Problem: Nitrogen dioxide reacts with water to form nitric acid and nitrogen monoxide according to the equation:3 NO2(g) + H2O(l) → 2 HNO3(l) + NO(g)Suppose that 5 mol NO2 and 1 mol H2O combine and react completely. How many moles of the reactant in excess are present after the reaction has completed?

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Balanced Reaction: 3 NO2(g) + H2O(l) → 2 HNO3(l) + NO(g)

The reactant in excess is the reactant that produces more products.

The reactant producing less of the product is called limiting reactant.

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Problem Details

Nitrogen dioxide reacts with water to form nitric acid and nitrogen monoxide according to the equation:
3 NO2(g) + H2O(l) → 2 HNO3(l) + NO(g)

Suppose that 5 mol NO2 and 1 mol H2O combine and react completely. How many moles of the reactant in excess are present after the reaction has completed?

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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. You can view video lessons to learn Limiting Reagent. Or if you need more Limiting Reagent practice, you can also practice Limiting Reagent practice problems.

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Based on our data, we think this problem is relevant for Professor Shewa's class at Sacramento City College.