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11th State Board Chemistry Equilibrium and Redox Reactions Important Questions Sep-30 , 2018

Important questions -chapter 7,8

11th State Board Chemistry Equilibrium and Redox Reactions Important Questions

Important questions -chapter 7,8

11th Standard

    Reg.No. :
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Chemistry

Use blue pen Only

Time : 01:00:00 Hrs
Total Marks : 55

    Part A

    Answer all the questions

    5 x 1 = 5

  1. Which among the following is an intensive property?

    (a)

    free energy

    (b)

    heat capacity

    (c)

    volume

    (d)

    molar volume

  2. Match the list I with list II and select the correct answer using the code given below the list.

    List-I List-II
    A ΔS<0 1 I2(s)⟶I2(g)
    B ΔG<0 2 \(Ice\overset { 273\quad K }{ \rightleftharpoons } Water\)
    C ΔG=0 3 2O3(g)⟶3O2(g)
    D ΔS>0 4 \(H_{ 2 }O_{ (I) }\overset { 270K }{ \longrightarrow } { H }_{ 2 }O_{ (s) }\)
    (a)
    A B C D
    1 2 3 4
    (b)
    A B C D
    3 4 1 2
    (c)
    A B C D
    1 2 4 3
    (d)
    A B C D
    4 3 2 1

  3. In general, for an exothermic reaction to be spontaneous:

    (a)

    temp should be high

    (b)

    temp should be zero

    (c)

    temp should be low

    (d)

    temp has no effect

  4. In the equilibrium,
    2A(g) ⇌ 2B(g) + C2(g)
    the equilibrium concentrations of A, B and C2 at 400 K are 1\(\times\)10–4 M, 2.0 \(\times\)10–3 M, 1.5 \(\times\)10–4 M respectively. The value of KC for the equilibrium at 400 K is ________

    (a)

    0.06

    (b)

    0.09

    (c)

    0.62

    (d)

    3 x 10-2

  5. In a chemical equilibrium, the rate constant for the forward reaction is 2.5 \(\times\)102 and the equilibrium constant is 50. The rate constant for the reverse reaction is ____________

    (a)

    11.5

    (b)

    5

    (c)

    2 x 102

    (d)

    2 x 10-3

    6. Part B

    Answer all the questions

    5 x 2 = 10

  6. Define the calorific value of food. What is the unit of calorific value?

  7. How do you measure the enthalpy of formation of carbon monoxide?

  8. Define System?

  9. What is the relation between KP and KC. Give one example for which KP is equal to KC.

  10. Consider the following reactions,
    H2(g) + I2(g) ⇌ 2 HI(g)
    In each of the above reaction find out whether you have to increase (or) decrease the volume to increase the yield of the product.

    11. Part C

    Answer all the questions

    5 x 3 = 15

  11. The equilibrium constant of a reaction is 10, what will be the sign of ΔG? Will this reaction be spontaneous?

  12. Applications of the heat of combustion?

  13. Define the Molar Heat of Sublimation

  14. The value of Kc for the following reaction at 717 K is 48.

  15. For the reaction
    SrCO3 (s) ⇌ SrO (s) + CO2(g),
    the value of equilibrium constant KP = 2.2 x 10–4 at 1002 K. Calculate KC for the reaction.

    16. Part D

    Answer all the questions

    5 x 5 = 25

  16. Calculate the entropy change of a process possessing ΔHt = 2090 J mole-1.

  17. Calculate the standard heat of formation of carbon di sulphide (l). Given that the standard heats of combustion of carbon (s), sulphur (s) and carbon di sulphide (l) are - 393.3, -293.72, and -1108. 76 kJ mol-1 respectively.

  18. Explain how heat absorbed at constant pressure is measured using coffee cup calorimeter with neat diagram.

  19. 1 mol of CH4, 1 mole of CS2 and 2 mol of H2S are 2 mol of H2 are mixed in a 500 ml flask. The equilibrium constant for the reaction KC = 4 x 10–2 mol2 lit–2. In which direction will the reaction proceed to reach equilibrium ?

  20. 28 g of Nitrogen and 6 g of hydrogen were mixed in a 1 litre closed container. At equilibrium 17 g NH3 was produced. Calculate the weight of nitrogen, hydrogen at equilibrium.

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