For a galvanic cell that uses the following two half-reactions, cr 2o 7 2-( aq) 14 h ( aq) 6 e - → 2 cr 3 ( aq) 7 h 2o( l)sn( s) → sn 2 ( aq) 2 e -how many moles of sn(s) are oxidized by four moles of cr 2o 7 2-

Answer : The number of moles of Sn(s) oxidized are 12 moles.

Explanation :

The given half cell reactions are:

Reduction half reaction :

Oxidation half reaction :

In order to balance the electrons, we will multiply oxidation half reaction by 3, we get:

Reduction half reaction :

Oxidation half reaction :

Now adding both half reaction, we get the overall reaction.

From the overall complete reaction, we conclude that

As, 1 mole of will oxidizes 3 moles of Sn

So, 4 moles of will oxidizes moles of Sn

Therefore, the number of moles of Sn(s) oxidized are 12 moles.

b

explanation:

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