Worksheet: Reaction Quotients and Directions of Change

In this worksheet, we will practice predicting changes in the position of equilibrium by comparing reaction quotients with equilibrium constants.

Q1:

Sulfuryl chloride decomposes reversibly into chlorine and sulfur dioxide, as shown by the equation. SOCl()SO()+Cl()2222ggg

In one gas mixture, [SOCl]22 = 0.16 M, [Cl]2 = 0.13 M, and [SO]2 = 0.075 M. The value of 𝐾c for the reaction is 0.078. In which direction will the reaction shift in order to reach equilibrium?

  • ATo the left
  • BNeither; it has already reached equilibrium
  • CTo the right

Q2:

The reaction shown has 𝐾=4.50×10P at 720 K. N()+3H()2NH()223ggg

If, at this temperature, a reaction vessel is filled with each gas to the partial pressures listed, in which direction will it shift to reach equilibrium? P(NH)=93atm3, P(N)=48atm2, and P(H)=52atm2.

  • ATo the right
  • BTo the left
  • CNeither; it has reached equilibrium

Q3:

Consider the reaction shown, where 𝐾=0.050P, 𝑃10.0(NO)=atm, and 𝑃𝑃5(N)=(O)=atm22. N()+O()2NO()22ggg

What is the reaction quotient?

  • A 𝑄 = 2 . 5 P
  • B 𝑄 = 4 . 0 P
  • C 𝑄 = 0 . 2 5 P
  • D 𝑄 = 0 . 4 P

In which direction will the reaction proceed from this point?

  • ATo the right
  • BNeither: it has reached equilibrium.
  • CTo the left

Q4:

Consider the reaction shown, where 𝐾=4.6×10c, [NO]=1.00M, [Cl]=1.00M2, and [NOCl]=0M. 2NO()+Cl()2NOCl()ggg2

What is the reaction quotient?

  • A 𝑄 = 0 c
  • B 𝑄 = 1 . 0 0 c
  • C 𝑄 = 2 . 0 0 c
  • D 𝑄 = 0 . 5 0 c
  • E 𝑄 c undefined

In which direction will the reaction proceed from this point?

  • ANeither; it has reached equilibrium
  • BTo the left
  • CTo the right

Q5:

Consider the reaction shown, where 𝐾=16.5P, P(SO)=1.00atm3, P(SO)=1.00atm2, and P(O)=1.00atm2. 2SO()2SO()+O()322ggg

What is the reaction quotient?

  • A 𝑄 = 2 . 5 0 P
  • B 𝑄 = 0 . 5 0 P
  • C 𝑄 = 2 . 0 0 P
  • D 𝑄 = 1 . 5 0 P
  • E 𝑄 = 1 . 0 0 P

In which direction will the reaction proceed from this point?

  • ATo the right
  • BTo the left
  • CNeither; it has reached equilibrium

Q6:

Consider the reaction shown, where 𝐾=6.8×10P, P(NH)=3.0atm3, P(N)=2.0atm2, and P(H)=1.0atm2. 2NH()N()+3H()322ggg

If the partial pressures of all species are 1.0 atm under standard conditions, what is the reaction quotient for this reaction to two significant figures?

  • A 𝑄 = 0 . 2 2 P
  • B 𝑄 = 0 . 8 9 P
  • C 𝑄 = 4 . 5 P
  • D 𝑄 = 0 . 6 7 P
  • E 𝑄 = 1 8 P

In which direction will the reaction proceed from this point?

  • ATo the left
  • BNeither; it has reached equilibrium
  • CTo the right

Q7:

Consider the reaction shown, where 𝐾=17c, [NH]=0.20M3, [N]=1.00M2, and [H]=1.00M2. 2NH()N()+3H()322ggg

If the concentrations of all species are 1.00 M under standard conditions, what is the reaction quotient for this reaction?

  • A 𝑄 = 0 . 2 0 c
  • B 𝑄 = 2 5 c
  • C 𝑄 = 5 . 0 c
  • D 𝑄 = 0 . 0 4 0 c
  • E 𝑄 = 0 . 4 5 c

In which direction will the reaction proceed from this point?

  • ANeither; it has reached equilibrium
  • BTo the left
  • CTo the right

Q8:

For the reaction CO()+HO()CO()+H()gggg222c,𝐾=0.64, initial concentrations of the species are:

  • [ C O ] = 0.0203 M,
  • [ H O ] 2 = 0.0203 M,
  • [ C O ] 2 = 0.0040 M,
  • [ H ] 2 = 0.0040 M.

In which direction does the reaction shift in order to reach equilibrium?

  • ATo the left
  • BNeither; the reaction is already at equilibrium
  • CTo the right

Q9:

The initial concentrations of the species in a solution are as follows: [CO] = 0.011 M, [HO]2 = 0.0011 M, [CO]2 = 0.037 M, and [H]2 = 0.046 M. These species participate in a reversible reaction represented by the equation: In which direction does the reaction shift in order to reach equilibrium?

  • ATo the right
  • BNeither: the reaction is already at equilibrium.
  • CTo the left

Q10:

The initial concentrations of the species in a solution are as follows: [CO] = 0.0094 M, [HO]2 = 0.0025 M, [CO]2 = 0.0015 M, and [H]2 = 0.0076 M. These species participate in a reversible reaction represented by the following equation. CO()+HO()CO()+H()gggg222c,𝐾=0.64 In which direction does the reaction shift in order to reach equilibrium?

  • ATo the left
  • BTo the right
  • CNeither; the reaction is already at equilibrium

Q11:

An equilibrium is established according to the following equation:

What will happen in a solution that is 0.20 M each in Hg22+, NO3, H+, Hg2+, and HNO2?

  • A H g 2 2 + will be reduced and NO3 oxidized.
  • B H g 2 + will be reduced and HNO2 oxidized.
  • C H g 2 + will be oxidized and HNO2 reduced.
  • DThere will be no change because all reactants and products have an activity of 1.
  • E H g 2 2 + will be oxidized and NO3 reduced.

Q12:

One of the solubility rules is that all chlorides are soluble except HgCl22, AgCl, PbCl2, and CuCl.

Which of the following expressions correctly describes the equilibrium constant, 𝐾c, for the equilibrium shown? Pb()+2Cl()PbCl()2+2aqaqs

  • A 𝐾 1 c
  • B 𝐾 0 c
  • C 𝐾 = 0 c
  • D 0 < 𝐾 1 c
  • E 𝐾 1 c

Q13:

Benzene is one of the compounds used as octane enhancers in unleaded gasoline. It is manufactured by the catalytic conversion of acetylene to benzene:

Which value of 𝐾c would make this reaction most useful commercially?

  • A 𝐾 0 . 1 c
  • B 𝐾 1 c
  • C 𝐾 0 . 0 1 c
  • D 𝐾 0 c
  • E 𝐾 1 0 c

Q14:

One of the solubility rules is that all chlorides are soluble except HgCl22, AgCl, PbCl2, and CuCl.

Which of the following expressions correctly describes the equilibrium constant, 𝐾c, for the equilibrium shown? AgCl()Ag()+Cl()saqaq+

  • A 𝐾 1 c
  • B 0 < 𝐾 1 c
  • C 𝐾 = 0 c
  • D 𝐾 0 c
  • E 𝐾 1 c

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