Consider the galvanic cell,Pt(s)∣ H₂(1 atm)|H⁺(1 M)∣∣ Cl^-(1 M)∣ Hg₂Cl₂(s)|Hg(l).Which one of the following changes to the cell would cause the cell potential to increase (i.e. ,become more positive)?

Question

Quizplus · Accepted Answer

The pH of the solution on the left side of the cell is acidic due to the presence of H+ ions, which can react with the H₂ ion to form H2₂. This reaction consumes some of the H₂ ion, which reduces the concentration of reactant in the anode compartment and decreases the cell potential. By increasing the pH, the amount of H+ ions in the solution can be reduced, which will slow down the consumption of the H₂ ion and increase the cell potential. Therefore, choice D is the correct answer. Choices A and B are incorrect because the mass of Pt does not affect the reaction at the electrodes, as Pt is only a catalyst. Choice C is incorrect because decreasing the pH would increase the amount of H+ ions and accelerate the reaction at the anode, which would decrease the cell potential.

Consider the Galvanic Cell,Pt(s)∣ H2(1 Atm)|H+(1 M)∣∣ Cl-(1 M)∣ Hg2Cl2(s)|Hg(l)

Consider the Galvanic Cell,Pt(s)∣ H₂(1 Atm)|H⁺(1 M)∣∣ Cl^-(1 M)∣ Hg₂Cl₂(s)|Hg(l)