N2 + 2H2 - -> N2H4

Part 1:

How many grams of hydrazine, N2H4, can be made from 10.66 g of N2 and excess H2?

Part 2:

How many grams of hydrazine, N2H4, can be made from excess N2 and 7.78 g of H2?

Part 3:

How many grams of N2 are required to make 99.69 g of hydrazine? Assume that H2 is in excess.

1. 12.18g of N2H4.

2. 62.24g of N2H4

3. 87.23g of N2

Explanation:

N2 + 2H2 - > N2H4

Molar Mass of N2 = 2x14 = 28g/mol

Molar Mass of N2H4 = (2x14) + (1x4) = 28 + 4 = 32g/mol

Molar Mass of H2 = 2x1 = 2g / mol

Mass conc of H2 from the balanced equation = 2 x 2 = 4g

1. From the balanced equation,

28g of N2 produced 32g N2H4.

Therefore, 10.66 g of N2 will produce = (10.66x32) / 28 = 12.18g of N2H4.

2. From the balanced equation,

4g of H2 produced 32g of N2H4.

Therefore, 7.78 g of H2 will produce = (7.78x32) / 4 = 62.24g of N2H4

3. From the balanced equation,

28g of N2 produced 32g N2H4.

Therefore, Xg of N2 will produce 99.69 g of N2H4 i. e

Xg of N2 = (28x99.69) / 32 = 87.23g