Balance the following redox reaction in acidic solution by inputting the correct coefficients.I- + NO2- → I2 + NO If H+ or H2O is not present as reactant or product, select "0" as the coefficient for the purposes of this question. You must also explicitly label a coefficient as "1" if only one molecule is present.Important: You MUST simplify all "like terms" on both sides of the chemical equation before selecting your answer: having the same compound on both sides of the equation will be marked incorrect. *The products are listed below the reactants so the whole equations fits on your computer screens better * Blank 1 Question 1 I- + Blank 2 Question 1 NO2- + Blank 3 Question 1 H+ + Blank 4 Question 1 H2O ↓Blank 5 Question 1 I2 + Blank 6 Question 1 NO + Blank 7 Question 1 H+ + Blank 8 Question 1 H2O

To balance the given redox reaction, we first need to separate it into two half-reactions, one for oxidation and one for reduction.

The oxidation half-reaction is: I- → I2 The reduction half-reaction is: NO2- → NO

Balancing the oxidation half-reaction: 2I- → I2

Balancing the reduction half-reaction: NO2- + 2H+ + e- → NO + H2O

Now, we need to balance the electrons in the two half-reactions. The oxidation half-reaction needs 2 electrons, while the reduction half-reaction only has 1. Therefore, we multiply the reduction half-reaction by 2 to balance the electrons:

2NO2- + 4H+ + 2e- → 2NO + 2H2O

Now, we can add the two half-reactions together:

2I- + 2NO2- + 4H+ → I2 + 2NO + 2H2O

So, the coefficients for the balanced redox reaction are:

Blank 1: 2 (for I-) Blank 2: 2 (for NO2-) Blank 3: 4 (for H+) Blank 4: 0 (for H2O, as it is not present in the reactants) Blank 5: 1 (for I2) Blank 6: 2 (for NO) Blank 7: 0 (for H+, as it is not present in the products) Blank 8: 2 (for H2O)