Question

2. How many grams of N2 are required to produce 10.0 grams of NH3? N2 + 3 H2 - 2 NH3

Answer 1

8.24g

Explanation:

Given parameters;

Mass of NH₃ = 10g

Unknown:

Mass of N₂ = ?

Solution:

  Reaction equation:

               N₂    +    3H₂     →      2NH₃

Step 1: Convert 10.0 g of NH₃ into moles of NH₃

number of moles = $\frac{mass}{molar mass}$

   molar mass of NH₃ = 14 + 3(1) = 17g/mol

 Number of moles = $\frac{10}{17}$  = 0.59mole

Step 2: Convert the moles of NH₃ calculated in Step 1 into moles of N₂

       1 mole of N₂    produced 2 mole of NH₃

   

0.59 moles of ammonia would be formed by $\frac{0.59}{2}$ mole = 0.29mole of N₂

Step 3: Convert the moles of N₂ calculated in Step 2 into grams of N₂.

Mass of N₂ = number of moles x molar mass

  Molar mass of N₂ = 14 x 2 = 28g/mol

  Mass of N₂ = 0.29 x 28 = 8.24g

learn more:

Number of moles brainly.com/question/1841136

#learnwithBrainly