# 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?

###### 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 = 7.93x106 g HCN

HCN from O2:

molar mass O2 = 32.00 g/mol

90% (147 ratings) ###### 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?

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Our data indicates that this problem or a close variation was asked in Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition. You can also practice Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition practice problems.