Textbook-Integrated Guide to Educational Resources

Calculate the G^o for the oxidation of 2 mole of silver in the following balanced reaction.

2Ag(s) + CaI₂(aq) Ca(s) + 2AgI(s)

Calculate E^o for the following balanced reaction.

Fe(s) + Fe₂(SO₃)₃(s) 3FeSO₃(s)

One method for protecting metals against corrosion is to connect the metal directly to a "sacrificial anode". This is the method used to protect pipelines and ships hulls. Which of the following metals would you consider the best candidate for a sacrificial anode for a ship's hull? The hull is steel (which is mostly iron).

Consider a cell composed of the following half-reactions. Determine the magnitude of E° for the cell and decide whether the reaction will be product-favored or reactant-favored as written.

Cs + Cl₂ CsCl₂

Fe + Fe₂(SO₃)₃ 3FeSO₃

What will be the products of the electrolysis of an aqueous solution of Tin (II) sulfate (SnSO₄)? (The electrodes themselves are platinum.)

Zn(s) Zn²⁺(aq) + 2e^-
2NH₄⁺(aq) + 2e^- 2NH₃(g) + H₂(g)

Consider the electrochemical cell diagram shown below. As you observe the reaction in the cell, you notice that the tin electrode seems to be disappearing while there are deposits forming on the silver electrode. Which of the following is a correct statement?

Au³⁺(aq) + 3 electrons Au(s)

Magnesium reacts with nitric acid to form magnesium nitrate and nitrogen monoxide in an acidic aqueous solution. Write the balanced equation for this reaction.