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Problem: Hydrogen azide, HN3, decomposes on heating by the following unbalanced equation:HN3(g) → N2(g) + H2(g)If 3.0 atm of pure HN3(g) is decomposed initially, what is the final total pressure in the reaction container? What are the partial pressures of nitrogen and hydrogen gas? Assume the volume and temperature of the reaction container are constant.

FREE Expert Solution

First step is to balance the equation:

HN3(g) → N2(g) + H2(g)

Balance H then N: 

2HN3(g) → 3N2(g) + H2(g)

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Problem Details

Hydrogen azide, HN3, decomposes on heating by the following unbalanced equation:

HN3(g) → N2(g) + H2(g)

If 3.0 atm of pure HN3(g) is decomposed initially, what is the final total pressure in the reaction container? What are the partial pressures of nitrogen and hydrogen gas? Assume the volume and temperature of the reaction container are constant.

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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 Gas Stoichiometry concept. If you need more Gas Stoichiometry practice, you can also practice Gas Stoichiometry practice problems.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor McCauley's class at California State University - Dominguez Hills.

What textbook is this problem found in?

Our data indicates that this problem or a close variation was asked in Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition. You can also practice Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition practice problems.