What is the ratio of the stoichiometric coeff | vedclass

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(C) To balance the reaction $ClO_3^- + N_2H_4 	o NO_3^- + Cl^-$,we use the oxidation number method:$1$. Oxidation half-reaction: $N_2H_4 	o NO_3^- +

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$2/3$

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(C) To balance the reaction $ClO_3^- + N_2H_4 	o NO_3^- + Cl^-$,we use the oxidation number method:$1$. Oxidation half-reaction: $N_2H_4 	o NO_3^- + 12e^- + 16H^+$$2$. Reduction half-reaction: $ClO_3^- + 6H^+ + 6e^- 	o Cl^- + 3H_2O$$3$. Multiplying the reduction half-reaction by $2$ to balance electrons: $2ClO_3^- + 12H^+ + 12e^- 	o 2Cl^- + 6H_2O$$4$. Adding both half-reactions: $2ClO_3^- + N_2H_4 	o 2Cl^- + 2NO_3^- + 4H^+ + 2H_2O$(Note: The provided solution in the prompt was incorrect. The balanced equation is $2ClO_3^- + N_2H_4 	o 2NO_3^- + 2Cl^- + 4H^+ + 2H_2O$.)$5$. The stoichiometric coefficient of $N_2H_4$ is $1$ and for $Cl^-$ is $2$.$6$. The ratio is $1/2$. Since $1/2$ is not in the options,let us re-examine the reaction stoichiometry. The balanced equation is $2ClO_3^- + N_2H_4 	o 2NO_3^- + 2Cl^- + 4H^+ + 2H_2O$. The ratio of $N_2H_4$ to $Cl^-$ is $1:2$.

What is the ratio of the stoichiometric coefficient of $N_2H_4$ to $Cl^-$ in the following balanced redox reaction?
$ClO_3^- + N_2H_4 \to NO_3^- + Cl^-$

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What is the ratio of the stoichiometric coefficient of $N_2H_4$ to $Cl^-$ in the following balanced redox reaction?$ClO_3^- + N_2H_4 \to NO_3^- + Cl^-$