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)

CO(g) + H₂O(g) CO₂(g) + H₂(g) H⁰= -41.2 kJ

What will happen to the concentration of CO₂ if the temperature is increased?

C₃H₈(g) + 5O₂(g) 3CO₂(g) + 4H₂O(l)

CH₄(g) + Cl₂(g) CH₃Cl(g) + HCl(g)

Which of the following statements is true?

You have 0.4 moles C₂H₂ and 0.2 moles O₂ present initially in a 5L flask. You allow the reaction to run until it reaches equilibrium. Which of the following is the correct ICE table for this process?

What is the equilibrium constant for the following reaction under the same conditions?
C₂H₆(g) H₂(g) + C₂H₄(g) K = ?

COCl₂(g) CO(g) + Cl₂(g)

If you have 1.00 mole of COCl₂(g) in a 1.00L container initially, how many moles of COCl₂ will be present when the system reaches equilibrium?

You have 0.50 mol SbCl₅ present initially in a 1.0L flask. The system is allowed to reach equilibrium at 450^oC. There is 0.10 mol Cl₂ present at equilibrium. What is the equilibrium constant, K?

What is the calculated reaction quotient, Q? {2:NUMERICAL:=2.1e-1:1e-2#Correct! ~%50%2.1e-1:5e-2#Close but not quite right}

If K_c for this reaction at the temperature of the experiment is 3.7 x 10³, will the reaction move toward the left or toward the right? {1:MULTICHOICE:left#Sorry, that's wrong.~=right#Correct!}

Hint: Remember that the total pressure is the sum of all the partial pressures.

K_p for this reaction is {x} at {y}°C. Calculate K_c at this temperature. (R = 0.0821 L atm/mol K)

Note:
DO NOT use scientific notation
Use integers (no decimal places) even is this is not the correct number of significant figures.
DO NOT write in the units.
eg: 18

N₂(g)+ O₂(g) 2NO(g)

If you have 0.75 moles of N₂(g) and 0.75 moles of O₂(g) in a 2.0L container initially, how many moles of N₂ will be present when the system reaches equilibrium?

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

Enter your answer to ONE decimal place.
DO NOT use scientic notation.
DO NOT write in the units.

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.

Calculate the pH of a {x}M sodium acetate solution.