In line with the correct answers to the previous question, applying Nernst equat

Question

In line with the correct answers to the previous question, applying Nernst equation under standard conditions to the reaction leads to K =10^(E0cell/(0.0592V/n))

For a cell reaction that uses 6 moles of electrons and produces a potential of 3.46 V, calculation of K leads to K = 10^__________________/(0.0592/_________________), which is_________________________(a 6-letter word with a "g" inside) than_______________________(a digit), which proves that the cell reaction favors

______________(a 8-letter word with letter "d" inside)

Explanation / Answer

K =10^(E0cell/(0.0592V/n))
On substituting the values of V = 3.46 V and n = 6 moles

K = 10^(E0cell/0.034) means K = e-DG/RT

For a cell reaction that uses 6 moles of electrons and produces a potential of 3.46 V, calculation of K leads to K = 10^_______E0cell___________/(0.0592/___0.034______________), which is_________________K = e-DG/RT________(a 6-letter word with a "g" inside) than_________a 6 numbers______________(a digit), which proves that the cell reaction favors

____________Addition__(a 8-letter word with letter "d" inside)

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