How long must a constant current of 50.0 a be passed through an electrolytic cell containing aqueous cu2+ ions to produce 5.00 moles of copper metal? how long must a constant current of 50.0 a be passed through an electrolytic cell containing aqueous cu2+ ions to produce 5.00 moles of copper metal? 5.36 hours 2.68 hours 0.373 hours 0.187 hours?

An electrolytic is a type of electrochemical cell that utilises current or the energy source for the potential development across the cell in which the redox chemical reaction occurs.

For 5.36 hours constant current should be passed.

Given,

Current (I)= 50A

Quantity of electricity (Q) is given as,

The half cell of the reaction can be shown as,

1 mole of copper is deposited by,

If,

1 mole of Copper = 193000 Coloumb

5 moles of Copper = X

Solving for X:

Substituting values of Q and I in the above equation:

We know,

1 hour = 3600 sec

t = 5.36 hours.

Therefore, 5.36 hours are needed for a constant current supply.

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5.36 hours

Explanation:

where Q= quantity of electricity in coloumbs

I = current in amperes = 50A

t= time in seconds = ?

of electricity deposits 1 mole of Cu.

1 mole of Copper is produced by = 193000 Coloumb

5 moles of Copper is produced by=

   (1 hour=3600sec)

in 1783 cavendish was working with his hydrogen gas and found that when he burned it and condensed the vapor it was water. this was very significant since it disproved the greek theory of elements completely since water was not a simple substance but the product of two gases. it was lavoisier who hearing of the experiment gave cavendish's gas the name hydrogen ("water-producer") and added that hydrogen burned by combining with oxygen and that water was a hydrogen-oxygen combination.

explanation: