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castortr0y [4]
3 years ago
9

An electrochemical cell is constructed with a zinc metal anode in contact with a 0.052 M solution of zinc nitrate and a silver c

athode in contact with a 0.0042 M solution of silver(I) nitrate. What is the value of Q to use in the Nernst equation for this cell
Chemistry
1 answer:
lana [24]3 years ago
6 0

Answer:

Q = 12.38

Explanation:

The Nernst equation is given as; Ecell = E°cell - (2.303RT/nF) log Q  ;where Q is the reaction quotient.

The reaction quotient, Q  in a reaction, is the product of the concentrations of the products divided by the product of the concentrations of the reactants.

In an electrochemical cell, Q is the ratio of the concentration of the electrolyte at the anode to that of the electrolyte at the cathode.

Q = [anode]/[cathode]

therefore , Q = 0.052/0.0042 = 12.38

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<u>Answer:</u>

<u>For a:</u> The mass of acetic anhydride needed is 73.91 grams.

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Putting values in equation 1, we get:

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By stoichiometry of the reaction:

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So, 0.724 moles of salicylic acid will react with = \frac{1}{1}\times 0.724=0.724mol of acetic anhydride.

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Hence, the mass of acetic anhydride needed is 73.91 grams.

  • <u>For b:</u>

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1 mole of salicylic acid is producing 1 mole of aspirin.

So, 0.724 moles of salicylic acid will produce = \frac{1}{1}\times 0.724=0.724mol of aspirin.

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Putting values in equation 1, we get:

0.724mol=\frac{\text{Mass of aspirin}}{180.158g/mol}\\\\\text{Mass of aspirin}=130.43g

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