# 4. All of the following half-reactions are balanced exceptNO3-(aq) + 4H+(aq) + 3e- = NO(g) + 2H2O(l)H3PO3(aq) + H2O(l) = H3PO4(aq) + 2H+(aq) + 2e-2Ta(s) + 5H2O(l) = Ta2O5(s) +10H+(aq) + 10e-2H2O(l) + 2e- = H2(g) + 2OH-(aq)H2O2(aq) = 2OH-(aq) +2e-

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4. All of the following half-reactions are balanced except

NO3-(aq) + 4H+(aq) + 3e- = NO(g) + 2H2O(l)

H3PO3(aq) + H2O(l) = H3PO4(aq) + 2H+(aq) + 2e-

2Ta(s) + 5H2O(l) = Ta2O5(s) +10H+(aq) + 10e-

2H2O(l) + 2e- = H2(g) + 2OH-(aq)

H2O2(aq) = 2OH-(aq) +2e-

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Step 1

A balanced redox reaction equation will have same number of atoms on both sides of the reaction and also a balanced charges on both sides of the reaction.

Step 2

Consider all the given reactions are first, second, third, fourth and fifth reaction in the same given order.

In the first reaction equation, the number of Nitrogen, oxygen and hydrogen atoms on both sides are balanced.  Also, the number of positive and negatives charges present on the reactant side are also balanced. Therefore, charge on both the reactant and product side remains neutral.  Hence, it is a balanced half-reaction.

Step 3

In the second reaction equation, the number of hydrogen, phosphorus and oxygen atoms on both sides are balanced.  Also, the number of positive and negatives charges present on the product side are also balanced.  Therefore, charge on both the reactant and product side remains neutral.  Hence, it is a balanced half-reaction.

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