IBChemistryHLExam QuestionsHow Much, How Fast & How Far?How Far? The Extent of Chemical Change

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How Far? The Extent of Chemical Change (HL IB Chemistry)

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11 mark

Which statement describes a closed system?

  • Only matter can be transferred across the boundary

  • Only energy can be transferred across the boundary

  • Energy and matter can be transferred across the boundary

  • Energy and matter cannot be transferred across the boundary

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21 mark

Dinitrogen tetraoxide, N2O4, and nitrogen dioxide exist in equilibrium. This is represented by the reaction below:

2NO2 (g)  ⇌  N2O4 (g)            increment straight H = -57 kJ mol-1

Which conditions give the greatest percentage of NO2 at equilibrium?

  • high pressure and high temperature 

  • low pressure and high temperature 

  • high pressure and low temperature 

  • low pressure and low temperature 

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31 mark

Which statement below best describes a dynamic equilibrium?

  • the rate of the forward reaction is equal to the backwards reaction, and the concentrations of reactants and products is constant

  • the rate of the forward reaction is equal to the backwards reaction in a closed system, and the concentrations of the reactants and products are equal

  • the rate of the forward reaction is equal to the backwards reaction in a closed system, and the concentrations of the reactants and products is constant

  • the rate of reaction changes in either direction to counteract a change in conditions

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41 mark

Ethanol is manufactured by reacting steam with ethene.

C2H4 (g) + H2O (g) ⇌ C2H5OH (g)                        increment straight H = -45 kJ mol-1

What would increase the equilibrium yield of ethanol in this process?

I

adding a catalyst
II

increasing the pressure
III

decreasing the temperature

  • I and II only 

  • I and III only 

  • II and III only 

  • I, II and III

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51 mark

Propyl ethanoate is formed in an esterification reaction. How can the value of the equilibrium constant Kc be increased?

Propan-1-ol + ethanoic acid  ⇌  propyl ethanoate + water          begin mathsize 16px style increment H end style = -10 kJ mol-1

  • increasing the temperature

  • adding a catalyst 

  • increasing the pressure 

  • lowering the temperature 

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61 mark

In the reaction where gaseous iodine reacts with hydrogen,an equilibrium is established at 450 degreeC. The reaction is exothermic.

H2 (g) +   I2 (g) ⇌ 2HI (g)
 colourless   purple   colourless


Which change in conditions will cause the purple colour of the equilibrium mixture to become paler?

  • decrease in pressure

  • decrease in temperature

  • increase in pressure

  • increase in temperature

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71 mark

Nitrosyl chloride decomposes into nitrogen monoxide and chlorine according to the following equation.

2NOCl (g)   ⇌   2NO +  Cl2 (g)

What is the correct expression for Kc?

  • fraction numerator left square bracket NOCl right square bracket squared over denominator left square bracket NO right square bracket squared space left square bracket Cl subscript 2 right square bracket end fraction

  • fraction numerator left square bracket NO right square bracket space left square bracket Cl subscript 2 right square bracket over denominator left square bracket NOCl right square bracket end fraction

  • fraction numerator 2 left square bracket NO right square bracket space left square bracket Cl subscript 2 right square bracket over denominator 2 left square bracket NOCl right square bracket end fraction

  • fraction numerator left square bracket NO right square bracket squared space left square bracket Cl subscript 2 right square bracket over denominator left square bracket NOCl right square bracket squared end fraction

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81 mark

An equilibrium is established in the reaction.

AB (aq) + CD (aq)  ⇌  AC (aq) + BD (aq)             increment straight H = +180 kJ mol-1

Which factors would affect the value of Kc  in this equilibrium?

  • change in temperature in the absence of a catalyst

  • change in pressure in the presence of a catalyst

  • increasing the concentration of AB

  • increasing the concentration of AC

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91 mark

What is the equilibrium constant expression for the following equation?

3Cl2 (g)   +   I2 (g)  ⇋  2ICl3 (l)

  • fraction numerator 2 left square bracket ICl subscript 3 right square bracket over denominator 3 left square bracket Cl subscript 2 right square bracket plus left square bracket straight I subscript 2 right square bracket end fraction

  • fraction numerator 2 left square bracket ICl subscript 3 right square bracket over denominator 3 left square bracket Cl subscript 2 right square bracket space left square bracket straight I subscript 2 right square bracket end fraction

  • fraction numerator left square bracket Cl subscript 2 right square bracket cubed space left square bracket straight I subscript 2 right square bracket over denominator left square bracket ICl subscript 3 right square bracket squared end fraction

  • fraction numerator left square bracket ICl subscript 3 right square bracket squared over denominator left square bracket Cl subscript 2 right square bracket cubed space left square bracket straight I subscript 2 right square bracket end fraction

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101 mark

Hydrogen iodide can be made by the direct combination of hydrogen and iodine in the following equilibrium reaction. What is the expression for the equilibrium constant?

H2 (g)   +    I2 (g)   ⇋   2HI (g)

  • fraction numerator left square bracket 2 HI right square bracket over denominator left square bracket straight H subscript 2 right square bracket space left square bracket straight I subscript 2 right square bracket end fraction

  • fraction numerator 2 left square bracket HI right square bracket squared over denominator left square bracket straight H subscript 2 right square bracket space plus space left square bracket straight I subscript 2 right square bracket end fraction

  • fraction numerator left square bracket 2 HI right square bracket over denominator left square bracket straight H subscript 2 right square bracket space plus space left square bracket straight I subscript 2 right square bracket end fraction

  • fraction numerator left square bracket HI right square bracket squared over denominator left square bracket straight H subscript 2 right square bracket space left square bracket straight I subscript 2 right square bracket end fraction

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111 mark

What is the significance of the value of Kc ≫1 in a reversible reaction?

  • The reaction is almost complete

  • Very little reaction occurs

  • Equilibrium is established very quickly

  • The rate of the forward reaction is larger than the rate of the backward reaction

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12
Sme Calculator1 mark

Which is the correct Kc expression for the reaction between hydrogen and fluorine?


H2 (g) + F2 (g) ⇌ 2HF (g)

  • fraction numerator left square bracket HF right square bracket squared over denominator left square bracket straight H subscript 2 right square bracket space left square bracket straight F subscript 2 right square bracket end fraction

  • fraction numerator left square bracket HF right square bracket over denominator left square bracket straight H subscript 2 right square bracket space left square bracket straight F subscript 2 right square bracket end fraction

  • fraction numerator 2 space left square bracket HF right square bracket over denominator left square bracket straight H subscript 2 right square bracket space left square bracket straight F subscript 2 right square bracket end fraction

  • fraction numerator left square bracket straight H subscript 2 right square bracket space left square bracket straight F subscript 2 right square bracket over denominator left square bracket HF right square bracket squared end fraction

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13
Sme Calculator1 mark

The Kc expression for the following reaction between hydrogen and iodine is shown 

H2 (g) + I2 (g) ⇌ 2HI (g)

K subscript straight C equals fraction numerator left square bracket HI right square bracket squared over denominator left square bracket straight H subscript 2 right square bracket space left square bracket straight I subscript 2 right square bracket end fraction

At equilibrium there were 0.234 moles of HI, 0.150 moles of H2 and 0.025 moles of I2.


Which is the correct Kc expression for the reaction between hydrogen and fluorine?

  • 14.60

  • 62.4

  • 6.85 x 10-2

  • 1.60 x 10-2

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14
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Nitrosyl chloride decomposes into nitrogen monoxide and chlorine according to the following equation. The forward reaction is endothermic 

2NOCl (g) ⇌ 2NO (g) + Cl2 (g)


Which change in condition would change the value for Kc?

  • Decreasing the pressure

  • Adding a catalyst

  • Increasing the temperature

  • Increasing the pressure

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15
Sme Calculator1 mark

Which of the following rows correctly describes Kc and ΔG for a reaction where the products are favoured?

  Kc ΔG
A. > 1 < 1
B. > 1 < 0
C. > 0 > 0
D. > 0 > 1

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    16
    Sme Calculator    1 mark

    At 300 K, iron oxidises according to the following equation:

    2Fe (s) + 3 over 2O2 (g) ⇌ Fe2O3 (s)

    The standard Gibbs free energy change for this reaction is -743.05 kJ mol-1.

    The quantitative relationship between the standard Gibbs free energy change, temperature and the equilibrium constant is:

    ΔG = –RT ln K

    What is the correct value of ln K?

    (R = 8.31 J K–1 mol–1)

    • 6.41 x 10-3

    • 3.36 x 10-3

    • 2.98 x 10-1

    • 2.98 x 102

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    11 mark

    Which systems are correctly described? 

    1. Matter and energy can be transferred across the boundary of an open system
    2. Only matter can be transferred across the boundary of a closed system
    3. Matter and energy cannot be transferred across the boundary of an isolated system

    • I and II only

    • I and III only 

    • II and III only 

    • I, II and III

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    21 mark

    Ethyne and hydrogen are formed from methane and a dynamic equilibrium is established.

    2CH4 (g)  ⇌   3H2 (g) +   C2H2 (g)                                                 

    What are the units for Kc?

    • mol dm-3

    • mol2 dm-6

    • mol3 dm-9

    • mol4 dm-12

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    31 mark

    The dissociation of gas X2Y4 into XY2 is represented in the equation below:

    X2Y4 (g)  ⇌  2XY2 (g)         straight capital delta straight H to the power of straight theta = +60 kJ mol-1 

    At constant pressure, if the temperature of the equilibrium mixture of the gases is increased, will the volume of the mixture increase or decrease and why?

    • the volume will increase, but only because of a shift of equilibrium towards the right 

    • the volume will increase, both because of a shift of equilibrium towards the right and also because of thermal expansion 

    • the volume will stay the same because any thermal expansion could be exactly counteracted by a shift of equilibrium towards the left

    • the volume will decrease because a shift of equilibrium towards the left would more than counteract any thermal expansion 

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    41 mark

    The reaction between nitrogen and hydrogen produces ammonia gas:

    N2 (g) + 3H2 (g)  rightwards harpoon over leftwards harpoon  2NH3 (g)

    If the equilibrium constant for the reaction is x, what is the equilibrium constant for the following reaction?

    2N2 (g) + 6H2 (g)  rightwards harpoon over leftwards harpoon  4NH3 (g)

    • x

    • 2x

    • x2

    • 2x2

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    51 mark

    For the following reaction at equilibrium

    H2S (aq)  +  Mg2+ (aq)  ⇋   MgS (s)   +  2H+ (aq)              ΔH < 0

    Which of the following changes will result in more MgS being produced?

    • Adding sodium hydroxide

    • Decreasing the pressure

    • Adding a catalyst

    • Increasing the temperature

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    61 mark

    When a chemical reaction reaches equilibrium which of the following can be said about the concentrations of the substances present, and the rates of reaction?

     

    Concentrations of the reactants and products

    Rates of forward and backward reactions

    A

    Continue to change

    Remain the same

    B

    Remain constant

    Remain the same

    C

    Continue to change

    Are different

    D

    Remain constant

    Are different

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      71 mark

      The Haber process is used to produce ammonia industrially by the following reaction

      N2 (g)  +  3H2 (g)  rightwards harpoon over leftwards harpoon  2NH3 (g)

      Which statements explain why a catalyst is used?

      I

      A catalyst lowers the activation energy
      II

      A catalyst moves the position of equilibrium towards the product
      III

      A catalyst allows the same rate to be achieved at a lower temperature

      • I and II only 

      • I and III only 

      • II and III only 

      • I, II and III

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      81 mark

      Study the following equilibrium reaction and determine which of the changes listed below will shift the equilibrium to the right hand side.

      2CO2 (g)   rightwards harpoon over leftwards harpoon  2CO (g)   +   O2 (g)

      I

      using a catalyst
      II

      reducing the oxygen concentration
      III

      increasing the volume of the container

      • I and II only 

      • I and III only 

      • II and III only 

      • I, II and III

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      91 mark

      Which of the following conclusions can be made about this reaction?

      H2O (g)   ⇋   H2 (g)   + 1 halfO2 (g)            Kc = 8 x 10-41 at 25 degreeC

      • The reaction does not proceed

      • The reaction goes almost to completion

      • The products have a higher concentration than the reactants

      • The concentrations of reactants and products are the same.

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      101 mark

      The value of Kc at 298K for the following reaction is 4.0. The reaction takes several days to react in equilibrium at room temperature.

      CH3COOH (l) +   CH3CH2OH (l)  ⇋  CH3COOCH2CH3 (l)   +  H2O (l)

      A student carried out the reaction shown and a day later measured the concentrations and calculated a value for the reaction quotient, Q. She found that the value of Q was 8.7.

      This value tells you that:

      • The reaction has not reached equilibrium and is moving left to right.

      • The reaction has not reached equilibrium and is moving right to left.

      • The reaction has reached equilibrium, but there are more products than reactants.

      • The reaction has reached equilibrium, but there are more reactants than products.

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      111 mark

      In the equilibrium reaction shown

      2ICl (l)   ⇋    I2 (g)   +   Cl2 (g)     ΔHᶿ = -26 kJ

      What will change if the temperature is lowered?

       

      The position of equilibrium

      The value of Kc

      A

      will shift to the right

      decreases

      B

      will shift to the right

      increases

      C

      will shift to the left

      decreases

      D

      will shift to the left

      increases

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        121 mark

        Which of these processes are endothermic?

        I.  Condensing

        II. Subliming

        III. Melting

        • I and II only

        • I and III only

        • II and III only

        • I, II and III

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        131 mark

        When gaseous dinitrogen pentoxide, N2O5 (g), decomposes at 358 K, the following equilibrium is established:

        2N2O5 (g)  ⇌ 4NO2 (g) + O2 (g)

        2.0 mol of N2O5 (g) were placed in a 1.0 dm3 container and allowed to reach equilibrium. At equilibrium 1.0 mol of N2O5 (g) were present. What is the value of Kc?

        • 0.125

        • 1

        • 2

        • 8

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        141 mark

        Consider the following reversible reaction:

        3O2 (g) ⇌ 2O3 (g) 

        What is the value of Kc when the equilibrium concentrations are [O2] = 4.0 mol dm-3 and [O3] = 4.0 mol dm-3 ?

        • 0.25

        • 4

        • 16

        • 64

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        151 mark

        Which if the following will shift the position of equilibrium to the right in the reaction  shown? 

        2N2O5 (g)  ⇌ 4NO2 (g) + O2 (g)     ΔH = +219.2 kJ 

        1.  Decreasing the concentration of NO2 (g)
        2.  Decreasing the temperature
        3.  Decreasing the pressure

        • I and II only

        • I and III only

        • II and III only 

        • I, II and III

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        161 mark

        Hydrogen iodide decomposes to form hydrogen and iodine vapour.

        2HI (g)  ⇌ H2 (g) + I2 (g)

        What is the effect of decreasing the volume of the equilibrium mixture at constant temperature?

        • The amount of H2 (g) remains the same but its concentration decreases

        • The forward reaction is favoured

        • The backward reaction is favoured

        • The value of Kc  remains unchanged

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        171 mark

        A mixture of 0.40 mol of SO2 (g) and 0.40 mol of O2 (g) was placed in a 1 dm3 container. The following equilibrium took place:

        2SO2 (g)  + O2 (g) ⇌  2SO3 (g) 

        At equilibrium the mixture contained 0.25 mol of O2 (g) .How many moles of SO2 (g) and SO3 (g) were present at equilibrium?

         

        SO2 (g) / mol

        SO3 (g) / mol

        A

        0.25

        0.15

        B

        0.30

        0.15

        C

        0.10

        0.30

        D

        0.25

        0.30

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          11 mark

          Study the following equilibrium reaction and determine which of the statements must be true.

          2X    ⇋   Y               Kc = 1.1

          • [X] ≫ [Y]

          • [X] ＞[Y]

          • [X] = [Y]

          • [X] ＜ [Y]

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          21 mark

          Hydrogen reacts with iodine according to the following equation

          H2 (g)  + I2 (g)   ⇋   2HI (g)

          The value of Kc for this reaction has been measured at different temperatures

          Kc  =  60  at 355 degreeC

          Kc  =  47  at 450 degreeC

          From the information given which of the following must be true?

          • The reaction is exothermic

          • The reaction is endothermic

          • The reaction barely proceeds at 355 degreeC

          • The reaction almost goes to completion at 450 degreeC

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          31 mark

          The following Kc values were obtained for a reaction carried out at different temperatures, T1 to T4.

          Temperature

          Kc value

          T1

          1 x 10-2

          T2

          1 x 101

          T3

          1

          T4

          1 x 102


          Which of the following gives the correct amount of products in the mixtures from least to most?

          • T1 ＜T2 ＜T3＜T4

          • T4 ＜T3 ＜T2＜T1

          • T4 ＜T2 ＜T3＜T1

          • T1 ＜T3 ＜T2＜T4

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          41 mark

          Which of the following conditions and reasons will increase the amount of hydrogen iodide produced?

          H2 (g)  + I2 (g)   ⇋   2HI (g)              ΔHᶿ = -126 kJ

           

          Condition

          Reason

          Condition

          Reason

          A

          increase T

          exothermic reaction

          increase P

          two gaseous reactants but only one gaseous product

          B

          increase T

          endothermic reaction

          no change in P

          equal numbers of moles of gases

          C

          decrease T

          exothermic reaction

          decrease P

          two moles of gaseous product but only one mole of each gaseous reactant

          D

          decrease T

          exothermic reaction

          no change in P

          equal numbers of moles of gases

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            51 mark

            The blood-red complex iron (III) thiocynanate, [FeSCN]2+ is formed when iron (III) ions react with thiocyanate ions in the following equilibrium reaction:

             Fe3+ (aq) + SCN- (aq) ⇋ [FeSCN]2+    ΔHᶿ = +12 kJ
            yellow    colourless    red    


            Which of the following changes would make the solution go darker?

            I

            raising the temperature of the solution
            II

            adding iron(III) chloride solution
            III

            adding a catalyst

            • I and II only 

            • I and III only 

            • II and III only 

            • I, II and III

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            61 mark

            Which of the following features is not a characteristic of a state of equilibrium?

            • Equilibrium is dynamic

            • Equilibrium is achieved in a closed system

            • Concentrations of reactants and products are equal

            • Equilibrium can be reached from either direction

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            71 mark

            What is the relationship between Kc1 and Kc2 in the following reactions?

            2NOBr (g)  ⇋   2NO (g)   +  Br2 (g)   Kc1

            NO (g)   +  1 halfBr2 (g) ⇋  NOBr (g)   Kc2

            • 2Kc2 = Kc1

            • (Kc2)2 = Kc1

            • Kc2 = fraction numerator 1 over denominator square root of K subscript straight c 1 end subscript end root end fraction

            • Kc2 = fraction numerator 1 over denominator 2 K subscript c 1 end subscript end fraction

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            81 mark

            Nitrogen dioxide can react with itself to produce a dimer molecule called dinitrogen tetroxide in the following equilibrium reaction.

            2NO2 (g)    ⇋  N2O4 (g)      Kc  = 0.01 at 25 degreeC

            In an experiment, 100 cm3 of nitrogen dioxide is placed in a gas syringe and the barrel is pushed in, meaning the volume is reduced to 50 cm3 at constant temperature.

            Which of the following statements are true?

            1. The value of Kc increases
            2. More N2O4 is formed
            3. The ratio of begin mathsize 14px style fraction numerator left square bracket NO subscript 2 right square bracket over denominator left square bracket straight N subscript 2 straight O subscript 4 right square bracket end fraction end style decreases

            • I and II only

            • I and III only

            • II and III only

            • I, II and III

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            91 mark

            One of the characteristics of a state of equilibrium, is that equilibria are said to be dynamic. What is the meaning of dynamic in this context?

            • The position of equilibrium is constantly changing

            • The rates of forward and backward reactions change

            • The reactants and products are continually reacting

            • The concentrations of the reactants and products continue to change

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            101 mark

            The reaction shown below has a value of Kc = 1.0 x 10-4 at 25 degreeC.

            2NOBr (g)   ⇌    2NO (g)   +  Br2 (l)

            Which of the following relationships is correct about this equilibrium at 25 degreeC?

            • [NO] ≫ [NOBr]

            • [NOBr] ≫ [Br2]

            • 2 x [NOBr] = [Br2]

            • [NO] = [NOBr]

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            11
            Sme Calculator            1 mark

            The Haber process is a key step in the manufacture of fertilisers:

            N2 (g) + 3H2 (g) rightwards harpoon over leftwards harpoon 2NH3 (g)         ΔH = -ve

            Which is correct about the effect of increasing temperature for this reaction?

              Effect on equilibrium position Effect on Kc
            A. Shifts left No change
            B. Shifts right No change
            C. Shifts right Increase
            D. Shifts left Decrease

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              12
              Sme Calculator              1 mark

              Which equation represents a reaction where the number of moles alone can not be used to calculate the value of Kc?

              • CH3CH2OH (aq) + CH3COOH (aq) rightwards harpoon over leftwards harpoon CH3CH2OCOCH3 (aq)  + H2O (l)

              • H2 (g) + I2 (g) rightwards harpoon over leftwards harpoon 2HI (g)

              • 2SO2 (g) + O2 (g) rightwards harpoon over leftwards harpoon 2SO3 (g)

              • N2 (g) + O2 (g) rightwards harpoon over leftwards harpoon 2NO (g)

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              13
              Sme Calculator              1 mark

              When 0.20 mol NO, 0.08 mol H2 and 0.10 mol of H2O are placed in a 1.0 dm3 flask, the following equilibrium is established:

              2NO (g) + 2H2 (g) rightwards harpoon over leftwards harpoon N2 (g) + 2H2O (g)

              At equilibrium, the concentration of H2 (g) was found to be 0.02 mol dm-3.

              What is the correct value of Kc?

              • 1.02 x 10-2

              • 98.0

              • 8.3

              • 489.8

              Choose your answer

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              14
              Sme Calculator              1 mark

              Nitrogen dioxide can form a dimer that can also break back down again as part of a reversible reaction:

              N2O4 (g) rightwards harpoon over leftwards harpoon NO2 (g)         ΔH = +ve

              The reaction reaches an equilibrium at temperature T, where Kc = 1

              What is true for a higher temperature, T2?

                Kc value ΔGθ value
              A. Increases Increases
              B. Decreases Increases
              C. Decreases Decreases
              D. Increases Decreases

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                15
                Sme Calculator                1 mark

                Which would be the correct way to plot a graph and then calculate ΔGθ from experimental data of Kc and temperature values?

                ΔGθ = -RT ln K

                  y-axis x-axis ΔGθ =
                A. 1 / T ln K -R x gradient
                B. ln K 1 / T -R x gradient
                C. ln K 1 / T R / gradient
                D. 1 / T ln K R / gradient

                  Choose your answer

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