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Qualitative

100

What does the equilibrium constant not contain?

solids or liquids

200

Which of the following is true at equilibrium?

a) only forward reaction stops

b) both reverse and forward reaction stop

c) rate constants for forward and reverse reactions are equal.

d) the rates of the forward and reverse reaction are equal

d

300

If Q_c is greater than K_c what direction will the system do to reach equilibrium?

Would perform reverse rate reaction

400

If the reaction quotient is equal to 2.39 x 10^-6 and K_c equals 3.39 x 10^-8 which way will the system have to move to reach equilibrium?

reverse rate- form more reactants

500

Given the reaction below, if the volume of the equilibrium mixture is suddenly increased, what is the resulting relationship between Q and Kc the instant the volume is increased and will the moles of NH₃ stay the same or will it increase or decrease as the reaction mixture seeks to re-establish equilibrium?

H₂NNH₂(g) + H₂(g) = 2NH₃(g)

a. Q>Kc, mol NH₃ decreases

b. Q> Kc mol NH₃ increases

c. Q<Kc, mol increases

d. Q=Kc, mol NH₃ stay the same

D

Quantitative

100

Calculate Kc if a container contains 1.00 Liter of 1.06 moles of H₂ and 1.57 moles of CO. At equilibrium, .200 moles of CH₃OH were in the container.

2H₂(g) + CO(g)= CH₃OH

.335

200

For a reaction, K_c equaled .0952. What would be the equilibrium concentration NO if the initial concentrations were .6 M N₂ and .6M O₂?

N₂ (g)+ O₂(g)=2NO(g)

.0802

300

What is the equilibrium constant(K_p) if O₂= .400 atm, NaO= 0 atm if the total equilibrium pressure equals .614?

2Na(s) + O₂= 2NaO

.984=k_p

400

if 20 moles of NaCl is placed in an empty 4-liter container. At equilibrium 8 mols Cl₂  was found in the container, calculate Kc

2NaCl= Cl₂ +2 Na

32

500

Calculate all equilibrium concentrations if the initial concentration for CO equals .300M for Cl2 is .500M and COCl2 is .700M. Kc=77.5

CO(g) + Cl2= COCl2(g)

CO=.049

Cl=.249

COCl=.951