what current will be able to produce 20 volume of chlorine by electrolysis at STP within one hour?
20 what volume? cc? L?
Please i dont understand
To determine the current needed to produce 20 volumes of chlorine gas by electrolysis at STP (Standard Temperature and Pressure) within one hour, we need to consider Faraday's Laws of Electrolysis.
1. Calculate the volume of chlorine gas produced:
According to Avogadro's Law, one mole of any gas occupies 22.4 liters at STP.
So, 20 volumes of chlorine gas would be 20 * 22.4 = 448 liters.
2. Determine the number of moles of chlorine gas produced:
Since the molar volume of any gas at STP is 22.4 liters, we can calculate the number of moles by dividing the volume by the molar volume:
448 liters / 22.4 liters/mol = 20 moles of chlorine gas.
3. Apply Faraday's Law:
Faraday's Law states that the amount of substance produced during electrolysis is directly proportional to the quantity of electricity passed through the electrolyte.
The equation for Faraday's Law is:
moles of substance = (current * time) / (number of electrons * Faraday's constant)
Here, we can rearrange it to solve for the current:
current = (moles of substance * number of electrons * Faraday's constant) / time
For chlorine gas, the number of electrons required is 2 because it is formed from 2 chloride ions.
The Faraday's constant is approximately 96,485 C/mol.
Plugging in the values:
current = (20 moles * 2 * 96,485 C/mol) / 3600 seconds
Simplifying:
current = 10715 C/s
Therefore, a current of approximately 10715 amperes (A) would be required to produce 20 volumes of chlorine gas by electrolysis at STP within one hour.