The formula to calculate the electrolysis voltage (V) is:
\[ V = \frac{\Delta G}{n \cdot F} \]
Where:
Let's say the Gibbs Free Energy Change (\( \Delta G \)) is 50000 J and the number of moles of electrons (\( n \)) is 2. Using the formula:
\[ V = \frac{50000}{2 \cdot 96485} \]
We get:
\[ V \approx \frac{50000}{192970} \approx 0.26 \]
So, the electrolysis voltage (\( V \)) is approximately 0.26 V.
Electrolysis voltage is the minimum voltage required to drive an electrochemical reaction through the process of electrolysis. During electrolysis, electrical energy is used to drive a non-spontaneous chemical reaction. The voltage required depends on the Gibbs Free Energy Change of the reaction, the number of moles of electrons involved, and Faraday’s Constant. This voltage is crucial in various industrial processes, such as the extraction of metals, electroplating, and the production of chemical compounds.
Definition: The minimum voltage required to electrolyze water into hydrogen and oxygen.
Formula: \( V = \frac{\Delta G}{nF} \)
Example: \( V = \frac{237000}{2 \times 96485} \)
Definition: The rate of electrolysis is the amount of substance produced or consumed at an electrode per unit time.
Formula: \( R = \frac{I \times t}{nF} \)
Example: \( R = \frac{5 \times 3600}{2 \times 96485} \)
Definition: Efficiency of water electrolysis is the ratio of the energy stored in the hydrogen produced to the electrical energy consumed.
Formula: \( \eta = \frac{H_{out}}{E_{in}} \)
Example: \( \eta = \frac{237000}{300000} \)
Definition: The chemical equation representing the electrolysis process.
Formula: \( 2H_2O(l) \rightarrow 2H_2(g) + O_2(g) \)
Example: \( 2H_2O(l) \rightarrow 2H_2(g) + O_2(g) \)
