Iron and nickel are used to make an electrochemical cell by using slat bridge to join a half-cell containing 1.0 M solution of Fe^(2+)(aq) in which a strip of iron has been immersed to a second half-cell which contains 1.0 M Ni^(2+)(aq) solution in which a strip of nickel has been immersed. A voltmeter is connected between the two metal strips. (i) In which cell does reduction occurs? (ii) Write the half-cell reactions involved. (iii) Which metal is the anode? (iv) In which direction are the electrons passing through the voltmeter? (v) What would be effect ont he voltmeter reading if Fe^(2+) concentration were increased? (vi) What will be the voltmeter readind when the cell reaches equilbirium? Given that the standard electrode potential of Fe^(2+)//Fe and Ni^(2+)//Ni electrodes are -0.44 and -0.25 volt respectively.

Iron and nickel are used to make an electrochemical cell by using slat

1.	Iron and nickel are used to make an electrochemical cell by using slat bridge to join a half-cell containing 1.0 M solution of Fe^(2+)(aq) in which a strip of iron has been immersed to a second half-cell which contains 1.0 M Ni^(2+)(aq) solution in which a strip of nickel has been immersed. A voltmeter is connected between the two metal strips. (i) In which cell does reduction occurs? (ii) Write the half-cell reactions involved. (iii) Which metal is the anode? (iv) In which direction are the electrons passing through the voltmeter? (v) What would be effect ont he voltmeter reading if Fe^(2+) concentration were increased? (vi) What will be the voltmeter readind when the cell reaches equilbirium? Given that the standard electrode potential of Fe^(2+)//Fe and Ni^(2+)//Ni electrodes are -0.44 and -0.25 volt respectively.
Answer» Answer :(i) Nickel half cell (ii) `NI^(2+)+2e^(-)toNi` (iii) Fe is anode (iv) IRON to nickel (v) Voltmeter reading decreases (VI) V=0