35. Because the CV(aq) anion is NOT oxidized by the Ag+(aq) cation, it can be safely assumed that the reduction potential of Cl2(g) is which of the following?
A . Less than -0.80 volts
B. Between -0.80 and 0.0 volts
C . Between 0.0 and 0.80 volts
D . Greater than 0.80 volts
(Ag+ is a reducing agent with the listed value being 0.80 V).
Can someone explain this to me? I'm okayish at Electrochemistry but I don't really understand how to go about doing the problem/understand the explaination.
Choice D is correct. According to Table 1, the reduction potential for silver cation is 0.80 volts. This means that because chloride anion is not oxidized to Cl2 by silver cation, the oxidation potential of CI- to Cl2(g) must less than (more negative than) -0.80 volts. Reversing this reaction means that the reduction potential of Cl2(g) to CI- must be greater than +0.80 volts. This makes choice D the best answer. You should have been instinctively inclined to zero in on either choice A or choice D without knowing anything about the numerical values, because they are the extreme answers that exclude the other choices.
40. Which of the following reactions would produce the LOWEST (or most negative) voltage?
Since the metal cations are reduced by chlorine gas in each case, we can simplify this question. Because chlorine is oxidized in each answer choice, the question of which reaction generates the lowest voltage is really a question of which cation has the lowest reduction potential. The lowest reduction potential, according to the data in Table 1, is found with Ag+. This makes choice A the best answer.
How do you get to the conclusion that lowest voltage is really a question of lowest reduction potential?
A . Less than -0.80 volts
B. Between -0.80 and 0.0 volts
C . Between 0.0 and 0.80 volts
D . Greater than 0.80 volts
(Ag+ is a reducing agent with the listed value being 0.80 V).
Can someone explain this to me? I'm okayish at Electrochemistry but I don't really understand how to go about doing the problem/understand the explaination.
Choice D is correct. According to Table 1, the reduction potential for silver cation is 0.80 volts. This means that because chloride anion is not oxidized to Cl2 by silver cation, the oxidation potential of CI- to Cl2(g) must less than (more negative than) -0.80 volts. Reversing this reaction means that the reduction potential of Cl2(g) to CI- must be greater than +0.80 volts. This makes choice D the best answer. You should have been instinctively inclined to zero in on either choice A or choice D without knowing anything about the numerical values, because they are the extreme answers that exclude the other choices.
40. Which of the following reactions would produce the LOWEST (or most negative) voltage?
Since the metal cations are reduced by chlorine gas in each case, we can simplify this question. Because chlorine is oxidized in each answer choice, the question of which reaction generates the lowest voltage is really a question of which cation has the lowest reduction potential. The lowest reduction potential, according to the data in Table 1, is found with Ag+. This makes choice A the best answer.
How do you get to the conclusion that lowest voltage is really a question of lowest reduction potential?
