Give balanced equations for the reducing reactions of ammonia with chlorine using excess $N H_{3}$ .

4 {N H}_{3} (e x c e s s) + 3 {C l}_{2} \to {6 N H}_{4} C l + N_{2}

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8 {N H}_{3} (e x c e s s) + 2 {C l}_{2} \to {4 N H}_{4} C l + N_{2}

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8 {N H}_{3} (e x c e s s) + 3 {C l}_{2} \to {6 N H}_{4} C l + N_{2}

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4 {N H}_{3} (e x c e s s) + 3 {C l}_{2} \to {3 N H}_{4} C l + N_{2}

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Solution

The correct option is C $8 {N H}_{3} (e x c e s s) + 3 {C l}_{2} \to {6 N H}_{4} C l + N_{2}$
$8 {N H}_{3} (e x c e s s) + 3 {C l}_{2} \to {6 N H}_{4} C l + N_{2}$

This is the correct chemical equation as it follows the law of conservation of mass.

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Similar questions

3 C l_{2} + 8 N H_{3}

⟶

A + B

3 C l_{2} + 4 N H_{3}

⟶

C + D

A

3 C l_{2} + 8 N H_{3}

⟶

A + B

3 C l_{2} + 4 N H_{3}

⟶

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{3 C l}_{2} + {6 O H}^{-} ⟶ {5 C l}^{-} + {C l O}_{3}^{-} + {3 H}_{2} O

C u O + N H_{3} ⟶ C u + H_{2} O + N_{2}

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