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Solution: A mixture of NH3(g) and N2H4(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 NH3(g) → N2(g) + 3 H2(g); N2H4(g) → N2(g) + 2 H2(g). After decomposition is complete the total pressure at 1200 K is found to be 4.5 atm.Find the percent (by volume) of N2H4(g) in the original mixture. (Assume two significant figures for the temperature.)

Problem

A mixture of NH3(g) and N2H4(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 NH3(g) → N2(g) + 3 H2(g); N2H4(g) → N2(g) + 2 H2(g). After decomposition is complete the total pressure at 1200 K is found to be 4.5 atm.

Find the percent (by volume) of N2H4(g) in the original mixture. (Assume two significant figures for the temperature.)

Solution

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. 

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