This chemistry question involves key chemical concepts and calculations. The detailed solution below walks through each step, from identifying the reaction type to computing the final answer.
ScanSolve AI Answer
Here are the solutions to question 32(a). Question 32(a): The diagram shows a Zinc-copper cell. Given: Standard electrode potential of Zinc (Zn^2+/Zn) = -0.76 V Standard electrode potential of Copper (Cu^2+/Cu) = +0.34 V (i) The identity of W In a Zinc-copper cell, Zinc has a more negative standard electrode potential (-0.76 V) compared to copper (+0.34 V). This means Zinc is more easily oxidized and acts as the anode (negative electrode). The electrode labeled W is on the left, typically representing the anode. The identity of W is Zinc (Zn). (ii) The identity of X Since W is the Zinc electrode, X must be the other electrode, which is copper. Copper acts as the cathode (positive electrode) where reduction occurs. The identity of X is Copper (Cu). (iii) The equation for the overall cell reaction Step 1: Write the half-reactions for oxidation (at anode) and reduction (at cathode). • At the anode (W, Zinc), oxidation occurs: Zn(s) Zn^2+(aq) + 2e^- • At the cathode (X, Copper), reduction occurs: Cu^2+(aq) + 2e^- Cu(s) Step 2: Combine the half-reactions to get the overall cell reaction. The electrons cancel out. Zn(s) + Cu^2+(aq) Zn^2+(aq) + Cu(s) (iv) The reading on the voltmeter The reading on the voltmeter is the standard cell potential (E^_cell). E^_cell = E^_cathode - E^_anode Here, E^_cathode is the standard reduction potential of copper (+0.34 V), and E^_anode is the standard reduction potential of zinc (-0.76 V). E^_cell = (+0.34 V) - (-0.76 V) E^_cell = 0.34 V + 0.76 V E^_cell = +1.10 V Last free one today — make it count tomorrow, or type /upgrade for unlimited.