Question

During formation of ammonia, what mass of hydrogen gas would be required to react completely

with 42 g of nitrogen gas.​

Answer 1

Answer:-

9g of Hydrogen gas would be required to react completely with 42g of Nitrogen gas.

Explanation:-

Molar mass of Nitrogen gas [N₂] :-

= 14×2

= 28 g/mol

Molar mass of Hydrogen gas [H₂] :-

= 1×2

= 2 g/mol

The balanced chemical equation for the reaction is :-

N₂ + 3H₂ → 2NH₃

From the balanced equation :-

∵ 28g N₂ → 6g H₂

∴ 42g N₂ → 42×6/28 = 9g H₂

Some Extra Information:-

Calculations based on the quantatitve relationship bewteen the reactants and the products are referred to as stoichiometry.

In order to solve problems based on chemical calculations, the steps are :-

(i) Write the balanced chemical equation.

(ii) From the chemical equation write the

molar ratio bewteen given and

required substance.

(iii) Convert these moles into the desired

parameters such as mass and volume.

(iv) Calculate the final result by applying

unitary method.

Answer 2

Explanation:

Answer✍️

9g of Hydrogen gas would be required to react completely with 42g of Nitrogen gas.

Explanation:-

Molar mass of Nitrogen gas [N₂] :-

= 14×2

= 28 g/mol

Molar mass of Hydrogen gas [H₂] :-

= 1×2

= 2 g/mol

The balanced chemical equation for the reaction is :-

N₂ + 3H₂ → 2NH₃

From the balanced equation :-

∵ 28g N₂ → 6g H₂

∴ 42g N₂ → 42×6/28 = 9g H₂

Some Extra Information:-

Calculations based on the quantatitve relationship bewteen the reactants and the products are referred to as stoichiometry.

In order to solve problems based on chemical calculations, the steps are :-

(i) Write the balanced chemical equation.

(ii) From the chemical equation write the

molar ratio bewteen given and

required substance.

(iii) Convert these moles into the desired

parameters such as mass and volume.

(iv) Calculate the final result by applying

unitary method.

hope this helps you!!

thank you ⭐