JEE Questions for Chemistry Thermodynamics Quiz 7 - MCQExams.com

In a change from state A to state B
  • q depends only on the initial and final state
  • w depends only on the initial and final state
  • ∆E depends only on the initial and final state
  • ∆E depends upon the path adopted by A to change into B
For which of the following process will energy be absorbed?
  • Separating an electron from an electron
  • Separating a proton from a proton
  • Separating a neutron from a neutron
  • Separating an electron from a neutral atom.
For which reaction from the following, ∆S will be maximum ?

  • Chemistry-Thermodynamics-8818.png
  • 2)
    Chemistry-Thermodynamics-8819.png

  • Chemistry-Thermodynamics-8820.png

  • Chemistry-Thermodynamics-8821.png
When water is added to conc. H2SO4 it gets very hot. This happens because dilution of conc. H2SO4 is
  • an exothermic reaction
  • an endothermic reaction
  • photochemical reaction
  • hydrolytic reaction
A solution of 500 ml. of 0.2 M KOH and 500 ml of 0.2 M HCl is mixed and stirred; the rise in temperature is T1. The experiment is repeated using 250 ml each of solution, the temperature rise is T2. Which of the following is true?
  • T1 = T2
  • T1 = 2T2
  • T1 = 4T2
  • T2 = 9T1
Enthalpy of a reaction at 27oC is 15 kJ mol-1. The reaction will be feasible if entropy is
  • 15 J mol-1K-1
  • – 50 J mol-1 K-1
  • greater than 5 J mol-1 K-1
  • less than 50J mol-1K-1
The occurrence of reaction is impossible if
  • ∆H is +ve ; ∆S is also +ve
  • ∆H is –ve ; ∆S is also –ve
  • ∆H is –ve ; ∆S is +ve
  • ∆H is +ve ; ∆S is –ve
Heat of neutralisation of a strong acid and a strong base is nearly equal to
  • 10 kJ /mole
  • 10Cal/mole
  • -57KJ/mole
  • -57Cal/mole
For the transition C (diamond) → C (graphite) ; ∆H = ‒ 1.5 kJ. It follows that
  • diamond is exothermic
  • graphite is endothermic
  • graphite is stabler than diamond
  • diamond is stabler than graphite
Which of the following is an endothermic reaction?
  • 2H2 + O2 → 2H2O
  • N2 + O2 → 2NO
  • 2NaOH + H2SO4 → Na2SO4 + 2H2O
  • C2H5OH + 3O2 → 2CO2 + 3H2O
The heat released when NH4OH and HCl neutralise is
  • 13.7 kcal
  • >13.7 kcal
  • < 13.7 kcal
  • none of the above

Chemistry-Thermodynamics-8823.png
  • ∆H1 > ∆H2
  • ∆H1 = ∆H2
  • ∆H1 < ∆H2
  • ∆H1 + ∆H2 = 0
For which one of the following reactions will there be a +ve ∆S ?
  • H2O(g) → H2O(l)
  • H2 + I2 → 2HI
  • CaCO3(s) → CaO(s) + CO2(g)
  • N2(g) + 3H2(g) →2NH3(g)
In which of the following reactions does the heat change represent the heat of formation of water?

  • Chemistry-Thermodynamics-8824.png
  • 2)
    Chemistry-Thermodynamics-8825.png

  • Chemistry-Thermodynamics-8826.png

  • Chemistry-Thermodynamics-8827.png
For the spontaniety of a reaction which statement is true?
  • ∆G = +ive ; ∆H = +ive
  • ∆H = +ive ; ∆S = ‒ive
  • ∆G = ‒ive ; ∆S = ‒ive
  • ∆H = ‒ive ; ∆S = +ive
Which of the following equations correctly represents the standard heat of formation (∆Hof ) of methane?
  • C (diamond) + 2H2(g) = CH4(g)
  • C (graphite) + 2H2(g) = CH4(l)
  • C (graphite) + 2 H2(g) = CH4(g)
  • C (graphite) + 4H = CH4(g)
The enthalpy change (- ∆H) for the neutralisation of 1 MHCl by caustic potash in dilute solution at 298 K is
  • 68 kJ
  • 65 kJ
  • 57.3 kJ
  • 50 kJ
At constant T and P which one of the following statements is correct for the reaction ?
S8(s) + 8O2(g) → 8SO2(g)
  • ∆H < ∆E
  • ∆H = ∆E
  • ∆H > ∆E
  • ∆H is independent of the physical state of the reactants.
Gibb’s free energy G, enthalpy H and entropy S are related to one another by
  • G = H + TS
  • G = H – TS
  • G – TS = H
  • S = H – G
Consider the following reaction occurring in an automobile 2C8H18(g) + 25O2(g) → 16CO2 + 18H2O(g) the sign of ∆H, ∆S and ∆G would be
  • +, ‒, +
  • ‒, +, ‒
  • ‒, +, +
  • +, +, ‒
Compounds with high heat of formation are less stable because
  • High temperature is required to synthesise them
  • Molecules of such compounds are distorted
  • It is difficult to synthesis them
  • Energy rich state leads to instability
The heat of neutralization of aqueous hydrochloric acid by NaOH is x kcal/mole of HCl. Calculate the heat of neutralisation per mole of aqueous acetic acid.
  • 0.5 x kcal
  • x kcal
  • 2x kcal
  • cannot be calculated from the given data
Heat of neutralisation of strong acid against strong base is constant and is equal to
  • 13.7 kcal
  • 57 kJ
  • 5.7 × 104 J
  • All of the above
The heat of formation of the compound in the following reaction is H2g + Cl2g → 2HCl(g) + 44 kcal
  • ‒ 44 kcal mol-1
  • ‒ 22 kcal mol-1
  • 11 kcal mol-1
  • ‒ 88 kcal mol-1
Heat capacity is

  • Chemistry-Thermodynamics-8829.png
  • 2)
    Chemistry-Thermodynamics-8830.png

  • Chemistry-Thermodynamics-8831.png
  • None of these
Enthalpy of a reaction ∆H is expressed as

  • Chemistry-Thermodynamics-8832.png
  • 2)
    Chemistry-Thermodynamics-8833.png

  • Chemistry-Thermodynamics-8834.png

  • Chemistry-Thermodynamics-8835.png
The standard Gibb’s free energy change, ∆Go is related to equilibrium constant, Kp as

  • Chemistry-Thermodynamics-8837.png
  • 2)
    Chemistry-Thermodynamics-8838.png

  • Chemistry-Thermodynamics-8839.png

  • Chemistry-Thermodynamics-8840.png

Chemistry-Thermodynamics-8842.png

  • Chemistry-Thermodynamics-8843.png
  • 2)
    Chemistry-Thermodynamics-8844.png

  • Chemistry-Thermodynamics-8845.png

  • Chemistry-Thermodynamics-8846.png
The relation between enthalpy (H), pressure (P), volume (V) and internal energy (E) is given by
  • E = H + PV
  • H = E + PV
  • H = E - PV
  • H = E + P + V
For which of the process, ∆S is negative ?
  • H2(g) → 2H(g)
  • N2(g 1 atm) → N2(g8 atm)
  • 2SO3(g) → 2SO2(g) + O2(g)
  • C(diamond) → C(graphite)

Chemistry-Thermodynamics-8848.png
  • (y - 2x)
  • (2x + y)
  • (x + y)
  • (2x / y)
If an endothermic reaction is non-spontaneous at freezing point of water and becomes feasible at its boiling point, then
  • ∆H is –ve, ∆S is +ve
  • ∆H and ∆S both are +ve
  • ∆H and ∆S both are –ve
  • ∆H is +ve, ∆S is –ve
For the reaction C3H8(g) + 5O2(g) → 3CO2(g) + 4H2O(l) at constant temperature, ∆H – ∆E is
  • + RT
  • – 3 RT
  • + 3 RT
  • – RT
Which one of the following has ∆So greater than zero ?

  • Chemistry-Thermodynamics-8850.png
  • 2)
    Chemistry-Thermodynamics-8851.png

  • Chemistry-Thermodynamics-8852.png

  • Chemistry-Thermodynamics-8853.png
The internal energy change when a system goes from state A to B is 40 kJ/mole. If the system goes from A to B by a reversible path and returns to state A by an irreversible path, what would be the net change in internal energy ?
  • > 40 k J
  • < 40 kJ
  • zero
  • 40 kJ
In an irreversible process taking place at constant T and P and in which only pressure –volume work is being done, the change in Gibbs free energy (dG) and the change in entropy (ds) satisfy the criteria
  • (dS)V, E > 0, (dG)T, P < 0
  • (dS)V, E = 0, (dG)T, P = 0
  • (dS)V, E = 0, (dG)T, P > 0
  • (dS)V, E < 0, (dG)T, P < 0
Which of the following reaction defines ∆Hof ?

  • Chemistry-Thermodynamics-8854.png
  • 2)
    Chemistry-Thermodynamics-8855.png

  • Chemistry-Thermodynamics-8856.png

  • Chemistry-Thermodynamics-8857.png
The enthalpy of formation for C2H4 (g), CO2 (g) and H2O (l) at 25oC and 1 atm pressure are 52, -394 and -286 kJ mol-1 respectively. The enthalpy of combustion of C2H4(g) will be
  • +1412 kJ mol-1
  • -1412 kJ mol-1
  • +141.2 kJ mol-1
  • -141.2 kJ mol-1
The heat evolved in the combustion of glucose (C6H12O6) is given by the equation (C6H12O6)(s) + 6O2(g) →6CO2(g) + 6H2O(g),ΔH = -680 kcal. The weight of CO2(g) produced when 170 kcal of heat is evolved in the combustion of glucose is
  • 264 g
  • 66 g
  • 11g
  • 44g

Chemistry-Thermodynamics-8860.png
  • ‒ 814.4 kJ
  • +320.5 kJ
  • ‒ 650. 3 kJ
  • ‒ 933.7 kJ.
Given the following thermo chemical equations
Zn + 1/2O2 → ZnO + 84,000 cals
Hg + 1/2O2 → HgO + 21,700 cals
Then the heat of reaction for the following reaction Zn + HgO → ZnO + Hg Heat is
  • 105,700 cals
  • 61,000 cals
  • 105,000 cals
  • 60,000 cals
  • 62,300 cals

Chemistry-Thermodynamics-8863.png
  • 62.8 kcal
  • 31.4 kcal
  • ‒ 31.4 kcal
  • ‒ 84.2 kcal

Chemistry-Thermodynamics-8864.png
  • 836
  • 1460
  • ‒ 836
  • ‒ 1460
The difference between heats of reaction at constant pressure and constant volume for the reaction
Chemistry-Thermodynamics-8866.png
  • ‒ 7.43
  • +3.72
  • ‒ 3.72
  • + 7.43
Given the following entropy values ( in J K-1 mol-1)at 298 K and 1 atm: H2(g) : 130.6, Cl2(g) : 223.0 and HCl (g) : 186.7. The entropy change (in J K mol-1) for the reaction H2(g) + Cl2(g) → 2HCl(g) is
  • +540.3
  • +727.0
  • -166.9
  • 19.8
What is the entropy change (in JK-1 mol-1) when one mole of ice is converted into water at 0oC ? (The enthalpy change for the conversion of ice to liquid water is 6.0 kJ mol-1 at 0oC)
  • 20.13
  • 2.013
  • 2.198
  • 21.98
The densities of graphite and diamond at 298 K are 2.25 and 3.31 g cm-3 respectively. If the standard free energy difference (∆Go) is equal to 1895 J mol-1, the pressure at which graphite will be transformed into diamond at 298 K is
  • 9.92 × 108 Pa
  • 9.92 × 107 Pa
  • 9.92 × 106 Pa
  • 9.92 × 105 Pa
  • None of these
One gram sample Of NH4NO3 is decomposed in a bomb calorimeter. The temperature of the calorimeter increases by 6.12K. The heat capacity of the system is 1.23kJ/g/deg.What is the molar heat of decomposition for NH4NO3 ?
  • ‒ 7.53 kJ/mol
  • ‒ 398.1 kJ/mol
  • ‒ 16.1 kJ/mol
  • 602 kJ/mol

Chemistry-Thermodynamics-8872.png

  • Chemistry-Thermodynamics-8873.png
  • 2)
    Chemistry-Thermodynamics-8874.png

  • Chemistry-Thermodynamics-8875.png
  • none
The standard state Gibbs free energy change for the isomerization reaction cis-2-pentene trans-2- pentene is -3.67 kJ/mol at 400 K. If more trans-2-pentene is added to the reaction vessel, then
  • additional trans -2- pentene is formed
  • more cis -2-pentene is formed
  • equilibrium is shifted in the forward direction.
  • equilibrium remains unaffected.
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