2. Write the oxidation and reduction half-reaction represented in each of these redox equations. a. PbO(s) + NH3(g) → N2(g) + H2O(1) + Pb(s) b. I2(s) + NaS2O3(aq) → Na2S2O4(aq) + Nal(aq) c. Sn(s) + 2HCl(aq) → SnC12(aq) + H2(g) Reaction PbO(s) + NH3(g) → N2(g) + H2O(1) + Pb(s) 12(s) + NaS203(aq) → Na2S2O4(aq) + Nal(ag) Sn(s) + 2HCl(aq) → SnC12(aq) + H2(g) Oxidation half Reduction half

2. Write the oxidation and reduction half-reaction represented in each of these redox equations. a. PbO(s) + NH3(g) → N2(g) + H2O(1) + Pb(s) b. I2(s) + NaS2O3(aq) → Na2S2O4(aq) + Nal(aq) c. Sn(s) + 2HCl(aq) → SnC12(aq) + H2(g) Reaction PbO(s) + NH3(g) → N2(g) + H2O(1) + Pb(s) 12(s) + NaS203(aq) → Na2S2O4(aq) + Nal(ag) Sn(s) + 2HCl(aq) → SnC12(aq) + H2(g) Oxidation half Reduction half

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

Determine whether or not each reaction is an oxidation and reduction reaction (explain why) For each redox reaction, identify the oxidizing and reducing agents. 1- 2Mg(s) + O2(g) -----> 2MgO(s) 2- 2HBr (aq) + Ca(OH)2(aq) -----> 2H2O(I) + CaBr2 (aq) 3- Zn(s) + Fe2+(aq) -----> Zn2+(aq) + Fe(s)
In the following reaction, which element in what species is reduced? Zn (s) + 2 HCI (aq) – ZnCl, (aq) + H, (g) A) Zn B) H in HCI C) Cl in HCI D) This is not an oxidation/reduction type of reaction.
1. Write oxidation and reduction half-reactions for the unbalanced net redox equations. Show that their sum is the net reaction. (c) Fe³+. (aq) + Cu*(aq) → Fe²* (aq) + Cu²+ (aq)
4. Identify the element oxidized and the element reduced in the first reaction of the lab: Assign oxidation numbers to each element to do this. HNO3(aq) + Cu(s) → Cu(NO3)2(aq) + H2O() + NO2(g)econbyH O biloa eeoubong nollosen abitua Mue () bos
In the following reaction, which species is the reducing agent? ClO3 ^-(aq) + 6 I^- (aq) + 6 H^+(aq) > Cl^- (aq) + 3 I2(s) + 3 H2O (aq) A. ClO3 B. H2O C. H+ D. I-
PART 1: Write the half – reaction of each redox reaction and determine the oxidizing and reducing agent. 1. H2 + F2 → 2HF 2. CO2 + H2O → CsH12O6 + O2 3. MnO2 + Al → Mn +Al2O3 4. Fe2O3 + 3CO → 2Fe + 3CO2 5. NH3 + OCI → N2H4 + H2O + CI
In the following reaction, which element in what species is reduced? Zn (s) + 2 HCI (aq) ZnCl2 (aq) + H2 (g) A) Zn B) H in HCI C) Cl in HCI D) This is not an oxidation/reduction type of reaction.
4. Cu(s) + 2 AgNO,(aq) → Circle one: VOLTAIC / ELECTROLYTIC Substance oxidized: Substance reduced:
Determine whether or not reaction is a redox reaction. For each redox reaction, identify the oxidizing agent and the reducing agent. Pb(NO3)2(aq) + Na2SO4(aq) -------->PbSO4(s) + 2 NaNO3(aq)
PART 1: Write the half - reaction of each redox reaction and determine the oxidizing and reducing agent. 1. H2 + F2 → 2HF 2. CO2 + H2O → C&H12O6 + O2 WRITE YOUR COMPLETE SOLUTION. 3. MnO2 + Al > Mn +Al2O3
Ll.26.
For the following Oxidation/Reduction reactions, show which element is oxidized and which is reduced. 3. Cr2O3 Cr + O2 a. b. CaSO3 + Fe FeSO3 Са с. Sn3N2 Fel3 SnI4 Fe3N2 d. Al2O3 N2 AIN + O2 page 2 + C.