A) Use the table \'Standard Reduction Potentials\' located in the \'Tables\', to

Question

A) Use the table 'Standard Reduction Potentials' located in the 'Tables', to predict if a reaction will occur when Cu metal is put into a 1M aqueous Mg2+ solution. If a reaction will occur, write a balanced net ionic equation for the reaction

B) Use the table 'Standard Reduction Potentials' located in the 'Tables', to predict if a reaction will occur when Al metal is put into a 1M aqueous Cd2+ solution.

If a reaction will occur, write a balanced net ionic equation for the reaction.

C) Use a table of Standard Reduction Potentials to predict if a reaction will occur between Co metal and Br2(l), when the two are brought in contact via standard half-cells in a voltaic cell.
If a reaction will occur, write a balanced net ionic equation for the reaction, assuming that the product ions are in aqueous solution

Explanation / Answer

The SRP values of Br2 =+1.09V

Cu = +0.34

Co =-0.28

C d = -0.40

Al = -1.66

Mg = -2.36

Qa) copper SRP is more positive than Mg , which shows Cu+2 has more tendency to under go reduction than Mg+2. Thus no reaction takes place.

b) When Al is placed in Cd+2 solution Al goes into solution and Cd is deposited. It is because Cd+2 has less negative SRP, that is more tendency to undergo reduction than Al+3.

The net ionic equation is

2 Al + 3Cd+2(aq) ------> 2Al+3 (aq) +3 Cd

c) Yes. There is a reaction between Co and Br2 as the SRP of bromine is more positive , means it readily gets reduced to bromide ions , oxidising Co into Co+2 ions.

The the net ionic equation is

Co + Br2 ------> Co+2 (aq)   + 2Br- (aq)

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