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# Consider the reaction between N2H4 and N2O4:2 N2H4(g) + ## Problem 68P Chapter 8

Introductory Chemistry | 5th Edition

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Problem 68P

PROBLEM 68P

Consider the reaction between N2H4 and N2O4:

2 N2H4(g) + N2O4(g) → 3 N2(g) + 4 H2O(g)

A reaction vessel initially contains 27.5 g N2H4 and 74.9 g of N2O4. Calculate the masses of N2H4, N2O4, N2, and H2O that will be in the reaction vessel after the reactants have reacted as much as possible. (Assume 100% yield.)

Step-by-Step Solution:

Solution 68P

Here, we are going to calculate the masses of each reactant after the completion of the reaction.

2 N2H4(g) + N2O4(g) → 3 N2(g) + 4H2O(g)

Step 1:

Molar mass of N2H4(g) = 32.0452 g/mol

Molar mass of N2O4(g) =92.011 g/mol

Step 2:

Determination of the Limiting reagent.

0.858 moles of N2H4 will require 0.429 moles of N2O4

so all the N2H4 will be used up before the N2O4 runs out, the N2H4 is the limiting reactant.

Thus, we know least amount of reactant determines the limiting reagent.

Hence, the limiting reactant is N2H4.

Thus, complete N2H4 is used to form the product

Therefore, Mass of N2H4(g) = 0.0 g

Step 3 of 3

##### ISBN: 9780321910295

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