Consider the rechargeable battery: Zn(s)0ZnCl (aq)7Cl2(aq)0Cl (l)0C(s) (a) Write reduction half-reactions for each electrode. From which electrode will electrons flow from the battery into a circuit if the electrode potentials are not too different from E 8 values

Complete Question

Consider the rechargeable battery:

(a) Write reduction half-reactions for each electrode. From which electrode will electrons flow from the battery into a circuit if the electrode potentials are not too different from values

(b)

if the battery delivers a constant current of for 1.00 h , how many kg of will be consumed

a

    At the anode

   At the cathode

b

The value  is  

Explanation:

Generally the  half-reactions for each electrode is mathematically represented as

   At the anode

   At the cathode

Generally  from the question we are told that  

    The current is  

     The time is  

Generally the quantity of  charge consumed is  

=>    

=>    

Generally the number of moles of electron consumed is  

Here F is the faradays constant with value  

So

=>      

Generally the number of moles of    consumed is mathematically represented as

=>      

=>            

Generally the mass of    consumed is mathematically represented as

Here Z is the molar mass of   is  Z  = 70.9 g/mole

So

=>  

=>  

=>  

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