Balance each of the following redox reactions occurring in acidic solution. 1. I−(aq)+NO−2(aq)→I2(s)+NO(g) 2. IO3−(aq)+H2SO3(aq)→I2(aq)+SO42−(aq) 3....

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Balance each of the following redox reactions occurring in acidic solution. 1. I−(aq)+NO−2(aq)→I2(s)+NO(g) 2. IO3−(aq)+H2SO3(aq)→I2(aq)+SO42−(aq) 3....

Balance each of the following redox reactions occurring in acidic solution.

1. I−(aq)+NO−2(aq)→I2(s)+NO(g)

2. IO3−(aq)+H2SO3(aq)→I2(aq)+SO42−(aq)

3. NO−3(aq)+Sn2+(aq)→Sn4+(aq)+NO(g)

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Answer 1

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Consider the given reaction, I(a)+NO(a) (s)+NO(g) Write the two half reactions, Oxidation half reaction 21. (aq)-→12 (s)+2e R NO, (aq)+Sn2 (a)>Sn (a)+NO(g) Write the two half reactions Oxidation half reaction, sn. (aq)--Sn4+ (aq) + 2e- eduction half

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Balance each of the following redox reactions occurring in acidic solution. 1. I−(aq)+NO−2(aq)→I2(s)+NO(g) 2. IO3−(aq)+H2SO3(aq)→I2(aq)+SO42−(aq) 3....

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Add Answer to: Balance each of the following redox reactions occurring in acidic solution. 1. I−(aq)+NO−2(aq)→I2(s)+NO(g) 2. IO3−(aq)+H2SO3(aq)→I2(aq)+SO42−(aq) 3....

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Balance each of the following redox reactions occurring in acidic solution. 1. I−(aq)+NO−2(aq)→I2(s)+NO(g) 2. IO3−(aq)+H2SO3(aq)→I2(aq)+SO42−(aq) 3....