In oxidation-reduction reactions: Oxidation and reduction reactions can never occur simultaneously The species that is oxidized loses electrons Oxidation is the gain of electrons The species that is reduced loses electrons The charge on the species that is oxidized goes down

In oxidation-reduction reactions: Oxidation and reduction reactions can never occur simultaneously The species that is oxidized loses electrons Oxidation is the gain of electrons The species that is reduced loses electrons The charge on the species that is oxidized goes down

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Which of the following is an oxidation-reduction reaction? O KOH + HNO3 → H₂O + KNO3 O CaCl2 + Na2SO4 → CaSO4 + 2NaCl O AgNO3 + NaCl → AgCl + NaNO3 O N₂ + O2 → 2NO O Al2(SO4)3 + 6KOH → 2Al(OH)3 + 3K2SO4
Consider this reaction: Mn(s) + SnCl2(aq) --> Sn(s) + MnCl2(aq) What is oxidized? What is reduced?
Animation-Analysis of Copper-Zinc Voltaic Cell Zinc Some oxidation-reduction reactions are spontaneous, and the energy released by them can be used for electrical work. This principle is used in the working of a voltaic cell. Voltaic cells, or electrochemical cells, make use of the electrons that are transferred from the species that releases electrons and undergoes oxidation to the species that accepts electrons and undergoes reduction. If it is possible by any means to separate the oxidation reaction and the reduction reaction and then connect them externally so that the electrons flow from one compartment to the other, you can construct an electrochemical cell. Watch the video that describes the cell reaction and the cell components of a voltaic cell. 1.10 14 of 42 Na₂SO₂(aq) Review | Constants | Periodic Table Z 5042 Cu2+ $0,² In a copper-zinc voltaic cell, one half-cell consists of a Zn electrode inserted in a solution of zinc sulfate and the other half-cell consists of a Cu…
Choose all of the statements from below which are true about oxidation and reduction. Ooxidation and reduction are opposite processes with respect to bookkeeping electrons. O Oxidation is what happens when an element in a substance increases its oxidation number. Electrons appear on the right side of an oxidation half reaction. An oxidant is an oxidizing agent, which becomes reduced during the course of a redox reaction. O Reduction is what happens when an element in a substance decreases its oxidation number. Electrons appear on the left side of a reduction half reaction. A reductant is an reducing agent, which becomes oxidized during the course of a redox reaction. K
In the following reaction, what species is the reducing agent?: Ca + Br2 --> CaBr2 Са Br2 This not an oxidation-reduction reaction
Oxidation and reduction occur simultaneously during a reaction.
The oxidation numbers of a redox reaction are not much help in balancing an equation. O True O False
Which of the following is an oxidation reduction (redox) reaction? 1. MgCl2 (aq) + Pb(NO3)2 (aq) = Mg(NO3)2 (aq) + PbCl2(s) 2. 2 Zn (s) + FeCl2 (aq) = Fe (s) + 2 ZnCl2 (aq) 3. 2 H2SO4 (aq) + NaOH (s) = 2H2O (l) + Na2SO4 (aq) 4. Na3PO4 (aq) + FeCl3 (aq) = 3NaCl (aq) + FePO4 (s)
How to tell what element is being oxidized and reduced in a redox reaction with no visible charge in the equation? 2Au(s) + 6HCl(aq) = 2AuCl3(aq) + 3H2(g) 4Fe(s) + 3O2(g) = 2Fe2O3(s)
Calculate the oxidation number for each element within these compounds using algebraic computations. Please show your work. The compounds are : Mg(PO4)2, NaOH, Po4^3-. Don’t forget to include the equation and the calculated oxidation number for each element.
The species in a redox reaction that becomes reduced is the catalyst product reducing agent oxidizing agent
Assign oxidation states to all of the species in the following redox reaction. For the reactants, also identify electron loss or gain, the species oxidized, the species reduced, the oxidizing agent and the reducing agent. Oxidation state Electron gain/loss Oxidized or reduced Reducing or oxidizing agent Mg(s) ♥ ↑ ↑ ♥ + Hg²+ (aq) ♥ ↑ ↑ ♥ Mg2+ (aq) + Hg(1) ◊ Total number of electrons transferred from the reducing agent to the oxidizing agent for the equation given is: