Consider the following balanced equation: 2N_2H_4(g) + N_2O_4(g) rightarrow 3N_2

Question

Consider the following balanced equation: 2N_2H_4(g) + N_2O_4(g) rightarrow 3N_2 (g) + 4 H_2O(g) Complete the following table showing the appropriate number of moles of reactants and products. If the number of moles of a reactant is provided, fa in the required amount of the other reactant as well as the moles of each product formed If the number of moles of a product is provided, fill in the required amount of each reactant to make that amount of product, as well as the amount of the other product mat is made.

Explanation / Answer

There is no concept of limiting reagent here... So all we have to do is to give the proportionate answer to the balanced chemical equation given...

Understanding the equation.....

2 moles of N2H2 reacts with 1 mole of N2O4

And gives 3 moles of N2 and 4 moles of H2O

So we have a propotional system of

2:1:3:4

So now all we have to do is substitute values and get corresponding proportional value

Like

1) 4 2 6 8

This means when 4 moles of N2H2 reacts to give products....

It will require 2 moles of N2O4 and will give 6 moles of N2 and 8 moles of H2O

Now you can analyse yourself... I will fill in the blanks

2) 18 9 27 36

3)7 3.5 10.5 14

4)4.5 2.75 8.25 , 11

5)8.4 4.2 12.6 16.8

6) 9.66 4.83 14.5 19.32

Please comment if something is not understood

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