14. We have EFe+/Fe= -0.440 V and Eag/Ag=0.800 V. a. Calculate the standard cell emf (Excell)...

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14. We have EºFe²+/Fe= -0.440 V and Eag/Ag=0.800 V. a. Calculate the standard cell emf (Excell) of a Galvanic cell that has been constructed from these species. (Show works!). b. Can you use an iron spoon to stir AgNO3 solution? Why? 15. Redox reaction: a. Split the following redox reaction into oxidation half and reduction half reactions, balance the half reactions (both charges and atoms), and write the balanced overall reaction. Cr2O72- + HNO2 + H+ → Cr³+ + NO3 + H₂O b. Identify the oxidant and reductant. c. What is happening to the oxidation number of an element of a redutant, increasing or decreasing? 16. The reaction 2NO(g) + 2H₂(g) →→→ N2(g) + 2H₂O(g) occurs in three steps. Step 1: NO + NO → N2O2 (fast) Step 2: _(slow) Step 3: N₂O + H2 → N2 + H₂O (fast) a. Write the reaction in step 2. b. What is the molecularity in the "rate determining step"? c. Mention two reaction intermediates in this reaction. 17. In the following reaction, the rate becomes nine times when concentration of B is tripled and concentration of A is kept constant. The rate becomes double when concentration of A is doubled and concentration of B is kept constant. A + B → C + D Write the rate law for this reaction. a. 14. We have EºFe²+/Fe= -0.440 V and Eag/Ag=0.800 V. a. Calculate the standard cell emf (Excell) of a Galvanic cell that has been constructed from these species. (Show works!). b. Can you use an iron spoon to stir AgNO3 solution? Why? 15. Redox reaction: a. Split the following redox reaction into oxidation half and reduction half reactions, balance the half reactions (both charges and atoms), and write the balanced overall reaction. Cr2O72- + HNO2 + H+ → Cr³+ + NO3 + H₂O b. Identify the oxidant and reductant. c. What is happening to the oxidation number of an element of a redutant, increasing or decreasing? 16. The reaction 2NO(g) + 2H₂(g) →→→ N2(g) + 2H₂O(g) occurs in three steps. Step 1: NO + NO → N2O2 (fast) Step 2: _(slow) Step 3: N₂O + H2 → N2 + H₂O (fast) a. Write the reaction in step 2. b. What is the molecularity in the "rate determining step"? c. Mention two reaction intermediates in this reaction. 17. In the following reaction, the rate becomes nine times when concentration of B is tripled and concentration of A is kept constant. The rate becomes double when concentration of A is doubled and concentration of B is kept constant. A + B → C + D Write the rate law for this reaction. a.