Classify the statements about redox reactions as true or false. True False Answer Bank If there are no changes in the oxidation state of the reactants or products of a particular reaction, that reaction is not a redox reaction. A reducing agent gets oxidized as it reacts. If something is reduced, it is formally losing electrons. If something is oxidized, it is formally losing electrons. In the redox reaction Fe3+ + Co² + Fe2 + + Co³ +, Fe3 + is the reducing agent and Co+ is the oxidizing agent. > Oxidizing agents can convert CO into CO,.

Classify the statements about redox reactions as true or false. True False Answer Bank If there are no changes in the oxidation state of the reactants or products of a particular reaction, that reaction is not a redox reaction. A reducing agent gets oxidized as it reacts. If something is reduced, it is formally losing electrons. If something is oxidized, it is formally losing electrons. In the redox reaction Fe3+ + Co² + Fe2 + + Co³ +, Fe3 + is the reducing agent and Co+ is the oxidizing agent. > Oxidizing agents can convert CO into CO,.

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...

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80°F Sunny The oxidation number of an element can vary. O True Search F8 6725 F9 O False - « Οι F10
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= ly sunny If an ion consists of a single atom, what can be said about the value of the oxidation number of the atom? O 0 smaller than the charge of the ion bigger than the charge of the ion equal to the charge of the ion $ FS 5 O Search 6 FB & 7 F9 ★ 8 Sc ( 9 a 81 0 G
a. In which of the following reactions does the oxidation number of carbon show the greatest increase?A. CH4(g) + 2O2(g) → CO2(g) + 2H2O(l)B. C(s) + O2(g) → CO2(g)C. 2CO(g) + O2(g) → 2CO2(g)D. CO2(g) + Ca(OH)2(aq) → CaCO3(s) + H2O(l) b. In which of the following changes is chlorine reduced?A. HCl to Cl2OB. HCl to HClO3C. Cl− to Cl2D. Cl2 to HCl
7. Write a balanced equation and the net ionic equation for the following reactions: a. An aqueous solution of silver (I) nitrate is added to an aqueous solution of magnesium bromide to produce solid silver (I) bromide and aqueous magnesium nitrate. b. An aqueous solution of copper (II) chloride is added to an aqueous solution of ammonium carbonate to produce solid copper (II) carbonate and aqueous ammonium chloride.
Chemistry write the equation as an ionic equation and ionic equation. write the oxidation numbers of each element in the product and reactant. Tell what is being oxidized and what is being reduced.
Assign oxidation state to the underlined element. 1. Cl2 2. SO2 3. K2O2 4. Cr2O7-2 5. Na2O2
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)
1. Clearly indicate the oxidation number of each element in the reactants and products. Which element is oxidized and which is reduced? H* (ag) + NO2 (ạg) + Al (s) → NH3 (g) + ALO2 lag)
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:
Consider the redox reaction 3 Ni² (aq) + 2 Co(s) → 2 Co³(aq) + 3 Ni(s) Which substance gets oxidized? Ni²+ Ni O Co³+ What is the oxidizing agent? Ni²+ Ni Co Which substance gets reduced? Ο Ni O Co³+ Co O Ni²+ What is the reducing agent? Co³+ Ni Co Ni²+