H2. If the amount of H2 is doubled, how many moles of H2O would have formed?

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2 H2 + O2  →  2 H2O


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Problem Details


Before the reaction, there are 10 H2 and 7 O2 molecules. After the reaction, there are 10 H2O, 2 O2, and no H2 molecules.


Because H2 is completely consumed, it is the limiting reactant. Because some O2 is left over after the reaction is complete, it is the excess reactant. The amount of H2O formed depends on the amount of limiting reactant, H2. If the amount of H2 is doubled, how many moles of H2O would have formed?

Frequently Asked Questions

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Limiting Reagent concept. If you need more Limiting Reagent practice, you can also practice Limiting Reagent practice problems.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Curtis' class at UNC.