Given the following redox reaction: 1/2 H2(g) + Ag+(aq) -> Ag(s) + H+(aq) Starti

Question

Given the following redox reaction:

1/2 H2(g) + Ag+(aq) -> Ag(s) + H+(aq)

Starting with a given concentation of Ag+(aq), and considering [H+] =1M and H2 =1 atm, how will the E measured change as an inert electrolyte such as NaNO3 is added in increasing concentration? Assume solution do not behave ideally with increasing NaNO3

A) E drops with increasing [NaNO3]

B) E increases drops with increasing [NaNO3]

C) E does not change with increasing [NaNO3]

can someone help me with a detail solution? thanks

4) Given the following redox reaction: + Starting with a given concentration of Ag^+(aq), and considering [H^+] = 1 M and H2 = 1 atm, how will the E measured change as an inert electrolyte such as NaNO3 is added in increasing concentration? Assume solutions do not behave ideally with increasing NaNO3 A) E drops with increasing [NaNO3] B) E increases drops with increasing [NaNO3] C) E does not change with increasing [NaNO3] D) The information provided is not sufficient E) Blank, do not choose

Explanation / Answer

right answer is (c) due to any of the species interact chemically with NaNO3 and changes in the activity of the ions are almost the same and cancels due form of Q in the nerst equation.

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