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miskamm [114]
3 years ago
9

9) How long would it take 100 molecules of valinomycin to transport enough K+ to change the concentration inside an erythrocyteo

f volume 100um3by10 mM? (Assume that valinomycin does not also transport any K+ out of the cell, which it really does, and that valinomycin molecules outside the cell are always saturated with K+.)
Chemistry
1 answer:
Alenkinab [10]3 years ago
3 0

Answer: Time required for 100 molecules of valinomycin to transport enough K^{+} to change the concentration inside an erythrocyte is 10 minutes.

Explanation:

The given data is as follows.

 Ions to be transported = (10 mM) \times (100 \mu^{3})(N)

            = 0.010 mol \times 10^{-13} L \times 6.02 \times 10^{23} ions/mol

             = 6.02 \times 10^{6} ions

Here, there are 100 ionophores are present and each one of ionophores are required to transport a value of  ions.

Therefore, the time required for 100 molecules of valinomycin to transport enough K^{+} to change the concentration inside an erythrocyte is as follows.

   6.02 \times 10^{6} ions \times \frac{1 sec}{10^{4} ions}

              = 602 sec

or,          = 10 minutes        (as 1 min = 60 sec)

Thus, we can conclude that time required for 100 molecules of valinomycin to transport enough K^{+} to change the concentration inside an erythrocyte is 10 minutes.

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Answer : The 'Ag' is produced at the cathode electrode and 'Cu' is produced at anode electrode under standard conditions.

Explanation :

Galvanic cell : It is defined as a device which is used for the conversion of the chemical energy produces in a redox reaction into the electrical energy. It is also known as the voltaic cell or electrochemical cell.

In the galvanic cell, the oxidation occurs at an anode which is a negative electrode and the reduction occurs at the cathode which is a positive electrode.

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The balanced two-half reactions will be,

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Reduction half reaction (Cathode) : Ag^{+}(aq)+e^-\rightarrow Ag(s)

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Cu(s)+2Ag^{+}(aq)\rightarrow Cu^{2+}(aq)+2Ag(s)

From this we conclude that, 'Ag' is produced at the cathode electrode and 'Cu' is produced at anode electrode under standard conditions.

Hence, the 'Ag' is produced at the cathode electrode and 'Cu' is produced at anode electrode under standard conditions.

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