Balance the following reaction in BASIC conditions. Use any method of your choice.  * Show all your steps * MnO4^- (aq) + I^-(aq) --> MnO4^2- (aq) + IO^3- (aq)

Balance the following redox reaction in BASIC conditions. Once you complete the balancing use your workings to answer four questions on this quiz. Mn2+ (aq) + BiO3 → Biš+ (aq) + MnO4 (aq) (aq) In the final balanced BASIC reaction, which statement is true? There is no water in the final balanced reaction There are 7 water molecules on the reactant side There are 7 water molecules on the product side There are 14 water molecules on the reactant side There are 14 water molecules on the reactant side and 7 water molecules on the product side

Balance the following oxidation-reduction reaction as if it were to occur in a basic solution. I (aq) + ClO (aq) – I3 (aq) + Cl-(aq) HOW DO WE GET THERE? Let's balance the oxidation half-reaction first. Which half-reaction correctly balances the elements on both sides? 3 1(aq) → I3 (aq) I(aq) → I3-(aq) I(aq) → 3 I3 (aq) I3 (aq) – I3 (aq) Check Next (2 of 8)

Write balanced half-reactions for the following redox reaction: 1₂(s)+2 NO₂(g) + 2 H₂O(1) → 21 (aq) + 2NO3(aq) + 4H* (aq) reduction: oxidation: 0 ロ→ロ X

Balance the following equation in basic solution using the lowest possible integers and give the coefficient of water. Cr(OH)3{s) + ClO (aq) → CrO4“ (aq) + Cl'(aq) A. 1 B. 4 C.5 O.D.2 OE. 3

Determine if the following reaction is a redox reaction. You evidence from the equation to explain your reasoning. Cu + NO, 3 (aq) - NO (), + Cu²+, (aq)

For the following (potentially unbalanced) reaction, determine what is being (a) reduced and (b) oxidized, (c) write the redox half-reactions, and (d) write a balanced net ionic equation. FeI2(aq) + CuI2(aq) −−→ CuI(s) + FeI3(aq)