Determine what redox reaction, if any, occurs (at 25°C) when tin metal (Sn) is added to...
Question 14 5 pts Consider this redox reaction: Sn (s) + 2H+ (aq) + 2 CF (aq) → Sn2+ (aq) + 2 C1 (aq) + H2(g) Which of the following is the reducing agent? Он* O Sn O Sn2
An electrochemical cell uses the redox reaction below. What half-reaction is occurring at the cathode? (5) 2 H+ (aq) + Sn (s) → Sn2+ (aq) + H2 (g) Sn — Sn2+ + 2e 2H* - H2+2e Sn + 2e + H2 Sn + 2e → Sn2+ 2H*+ 2e → H2
Use the data in the table below to calculate the equilibrium constant at 25°C for the reaction: Cl2(g) + Sn(aq) + Sn2+ (aq) + 2C1- (aq) Standard Reduction Potentials at 25°C Sn(aq) + 2e + Sn2+ (aq) E° = -0.14 V Cl2 (g) + 2e + 2C1- (aq) E° = 1.36 V Express your answer to two significant figures. O ALQ O a ?
29. Use the Standard Reduction Potentials table to predict whether the redox reactions below would be spontaneous or nonspontaneous in the forward direction in 1.0 Maqueous solution 25°C. a) Snº+(ag) + Ni(s) → Ni2+(aq) + Sna+(aq) b) H2(g) + 2 OH- (aq) + Ca2+(ag) - Ca(s) + 2 H20 (1)
4. The following balanced redox reaction occurs in voltaic cell at 25°C H2 (g) + 2Ag+ (aq) → 2H* (aq) + 2 Ag (s) 2H+ + 2e → H2 (g) EⓇ = 0.00V Ag (aq) + le → Ag(s) E = +0.80V a. Write the two half-reactions (oxidation and reduction) occurring in the cell. Clearly indicate which reaction shows oxidation and which shows reduction. Clearly indicate which reaction occurs at the anode and which reaction occurs at the cathode. (4...
2. Indicate True or False for the following scenarios and explain if the reaction occurs using “higher than" and "lower than" using the sample table 3. True/False Scenario Justification Silver metal will dissolve in nitric acid, liberating H2 gas. Chromium metal can dissolve in dilute HCI. Oxygen in moist air can oxidize Fe2+ to Fe3+ Tin metal will reduce Co2+, but not Sn4+ 178 Page (intel V IA "ost Lab Questions: To receive full credit, you must SHOW ALL YOUR...
Post Lab Questions: To receive full credit, you must SHOW ALL YOUR WORK!! Use the table of reduction half reactions to answer the following Post-Lab questions: Table 3. Example reduction Reduction Potential Chart half reactions. The easiest to Ce+(aq) + 3e - Ce3+ (aq) reduce is at the top. The more Au3+ (aq) + 3e Au(s) difficult to reduce is at the bottom. Cl2(g) + 2e 2CH(ag) Ag+ (aq) + e- Ag(s) Fe3+ (aq) + e- Fe2+ (aq) AgCl(s) +...
Imagine that the hypothetical elements. A B C and D form the ions A2+, B2, C2, and Dar. The following reactions show the interactions that do or do NOT occur. Use this information to order the species in a reduction half reaction table. D2+ + C → C2+ + D Easiest to Hardest to Reduce Oxidize D2+ + B - No reaction C2+ + A - A2+ + C Hardest to Reduce Easiest to Oxidize st Lab Questions: To receive...
Table 20.1 Half Reaction E°(V). F2 (g) + 2e →2F (aq) +2.87 Cl2 (g) + 2e → 2CV (aq) +1.359 Br2 (1) + 2e → 2Br (aq) +1.065 O2 (g) + 4H+ (aq) + 4e → 2H20 (1)+1.23 Agt te → Ag (s) +0.799 Fe3+ (aq) + € → Fe2+ (aq) +0.771 12 (s) + 2e → 21+ (aq) +0.536 Cu2+ + 2e → Cu(s) +0.34 2H+ + 2e → H2 (g) Pb2+ + 2e → Pb (s) -0.126 Ni2+...
Please help me answer the questions with detailed steps. Thankyou! 19. Determine which of the following pairs of reactants will result in a spontaneous reaction at 25°c. A) I(aq) Fe2+(aq) B) Ag(s) Sn2+(aq) C) Ca(s) Mg2+(aq) D) H2(g)Sn2+(aq) (5) Balance the following redox reaction if it occurs in acidic solution and write the net ionic equation. 21. Ni2+(aq)+NH4+(aq)Ni(s)+ NO3 (aq)