Question

For the chemical reaction shown,2 H2O2 (l) + N2H4 (l) => 4H2O(g) + N2 (g)determine how many grams of N2 are produced from the reaction of 8,82 g of H2O2 and 6,81 g of N2H4N2 produced:800TOOLSx10

Answer 1

Step 1

The limiting reactant:

The limiting reactant is the one that is consumed first in a reaction and limits the amount of product produced.

Let's find it!

Write the reaction: 2H2O2 (l) + N2H4 (l) => 4H2O(g) + N2 (g) (balanced)

We also need the molar masses of H2O and N2H4

For H2O) 18 g/mol

For N2H4) 32 g/mol

Procedure:

2 x 18 g H2O ------ 1 x 32 g N2H4

8.82 g H2O ------- X = 7.84 g N2H4

(you can analyze it with 6.81 g of N2H4 too)

For 8.82 g of H2O, 7.84 g of N2H4 are needed, but we have 6.81 g, therefore N2H4 is the limiting reactant.

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Step 2

The limiting reactant: N2H4

We also need the molar mass of N2 => 28 g/mol

1 x 32 g N2H4 -------- 1 x 28 g N2

6.81 g N2H4 -------- X = 5.96 g approx.

Answer: 5.96 g of N2 produced