**Writing the Overall Reaction for a RedOx Reaction in an Acidic Environment** **Reaction:** \[ \text{Cr}_2\text{O}_7^{2-} \text{(aq)} + \text{SnCl}_2 \text{(aq)} + \text{Cl}^- \text{(aq)} \rightarrow \text{Cr}^{3+} \text{(aq)} + \text{SnCl}_4 \text{(aq)} \] **Steps for Writing Half-Cell Reactions and Overall RedOx Reactions:** 1. **Balance Atoms Other Than H and O:** - Adjust coefficients to balance atoms. 2. **Balance Oxygen Atoms:** - Add \(\text{H}_2\text{O}\). 3. **Balance Hydrogen Atoms:** - Add \(\text{H}^+\). 4. **Balance the Charge:** - Add electrons. 5. **Combine Oxidation and Reduction Equations:** - Ensure electrons cancel each other. 6. **Cancel Common Species:** - Eliminate or reduce species appearing on both sides. **Diagrams:** - The diagrams compare and show the step-by-step species involved in the redox reaction. - **First Diagram:** - Represents the reactants: Dichromate ion, Tin (II) chloride, and \(\text{H}^+\). - **Second Diagram:** - Represents the products: Chromium ion and Tin (IV) chloride. For more information, refer to the detailed diagrams included.

Writing the Overall Reaction for a RedOx Reaction in an Acidic Environment Reaction: \[ \text{Cr}_2\text{O}_7^{2-} \text{(aq)} + \text{SnCl}_2 \text{(aq)} + \text{Cl}^- \text{(aq)} \rightarrow \text{Cr}^{3+} \text{(aq)} + \text{SnCl}_4 \text{(aq)} \] Steps for Writing Half-Cell Reactions and Overall RedOx Reactions: 1. Balance Atoms Other Than H and O: - Adjust coefficients to balance atoms. 2. Balance Oxygen Atoms: - Add \(\text{H}_2\text{O}\). 3. Balance Hydrogen Atoms: - Add \(\text{H}^+\). 4. Balance the Charge: - Add electrons. 5. Combine Oxidation and Reduction Equations: - Ensure electrons cancel each other. 6. Cancel Common Species: - Eliminate or reduce species appearing on both sides. Diagrams: - The diagrams compare and show the step-by-step species involved in the redox reaction. - First Diagram: - Represents the reactants: Dichromate ion, Tin (II) chloride, and \(\text{H}^+\). - Second Diagram: - Represents the products: Chromium ion and Tin (IV) chloride. For more information, refer to the detailed diagrams included.

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

21
Suppose the galvanic cell sketched below is powered by the following reaction: Mg(s)+CuCl,(aq) MgCl,(aq)+Cu(s) e- E1 E2 S1 S2 Write a balanced equation for the half-reaction that happens at the cathode of this cellI. O- Write a balanced equation for the half-reaction that happens at the anode of this cell. 0,0. Of what substance is E1 made? Of what substance is E2 made? What are the chemical species in solution S1? What are the chemical species in solution S2?
74. A voltaic cell employs the redox reaction: Sn²+(aq) + Pb(s) Sn(s) + Pb2+(aq) E° cell = 0.010 V Calculate the cell potential, Ecell, at 25°C under each set of conditions. a. [Pb2+] = 0.010 M; [Sn²+] = 0.010 M b. [Pb2+] c. [Pb2+] = = 1.0 × 10 6 M; [Sn²+] = 2.0 M 1.5 M; [Sn2] = 0.010 M
Write the overall reaction for the Redox reaction (below) when it occurs in a basic environment. H3ASO4 (aq) + Zn (s) → AsH3 (1) + Zn²+ (aq) Steps for writing half-cell reactions and overall Redox reactions: 1. Balance atoms other than H and O by changing their coefficients 2. Balance the O's and H's by adding OH and/or H₂O 3. Add electrons to balance the charge 4. Add the Oxidation and Reduction equations once the electrons in each cancel out 5. Cancel out (or reduce to the lowest possible numbers) any other species that are present on both sides of the reaction More Information H3ASO4 + AsH3 Zinc + Zinc ions
Given the standard electrode reduction potentials, which reaction will occur spontaneously?
2.Write a balanced cell reaction. Include the phases of all species in the chemical equation.
A galvanic (voltaic) cell consists of an electrode composed of nickel in a 1.0 M nickel(II) ion solution and another electrode composed of gold in a 1.0 M gold(III) ion solution, connected by a salt bridge. Calculate the standard potential for this cell at 25 °C. Refer to the list of standard reduction potentials. E° V 'cell * TOOLS х10
Consider a galvanic cell based in the reaction Fe2+ + Cr,O,→ Fe³+ + Cr³* . Cr,03- + 14H* + 6e¯ →2Cr+ + 7H,0 1.33 Fe+ + e→ Fe?+ 0.77 Balance the reaction. What is the coefficient of Fe3+ in the balanced equation? а. 3 b. 6 с. 4 d. 2 e. none of these
6. Sketch a voltaic cell for the following overall redox reaction. 3 Cl2(g) + 2 Fe(s) — 6 CІ (аq) + 2 Fe3+(aq) а. Label the anode and cathode b. Indicate the half-reaction occurring at each electrode c. Indicate the species present in each solution.
Zn(s) + 2 H*(aq) → Zn²*(aq) + H2(g) 1. What is the effect on the cell potential of a voltaic cell wi h the above reaction when: The pressure of H2 gas is increased in the cathode. c. Sodium hydroxide is added to the cathode half-cell decreasing the [H"]. а. b. Zinc nitrate is added to the anode d. The surface area of the anode is doubled. half-cell.
Consider the cell diagram: Pb(s)|Pb(NO3)2(aq)||FeCl3(aq)|Fe(s). Write the balanced net-ionic equations for the half-reactions that occur at the two electrodes. a. Anode= b. Cathode=
L. Balance the following Galvanic cell redox reactions and write its cell notation. 1. 2Cro) + 3Cu*(aq)2Cr (aq) +3Cu() 2. 5Fe*(aq) + Mno, (aq) + 8H (aq)- SFe (aq) + Mn (aq) + 4H,O()