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I2(s) + HN03(aq) → HI0;(aq) + NO2(g) + A) 1 B) 2 C) 4 D) 10 E) none of the above When the following redox equation is balanced with smalle coefficients, the coefficient for the iodide ion will be I(aq) + NO3 (aq) → NO(g) + 2(s) (acidic A) 2 B) 3 C) 6 D) 8 E) none of the above

I2(s) + HN03(aq) → HI0;(aq) + NO2(g) + A) 1 B) 2 C) 4 D) 10 E) none of the above When the following redox equation is balanced with smalle coefficients, the coefficient for the iodide ion will be I(aq) + NO3 (aq) → NO(g) + 2(s) (acidic A) 2 B) 3 C) 6 D) 8 E) none of the above

Chemistry by OpenStax (2015-05-04)
Chemistry by OpenStax (2015-05-04)
1st Edition
ISBN:9781938168390
Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Chapter17: Electrochemistry
Section: Chapter Questions
Problem 10E: Why is it not possible for hydroxide ion (OH-) to appear in either of the half-reactions or the...
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ANSWER NO. 3 ONLY!

2. When the following redox equation is balanced with smallest whole number coefficients, the coefficient for nitrogen dioxide will be I2(s) + HNO3(aq) → HIO3(aq) + NO2(g) + H2O(!) A) 1 B) 2 C) 4 D) 10 E) none of the above 3. When the following redox equation is balanced with smallest whole number coefficients, the coefficient for the iodide ion will be I(aq) + NO3 (aq) → NO(g) + I2(s) (acidic solution) A) 2 B) 3 C) 6 D) 8 E) none of the above
Transcribed Image Text:2. When the following redox equation is balanced with smallest whole number coefficients, the coefficient for nitrogen dioxide will be I2(s) + HNO3(aq) → HIO3(aq) + NO2(g) + H2O(!) A) 1 B) 2 C) 4 D) 10 E) none of the above 3. When the following redox equation is balanced with smallest whole number coefficients, the coefficient for the iodide ion will be I(aq) + NO3 (aq) → NO(g) + I2(s) (acidic solution) A) 2 B) 3 C) 6 D) 8 E) none of the above
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