**2 NH _{3} _{(g)} + 3 O_{2} _{(g)} + 2 CH_{4} _{(g)} → 2 HCN _{(g)} + 6 H_{2}O _{(g)}**

**the reaction is balanced*

**Determine the limiting reactant (use HCN first):**

molar mass HCN = 27.028 g/mol

**HCN from NH _{3}:**

molar mass NH_{3} = 17.034 g/mol

$\mathbf{mass}\mathbf{}\mathbf{HCN}\mathbf{=}\mathbf{5}\mathbf{.}\mathbf{00}\mathbf{\times}{\mathbf{10}}^{\mathbf{3}}\mathbf{}\overline{)\mathbf{kg}\mathbf{}{\mathbf{NH}}_{\mathbf{3}}}\mathbf{\times}\frac{{\mathbf{10}}^{\mathbf{3}}\mathbf{}\overline{)\mathbf{g}}}{\mathbf{1}\mathbf{}\overline{)\mathbf{kg}}}\mathbf{\times}\frac{\mathbf{1}\mathbf{}\overline{)\mathbf{mol}\mathbf{}{\mathbf{NH}}_{\mathbf{3}}}}{\mathbf{17}\mathbf{.}\mathbf{034}\mathbf{}\overline{)\mathbf{g}\mathbf{}{\mathbf{NH}}_{\mathbf{3}}}}\mathbf{\times}\frac{\mathbf{2}\mathbf{}\overline{)\mathbf{mol}\mathbf{}\mathbf{HCN}}}{\mathbf{2}\mathbf{}\overline{)\mathbf{mol}\mathbf{}{\mathbf{NH}}_{\mathbf{3}}}}\mathbf{\times}\frac{\mathbf{27}\mathbf{.}\mathbf{028}\mathbf{}\mathbf{g}\mathbf{}\mathbf{HCN}}{\mathbf{1}\mathbf{}\overline{)\mathbf{mol}\mathbf{}\mathbf{HCN}}}$

**mass HCN = 7.93x10 ^{6} g HCN**

**HCN from O _{2}:**

molar mass O_{2} = 32.00 g/mol

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

2 NH_{3} _{(g)} + 3 O_{2} _{(g)} + 2 CH_{4} _{(g)} → 2 HCN _{(g)} + 6 H_{2}O _{(g)}

If 5.00 x 10^{3} kg each of NH_{3}, O_{2}, and CH_{4} are reacted, what mass of HCN and of H _{2}O will be produced, assuming 100% yield?

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