Question

Take a series of observations to determine if process is spontaneous. Based upon those observations, you will create an activity series, listing the metals in order of their reactivity. Second, you will construct a series of virtual galvanic cells and use those to power a stopwatch. Third, you will determine the standard reduction potential of an unknown metal; comparing its reduction potential to a standard list, you will identify the unknown. Finally, you will create a situation in which the cells are not in the standard condition and measure the cell potential; using the Nernst equation, you will determine the concentration of an unknown solution

Answer the below questions for the portion of the activity in which Sn(s) is placed in AgNO3(aq)
1. Is there a reaction? (circle the correct response) Yes / No
2. How many electrons are transferred 4 electrons
3. Write the balanced redox reaction for the combination of AgNO3(aq) and Sn(s)Sn(s) + Ag+(aq)  Sn2+(aq) + Ag(s)

Answer 1

Step-by-step explanation:

2AgNO₃ + Sn ⇄ Sn( NO₃)₂ + 2Ag

Ag⁺/Ag = .80 V

Sn⁺²/Sn = - .14 V

Hence Ag will be reduced and Sn will be oxidised . Hence the reaction will take place . YES .

2 ) 2 electrons are transferred .

3 )

2Ag⁺ + 2e = 2Ag

Sn = Sn⁺² + 2e

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2Ag⁺ + Sn = Sn⁺² + 2Ag .