Textbook-Integrated Guide to Educational Resources

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 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?

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?

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!}