For the standard cell, the Cu2 half-cell was made with 1.0L of 1.0MCu(NO3)2 and the Zn2 half-cell was made with 1.0L of 1.0MZn(NO3)2. The experiment was repeated, but this time the Cu2 half-cell was made with 0.50L of 2.0MCu(NO3)2 and the Zn2 half-cell was made with 1.0L of 1.0MZn(NO3)2. Is the cell potential for the nonstandard cell greater than, less than, or equal to the value calculated in part (b)

Explanation:

Electrochemistry

For parts of the free-response question that require calculations, clearly show the method used and the steps involved in arriving at your answers. You must show your work to receive credit for your answer. Examples and equations may be included in your answers where appropriate. jpeg Answer the following questions related to the standard galvanic cell represented in the diagram above. The reduction half-reactions for Cu2+ and Zn2+ are given in the table below. Half-Reaction E°(V) Cu2++2e−→Cu(s) 0.34 Zn2++2e−→Zn(s) −0.76 (a) What is the net-ionic equation for the overall reaction that takes place as the cell operates? (b) What is the value of E° for the cell? (c) What is the value of ΔG°, in kJ/molrxn, for the cell? (d) The following diagram on the left represents the copper nitrate solution in the half‑cell before the galvanic cell starts to operate. In the following diagram on the right, draw a representation of the solution in the same half‑cell after the galvanic cell has been operating for some time and is still producing a voltage.(e) Assume that the mass of the Cu electrode changes by x grams in a certain period of time. What is the mathematical expression for the change in mass of the Zn electrode during the same period of time?

(f) For the standard cell, the Cu2+ half-cell was made with 1.0L of 1.0MCu(NO3)2 and the Zn2+ half-cell was made with 1.0L of 1.0MZn(NO3)2. The experiment was repeated, but this time the Cu2+ half-cell was made with 0.50L of 2.0MCu(NO3)2 and the Zn2+ half-cell was made with 1.0L of 1.0MZn(NO3)2. Is the cell potential for the nonstandard cell greater than, less than, or equal to the value calculated in part (b)? Justify your answer.(g) If the experiment is repeated with the Cu electrode replaced with a Cu electrode with twice the mass, will the initial cell voltage be greater than, less than, or equal to the initial cell voltage in the original experiment? Justify your answer.

consider the reaction below.

 no rx

at 500 k, the reaction is at equilibrium with the following concentrations.

[pci5]= 0.0095 m

[pci3] = 0.020

[ci2] = 0.020 m

what is the equilibrium constant for the given reaction?

0.042

0.42

2.4

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