Question

When dinitrogen pentoxide N2O5 a white solid is heated it decomposes to nitrogen dioxide and oxygen if a sample of N2O5 produces 1.60 gm O2 how many grams of NO2 are formed?

Answer 1

Given - Oxygen produced - 1.6 gram

Decomposition of N2O5 takes place.

Find - Amount of NO2 produced.

Solution - The decomposition reaction is as follows -

2N2O5 --> 4NO2 + O2

Moles of O2 gas - 1.6/16 - 0.1 moles.

1 mole of O2 is produced from 2 moles of dinitrogen pentoxide

0.1 mole of O2 will be produced from - 0.2 moles.

Now, 2 moles of dinitrogen pentoxide produce 4 moles of NO2

0.2 moles of dinitrogen pentoxide will produce - 4/2*0.2

NO2 produced will be - 0.4 moles.

Weight of NO2 produced - 0.4*46

Weight of NO2 produced - 18.4 gram

Thus, grams of NO2 produced are 18.4

Answer 2

Answer:

9.2 grams of NO2

Explanation:

Firstly the balanced equation

2N2O5-----) 4N02(g) +O2

As given by the question a sample of N205

produces 1.6 gm of O2 then

1.6/32=0.05 Mole of O2

so 2 Moles of N2O5 will give 1 mole of O2

hence the ratio is 2:1 the

2/1 × 0.05=0.1 mole of N2O5

then 2 moles of N2O5 will produce 4 moles of NO2 hence

4/2 ×0.1 = 0.2 moles of NO2

since we got the moles of NO2 it will we easy to get the answer in gm

so 0.2 ×46 = 9.2 gm of NO2