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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?

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

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