🤓 Based on our data, we think this question is relevant for Professor Tang's class at USF.

First, we **set variables** for the moles of each reactant:

We can** add them up to get the total initial moles reactant. **

Next, we **use these variables to express the amount of product** by doing a **mole to mole comparison** using the coefficients of the balanced reaction. The mole products are just the sum of its coefficient per reaction.

A mixture of NH_{3}(g) and N_{2}H_{4}(g) is placed in a sealed container at 320 K . The total pressure is 0.49 atm . The container is heated to 1200 K at which time both substances decompose completely according to the equations 2 NH_{3}(g) → N_{2}(g) + 3 H_{2}(g); N_{2}H_{4}(g) → N_{2}(g) + 2 H_{2}(g). After decomposition is complete the total pressure at 1200 K is found to be 4.5 atm.

Find the percent (by volume) of N_{2}H_{4}(g) in the original mixture. (Assume two significant figures for the temperature.)

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 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 Tang's class at USF.