Question
Please help me with these questions.
Multiple Choice: Choose the single best answer for questions 1 - 5. Put your answers on the scantron sheets provided A copper and an iron electrode are placed in adjacent solutions containing Cu5O4 (aq) and FeSO4 (Cq) respectively. The standard reduction potential of Fe2* to Fe is -0.44 V and the standard reduction potential of Cu2* to Cu is +0.340 V. A wire connects the two electrodes but nothing connects the solutions (there is no salt bridge). If a light bulb was hooked up to the wire and then each electrode was placed in their respective solutions, what would you see? the light bulb would turn on the light bulb would turn off the light bulb would flash on very briefly and then turn off it is impossible to know what will happen none of these would happen The same situation as above is set up but now with a salt bridge connecting the two solutions. The solution in which the iron electrode is placed is replaced with a CaC03 solution instead of the FeS04. Fe2+ makes an insoluble compound FeCO3 when placed in solution with CO32- ions but Cu2+ makes a soluble compound CuCO3. If the two electrodes are placed in the solutions as before, what would you see? the light bulb would turn on and stay on for only a few seconds the light bulb would burn out the light bulb would flash on and then turn off the light bulb would not turn on the light bulb would turn on The iron/iron sulfate standard electrode -0.44 V The standard electrode The iron/iron sulfate standard electrode potential is -0.44 v. The standard electrode potential for copper sulfate is +0.340 V. what is the galvanic cell potential of this cell? -0.1V b.-0.10V c.+0.10V d.+078V e.+0.780V
Explanation / Answer
1)a
2)d
3) Ecell = 0.34 - (-0.44) = 0.78 v
option d is correct
