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Problem: Hydrogen cyanide is produced industrially from the reaction of gaseous ammonia, oxygen, and methane:2 NH3 (g) + 3 O2 (g) + 2 CH4 (g) → 2 HCN (g) + 6 H2O (g)If 5.00 x 103 kg each of NH3, O2, and CH4 are reacted, what mass of HCN and of H 2O will be produced, assuming 100% yield?

🤓 Based on our data, we think this question is relevant for Professor Ratliff's class at USF.

FREE Expert Solution

2 NH3 (g) + 3 O2 (g) + 2 CH4 (g) → 2 HCN (g) + 6 H2O (g)

*the reaction is balanced


Determine the limiting reactant (use HCN first):

molar mass HCN = 27.028 g/mol 


HCN from NH3:

molar mass NH3 = 17.034 g/mol

mass HCN=5.00×103 kg NH3×103 g1 kg×1 mol NH317.034 g NH3×2 mol HCN2 mol NH3×27.028 g HCN1 mol HCN

mass HCN = 7.93x106 g HCN


HCN from O2:

molar mass O2 = 32.00 g/mol

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Problem Details

Hydrogen cyanide is produced industrially from the reaction of gaseous ammonia, oxygen, and methane:

2 NH3 (g) + 3 O2 (g) + 2 CH4 (g) → 2 HCN (g) + 6 H2O (g)

If 5.00 x 103 kg each of NH3, O2, and CH4 are reacted, what mass of HCN and of H 2O will be produced, assuming 100% yield?

Frequently Asked Questions

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Limiting Reagent concept. If you need more Limiting Reagent practice, you can also practice Limiting Reagent practice problems.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Ratliff's class at USF.

What textbook is this problem found in?

Our data indicates that this problem or a close variation was asked in Chemistry: An Atoms First Approach - Zumdahl 2nd Edition. You can also practice Chemistry: An Atoms First Approach - Zumdahl 2nd Edition practice problems.