Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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Electroplating is a process in which metal ions in solution are deposited as a solid onto another metal, which acts as a conductor for electrons. Electroplating requires an external energy source to provide the electrons that will be captured by the ions to become neutral metal atoms. One species that can be electroplated is platinum.
What quantity of
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- Use the following standard reduction potentials to determine which species is the strongest reducing agent. 2 H+(aq) + 2 e– → H2(g); 0.00 VK+(aq) + e– → K(s); –2.93 V F2(g) + 2 e– → 2 F–(aq); 2.87 VAl3+(aq) + 3 e– → Al(s); –1.66 VPb2+(aq) + 2 e– → Pb(s); –0.13 Varrow_forward7. What is the equilibrium constant, K, at 25°C for this redox reaction under standard conditions? -> 3 Ag(s) + NO¯(aq) + 4 H+(aq) → 3 Ag+(aq) +NO(g) + 2 H2O(l) A. 1.3 × 108 B. 4.8 x 1018 C. 1.9 × 10-2 D. 5.1 x 102 E. 7.6 × 10-9arrow_forwardConsider the following equation in aqueous solution: Cr:0,2 (aq) + S2O3² (aq) → Cr®*(aq) + S.O² (aq) Given that sulfur is oxidized, write the half-reaction for the oxidation in acidic solution. S:0:2-(aq) → S.Oc²-(aq) D2+|03+ 74+ 1 3 5 7 8 9 04 18 Do 5 (s) (1) (g) (aq) + H2O e H+ H H3O+ Reset • x H2O Delete 1L 4.arrow_forward
- 2 H202(aq) -> 2 H2O(I) + O2(g) In the equation above what is the oxidizing agent and what is the reducing agent? Give oxidation numbers of atoms to support your answer.arrow_forwardComplete and balance the following redox reaction in basic solution. Be sure to include the proper phases for all species within the reaction. MnO₄⁻(aq) + C₂O₄²⁻(aq) → MnO₂(s) + CO₂(g)arrow_forwardBalance the following equations. When balancing equations for redox reactions in aqueous solution, it is necessary to add water molecules (H₂O) and either H+ (aq) in acidic solution or OH(aq) in basic solution to the equation. (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank. If needed, use H+ for the hydronium ion.) a. b. Submit Answer 2+ Zn(s) + VO²+ (aq) + + + Ni(s) + CIO¯¯ (aq) Ni(OH)2 (s) + Cl(aq) (basic solution) + → Zn²+ (aq) + V³+ (aq) (acid solution) Retry Entire Group + + + 6 more group attempts remainingarrow_forward
- An acidic solution of permanganate (MnO4–) ions can oxidize nitrous acid to nitrate ions. The products include dissolved Mn2+ ions. Write the chemical equations describing the oxidation of nitrous acid and the reduction of permanganate, and combine the two half-reactions to write a net ionic equation describing the overall redox reaction. Use the lowest whole-number coefficients possible and include states of matter. Define Oxidationarrow_forwardSubstances A, B, and C can all act as oxidizing agents. In solution, A is green, B is yellow, and C is red. In the reactions in which they participate, they are reduced to A−, B−, and C− ions, all of which are colorless. You are given an unknown, colorless, solution that contains one of the following salts: NaA, NaB, NaC. In solution, each salt dissociates completely into the Na+ ion and the anion A−, B−, or C−. The Na+ ion is effectively inert. You are given the availability of solutions of A, B, and C, develop a simple procedure for identifying the salt that is present in your unknown. Question 6 options: React your unknown with NaA, NaB and NaC respectively. If a reaction occurs, your unknown is a better oxidizing agent than what you reacted it with. Use the oxidation strength order calculated in the previous question to determine your unknown. React your unknown with NaA, NaB and NaC respectively. If a reaction occurs, your unknown is a worse…arrow_forwardNn.112. Subject:- Chemistryarrow_forward
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