Question

The following reaction is performed: 3H₂ + N₂ → 2NH₃ . You begin this reaction with 10.00 grams of each reactant. What is the theoretical mass of ammonia (NH₃) that can be formed

Answer 1

The theoretical mass of ammonia is 56.6 grams when reaction is begun with 10.00 grams of each reactant.

Step-by-step explanation:

Data given:

mass of reactants = 10 gram

The reactants are hydrogen and nitrogen gas.

Theoretical mass of ammonia =?

balanced chemical reaction is :

3
`H_(2)` +
`N_(2)` ⇒ 2 N
`H_(3)`

Atomic mass of hydrogen gas = 2 grams/mole

atomic mass of nitrogen gas = 28 grams/mole

number of moles of each reactant is determined:

number of moles =
`(mass)/(atomic mass of 1 mole)`

putting the values for hydrogen gas

number of moles =
`(10)/(2)`

number of moles = 5

number of moles of nitrogen gas =
`(10)/(28)`

= 0.35 moles

from the balanced equation,

3 moles of hydrogen gas reacted to give 2 moles of ammonia

5 moles of hydrogen will give x moles

`(2)/(3)` =
`(x)/(5)`

3x =10

x = 3.33 moles

mass of ammonia produced = number of moles x atomic mass

= 3.33 x 17

= 56.61 grams of ammonia produced from hydrogen

For nitrogen gas,

1 mole nitrogen gas reacted to give 2 moles of ammonia gas

0.35 moles will give x moles

`(2)/(1) =(x)/(0.35)`

x = 0.7 moles of ammonia formed

mass = number of moles x atomic mass

= 0.7 x 17

= 11.9 grams

Thus the limiting reagent is hydrogen gas in the reaction.

The mass from limiting reagent is called theoretical yield = 56.61 grams