Problem: Consider the following reaction: 3 NO2 (g) + H2O (l) → 2 HNO3 (l) + NO (g) How many moles of NO2(g) are required to react with 1.50 moles of water to produce 4.00 moles of nitric acid? a) Not enough water is available to produce 4.00 moles of nitric acid. b) 8.00 mol c) 3.00 mol d) 6.00 mol e) 1.33 mol 

FREE Expert Solution
85% (409 ratings)
Problem Details

Consider the following reaction:

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

How many moles of NO2(g) are required to react with 1.50 moles of water to produce 4.00 moles of nitric acid?

a) Not enough water is available to produce 4.00 moles of nitric acid.

b) 8.00 mol

c) 3.00 mol

d) 6.00 mol

e) 1.33 mol 

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. 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.

What is the difficulty of this problem?

Our tutors rated the difficulty ofConsider the following reaction: 3 NO2 (g) + H2O (l) → 2 HN...as medium difficulty.

How long does this problem take to solve?

Our expert Chemistry tutor, Jules took 3 minutes and 30 seconds to solve this problem. You can follow their steps in the video explanation above.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Hoeger's class at UCSD.