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18 Dec 2019

Calculate the cell potential at 298 K in non-standard conditions, Ecell, for the reaction 2H+(aq) + Zn(s) → H2(g) + Zn2+(aq) when the concentration of Zn2+ is 0.010M, the concentration of H+ is 2.5M, and the partial pressure of hydrogen gas is 0.30 atm.

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Nelly Stracke
Nelly StrackeLv2
31 Dec 2019

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Related questions

Consider the following cell reaction: Zn(s) + 2H+(aq) → Zn2+(aq) + H2(g); E°cell = 0.76 V Under standard-state conditions, what is E° for the following half-reaction? Zn2+(aq) + 2e– → Zn(s)

What is the effect on the emf of the cell shown in Figure 20.9, which has the overall reaction Zn(s) + 2H+(aq)→Zn2+(aq) + H2(g), for each of the following changes?

(a) The pressure of the H2 gas is increased in the cathode halfcell.

(b) Zinc nitrate is added to the anode half-cell. (c) Sodium hydroxide is added to the cathode half-cell, decreasing [H+]. (d) The surface area of the anode is doubled.

Zn (s) + 2H+ (aq) → Zn2+ (aq) + H2(g);

A voltaic cell is constructed that uses the following reaction and operates at 298 K: Zn(s)+Ni2+(aq)→Zn2+(aq)+Ni(s).

(a). What is the emf of this cell under standard conditions?

(b.) What is the emf of this cell when [Ni2+]= 3.30 M and [Zn2+]= 0.150 M ?

(c.) What is the emf of the cell when [Ni2+]= 0.100 M and [Zn2+]= 0.999 M ?

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