Thank you for the help. There are two questions. The first I have answered, but
ID: 875630 • Letter: T
Question
Thank you for the help. There are two questions. The first I have answered, but it is needed for the second question.
Question 1.
An electrochemical cell is created using gold and magnesium half-cells under standard conditions (ie. A gold bar in a gold ion solution, and a magnesium strip in a magnesium ion solution).
Write the equations for the half-cell undergoing oxidation and undergoing reduction
Write the overall, balanced equation
Identify the anode and cathode
Calculate the voltage for the cell
You do not need to diagram the cell
Answer to Question 1.
Question 2.
Consider the same electrochemical cell as in the question above.
Imagine that after the cell has run for some time, the mass of the magnesium electrode has changed by 5.0 g. What must have been the change in mass of the gold electrode, and will its mass increase or decrease?
Attempt at answer:
"As the electrons will be deposited at the cathode, Mg2+ will gain 5g and Au (the gold electrode) will lose 5g."
But I need to include stoichiometry in my answer and I'm not sure how. Thank you for any help!
ealance For eH Half- reachons LJ .50 V 2.37 V 3.87 V aftce kor e Cdthoda An LOl 21Explanation / Answer
its mass increase because they are proportional
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