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How many moles of NH3 can be produced from 12.0 mol of H2 and excess N2? Express your answer numerically in moles. View Available Hint(s) nothing mol NH3m o l N H 3 Part B How many grams of NH3 can be produced from 4.04 mol of N2 and excess H2. Express your answer numerically in grams. View Available Hint(s) nothing g NH3g N H 3 Part C How many grams of H2 are needed to produce 13.02 g of NH3? Express your answer numerically in grams. View Available Hint(s) nothing g H2g H 2 Part D How many molecules (not moles) of NH3 are produced from 7.62×10−4 g of H2? Express your answer numerically as the number of molecules. View Available Hint(s) nothing moleculesm o l e c u l e s

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Answer:

A) 8.00 mol NH₃

B) 137 g NH₃

C) 2.30 g H₂

D) 1.53 x 10²⁰ molecules NH₃

Explanation:

Let us consider the balanced equation:

N₂(g) + 3 H₂(g) ⇄ 2 NH₃(g)

Part A

3 moles of H₂ form 2 moles of NH₃. So, for 12.0 moles of H₂:

[tex]12.0molH_{2}.\frac{2molNH_{3}}{3molH_{2}} =8.00molNH_{3}[/tex]

Part B:

1 mole of N₂ forms 2 moles of NH₃. And each mole of NH₃ has a mass of 17.0 g (molar mass). So, for 4.04 moles of N₂:

[tex]4.04molN_{2}.\frac{2molNH_{3}}{1molN_{2}} .\frac{17.0gNH_{3}}{1molNH_{3}} =137gNH_{3}[/tex]

Part C:

According to the balanced equation 6.00 g of H₂ form 34.0 g of NH₃. So, for 13.02g of NH₃:

[tex]13.02gNH_{3}.\frac{6.00gH_{2}}{34.0gNH_{3}} =2.30gH_{2}[/tex]

Part D:

6.00 g of H₂ form 2 moles of NH₃. An each mole of NH₃ has 6.02 x 10²³ molecules of NH₃ (Avogadro number). So, for 7.62×10⁻⁴ g of H₂:

[tex]7.62 \times 10^{-4} gH_{2}.\frac{2molNH_{3}}{6.00gH_{2}} .\frac{6.02\times 10^{23}moleculesNH_{3}  }{1molNH_{3}}=1.53\times10^{20}moleculesNH_{3}[/tex]

The moles of NH₃ that can be produced are:

A) 8.00 mol NH₃

B) 137 g NH₃

C) 2.30 g H₂

D) 1.53 x 10²⁰ molecules NH₃

Balanced chemical equation:

N₂(g) + 3 H₂(g) ⇄ 2 NH₃(g)

Part A

3 moles of H₂ form 2 moles of NH₃.

So, for 12.0 moles of H₂: [tex]12*\frac{2}{3} =8[/tex] moles of NH₃

Part B:

1 mole of N₂ forms 2 moles of NH₃. And each mole of NH₃ has a mass of 17.0 g (molar mass).

So, for 4.04 moles of N₂: [tex]4*\frac{2}{3}*\frac{17}{1}=137[/tex] grams of NH₃.

Part C:

According to the balanced equation 6.00 g of H₂ form 34.0 g of NH₃.

So, for 13.02g of NH₃: [tex]13.02*\frac{6}{34}=2.30[/tex] grams of NH₃.

Part D:

6.00 g of H₂ form 2 moles of NH₃. An each mole of NH₃ has 6.02 x 10²³ molecules of NH₃ (Avogadro number).

So, for 7.62×10⁻⁴ g of H₂: [tex]7.62*10^{-4}*\frac{2}{6} *\frac{6.022*10^{23}}{1}= 1.53*10^{20}[/tex] molecules of NH₃.

Find more information about Balanced chemical equation here:

brainly.com/question/15355912

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