Electrochemistr...

Assertion : A voltaic cell spontaneously converts chemical energy into electrical energy.

The below reaction is the gold-plating process reaction.
            $${ Au }^{ 3+ }\left( aq \right) +3{ e }^{ - }\rightarrow Au\left( s \right) $$
If $$0.600 g$$ of $$Au$$ is plated onto a metal, how many coulombs are used?

In an electrochemical cell, reduction takes place at anode          BECAUSE           oxidation always takes place at the cathode.

Which of these processes could be associated with the following reaction.

A salt bridge :

A positive cell potential tells you ________.

Consider the table of standard reduction potentials shown below.

Half-reaction	$$E^{\circ}$$
$$Cl_{2} + 2e^{-}\rightarrow 2Cl^{-}$$	$$1.36\ V$$
$$O_{2} + 4H^{+} +  4e^{-} \rightarrow 2H_{2}O$$	$$1.23\ V$$
$$2H_{2}O + 2e^{-} \rightarrow H_{2} + 2OH^{-}$$	$$-0.83\ V$$
$$Rb^{+} + e^{-} \rightarrow Rb$$	$$-2.93\ V$$

Use the information from the table and your knowledge of electrochemistry to predict the CORRECT net ionic equation for the reaction that will occur when an aqueous solution of rubidium chloride undergoes electrolysis.

A steady current of $$10.0$$ Amps is passed through a nickel production cell of $$15$$ minutes.
Which of the following is the correct expression for calculating the number of grams of nickel produced?
Note:
$$\bullet 1\ faraday = 96,500\ Coulombs$$
$$\bullet$$ The electroytic cell involves the following half-reaction:
$$Ni_{(aq)}^{2+} + 2e^{-} \rightarrow Ni_{(s)}$$

Two half-cells have potentials $$-0.44$$ and $$0.799$$ volt respectively. These two are coupled to make a galvanic cell. Which of the following will be true?

(A) 1 faraday = 96,500 coulomb.
It is a charge of 1 mole electrons.
(R) 1 faraday charge liberates one gram equivalent of substance at an electrode.