JEE Questions for Chemistry Thermodynamics Quiz 10 - MCQExams.com


Chemistry-Thermodynamics-8923.png
  • A = S, B = R, C = Q, D = P
  • A = P, B = Q, C = R, D = S
  • A = R, B = S, C = Q, D = P
  • A = S, B = R, C = P, D = Q
Statement–1 : The enthalpy of formation of H2O(l) is greater than of H2O (g).
Statement–2: Enthalpy change is negative for the condensation reaction H2O (g) → H2O(l)
  • Statement –1 is true, Statement –2 is true.Statement –2 is the correct explanation for statement –1
  • Statement –1 is true,Statement –2 is true.Statement –2 is not the correct explanation for statement –1
  • Statement –1 is true, Statement –2 is False
  • Statement –1 is false Statement –2 is True
Statement–1 : Heat of neutralisation of perchloric acid, HClO3, with NaOH is same as that of HCl with NaOH.
Statement–2: Both HCl and HClO4 are strong acids.
  • Statement –1 is true, Statement –2 is true.Statement –2 is the correct explanation for statement –1
  • Statement –1 is true,Statement –2 is true.Statement –2 is not the correct explanation for statement –1
  • Statement –1 is true, Statement –2 is False
  • Statement –1 is false Statement –2 is True
Statement–1 : When a gas at high pressure expands against vacuum, the work done is maximum.
Statement–2: Work done in expansion depends upon the pressure inside the gas and increase
  • Statement –1 is true, Statement –2 is true.Statement –2 is the correct explanation for statement –1
  • Statement –1 is true,Statement –2 is true.Statement –2 is not the correct explanation for statement –1
  • Statement –1 is true, Statement –2 is False
  • Statement –1 is false Statement –2 is True
Statement–1 : In the following reaction :C(s) + O2 (g) → CO2 (g); ∆H = ∆U – RT
Statement–2: ∆H is related to U by the equation, ∆H = ∆U – ∆ng RT
  • Statement –1 is true, Statement –2 is true.Statement –2 is the correct explanation for statement –1
  • Statement –1 is true,Statement –2 is true.Statement –2 is not the correct explanation for statement –1
  • Statement –1 is true, Statement –2 is False
  • Statement –1 is false Statement –2 is True
Statement I : The chemical reaction, 3H2(g) + N2(g) → 2NH3 shows decrease in entropy.
Statement II: The process passes into equilibrium state when ∆GT,P becomes zero.
  • Statement –1 is true, Statement –2 is true.Statement –2 is the correct explanation for statement –1
  • Statement –1 is true,Statement –2 is true.Statement –2 is not the correct explanation for statement –1
  • Statement –1 is true, Statement –2 is False
  • Statement –1 is false Statement –2 is True
Statement I : Both H and U are state functions.
Statement II: Absolute values of H or U can be determined
  • Statement –1 is true, Statement –2 is true.Statement –2 is the correct explanation for statement –1
  • Statement –1 is true,Statement –2 is true.Statement –2 is not the correct explanation for statement –1
  • Statement –1 is true, Statement –2 is False
  • Statement –1 is false Statement –2 is True
Calculate the work performed when 2 moles of hydrogen expand isothermally and reversibly at 25ºC form 15 to 50 litres.
  • –1438 Cal
  • –1436 cal
  • –1348 cal
  • –1346 cal
The ∆Hf0 for CO2(g), CO(g) and H2O (g) are –393.5, –110.5 and –241.8 kJ mol–1 respectively. The standard enthalpy change (in kJ) for the reaction CO2(g) + H2(g) → CO(g) + H2O (g) is –
  • 524.1
  • 41.2
  • – 262.5
  • – 41.2
For reaction carried out in automobiles, what is the value of ∆H, ∆S and ∆G ? 2C8H18(g) + 25O2(g) 16CO2(g)+ 18H2O(g)
  • +, –, +
  • –, + , –
  • –, +, +
  • +, +, –

Chemistry-Thermodynamics-8925.png
  • +9197.5
  • –9197.5
  • +771
  • –771.6
The conversion A to B is carried out by the following path :
Given : ∆S(A → C) = 50 e.u. , ∆S(C → D) = 30 e.u. , ∆S(B → D) = 20 e.u.
Where e.u. is entropy unit then ∆S(A → B) is
Chemistry-Thermodynamics-8927.png
  • +100 e.u.
  • + 60 e.u.
  • –100 e.u.
  • – 60 e.u.
For the chemical reaction A + B → P + Q two paths are given in the diagram. Which of the following relationship is correct –
Chemistry-Thermodynamics-8928.png
  • ∆H1 + ∆H2 = ∆H3 + ∆H4
  • ∆H1 + ∆H2 = ∆H3 – ∆H4
  • ∆H3 – ∆H1 = ∆H4 – ∆H2
  • ∆H1 – ∆H2 = ∆H3 + ∆H4

Chemistry-Thermodynamics-8929.png
  • –289 kJ mol–1
  • – 124 kJ mol–1
  • + 124 kJ mol–1
  • +289 kJ mol–1
The value of ∆Hºf of U3O8 is –853.5 KJ mol–1. Also ∆Hº for the reaction 3UO2 + O2 → U3O8, is –76.00 KJ. The value of ∆Hºf of UO2 is approx –
  • –259.17 KJ
  • –310.17 KJ
  • + 259.17 KJ
  • 930.51 KJ
The heat produced by complete neutralisation of 100 ml of HNO3 with 300 ml of decimolar KOH solution is 1.713 kJ. The morality of HNO3 solution will be –
  • 0.1
  • 1
  • 0.3
  • 0.5
The heats of neutralisation of four acids a, b, c and d when neutralised against a common strong base are 13.7, 9.4, 11.2 and 12.4 Kcal respectively. The weakest among the acids is
  • a
  • b
  • c
  • d
A gas is allowed to expand at constant pressure from a volume to 1.0 litre to 10.0 litre against an external pressure of 0.50 atm. If the gas absorbs 250J of heat the surroundings, what are the values of q, w and ∆E ? (Given 1 L atm = 101 J)
  • q = 250 J, w = –455J, ∆E = – 205J
  • q = – 250J, w = –455 J, ∆E = – 710J
  • q = 250J, w = 455J, ∆E = 710J
  • q = – 250J, w = 455J, ∆E = 250J
The enthalpy of the reaction H2O2(l) → H2O(l) + ½ O2 (g) is –23.5 Kcal mol–1. The enthalpy of formation of H2O2(l) is
  • –44.8 Kcal mol–1
  • 44.8 Kcal mol–1
  • –91.8 Kcal mol–1
  • 91.8 Kcal mol–1
The work done by the system in a cyclic process involving one mole of an ideal monoamotic gas is –50 KJ / cycle. The heat absorbed by the system per cycle is
  • Zero
  • 50KJ
  • - 50KJ
  • 250 KJ
9.0 gm of H2O is vaporised at 100oC and 1 atm pressure. If the latent heat of vaporisation of water is xJ/gm, then ∆S is given by

  • Chemistry-Thermodynamics-8930.png
  • 2)
    Chemistry-Thermodynamics-8931.png

  • Chemistry-Thermodynamics-8932.png

  • Chemistry-Thermodynamics-8933.png
Equal volumes of monoatomic and diatomic gases at same initial temperature and pressure are mixed. The ratio of specific heats of the mixture (CP/Cv) will be
  • 1
  • 2
  • 1.67
  • 1.5

Chemistry-Thermodynamics-8935.png
  • 816.15 KJ
  • 1632.3 KJ
  • 6528.2 KJ
  • 2448.45 KJ
A cylinder of gas is assumed to contain 11.2 kg of butane (C4H10). If a normal family needs 20000KJ of energy per day. The cylinder will last : (Given that for combustion of butane is –2658 KJ)
  • 20 days
  • 25 days
  • 26 days
  • 24 days
Which expression is correct for the work done in adiabatic reversible expansion of an ideal gas

  • Chemistry-Thermodynamics-8937.png
  • 2)
    Chemistry-Thermodynamics-8938.png

  • Chemistry-Thermodynamics-8939.png

  • Chemistry-Thermodynamics-8940.png
Calculate ∆Go for a reaction having standard free energy change of NO2, NO and O3 as 12.39 20.72 and 39.06 Kcal/mole
  • 47.39
  • 47.38
  • 4.739
  • –4.739
The equilibrium concentration of the species in the reaction A + B = C + D are 3, 5, 10 and 15 mole L–1 respectively at the for the reaction is
  • 13.81
  • –1381.8
  • –138.18
  • 1391.6
The standard Gibbs free energy change ∆Go is related to equilibrium constant KP as

  • Chemistry-Thermodynamics-8942.png
  • 2)
    Chemistry-Thermodynamics-8943.png

  • Chemistry-Thermodynamics-8944.png

  • Chemistry-Thermodynamics-8945.png
In the reaction for the transition of carbon in the diamond from to carbon in the graphite from, ∆H is –453.5 cal. This points out that
  • Graphite is chemically different from diamond
  • Graphite is as stable as diamond
  • Graphite is more stable than diamond
  • Diamond is more stable than graphite
Which of the following is correct ?
  • 1 cal > 1 erg > 1 joule
  • 1 erg > 1 cal > 1 joule
  • 1 cal > 1 joule > 1 erg
  • 1 joule > 1 cal > 1 erg
When two moles of water is boiled at 100o C temperature which gets converted to vapour same temperature. Then what will be change in entropy of system ?
  • 25.12
  • 52.12
  • 21.76
  • 217.6
Heat of vapourisation of benzene is 7350 calorie K–1 mol–1. Calculate the change in entropy to convert 1 mole gaseous benzene to liquid benzene at 77o C
  • 21 calories K–1 mol–1
  • –21 calorie K–1 mol–1
  • –21 calorie K–1
  • 21 Calorie K–1
What is the value of Go at 25oC for the reaction having equilibrium constant 4.0?
C2H5OH + CH3COOHCH3COOC2H5 + H2O
  • –82.11
  • + 82.11
  • + 821.1
  • –821.1
Standard cell potential of electro chemical cell is 1.20 volt for given reaction. Calculate change in free energy in KJ associated with it
Chemistry-Thermodynamics-8948.png
  • 115.8
  • –115.8
  • –231.6
  • 231.6
In reaction X → y ∆H = 4 kcal/mol and ∆S = 10 cal/mol K–1 then at what temperature reaction will be spontaneously ?
  • 500 K
  • 350 K
  • 200 K
  • 250 K
For the reaction A + B = C, the values of standard free energy charge for A, B and C are –10, –15 and –25K. cal mol–1 respectively, then what is the value of equilibrium constant ?
  • Zero
  • One
  • More than one
  • Less than one
If is the change in enthalpy and the change in internal energy accompanying a gaseous reaction
  • ∆H is always greater than
  • ∆H < ∆E only if the number of moles of the products in greater than the number of the reactants
  • ∆H is always less than ∆E
  • ∆H < ∆E only if the number of moles of the products is less than the number of moles of the reactants
A schematic plot of versus inverse of temperature for a reaction is shown below. The reaction must be
Chemistry-Thermodynamics-8952.png
  • Exothermic
  • Endothermic
  • One with neligible enthalpy change
  • Highly spontaneous at ordinary temperature at ordinary temperature
The heat of reaction at constant pressure is given by

  • Chemistry-Thermodynamics-8953.png
  • 2)
    Chemistry-Thermodynamics-8954.png

  • Chemistry-Thermodynamics-8955.png

  • Chemistry-Thermodynamics-8956.png
2.2016 gm of acetaldehyde produced 13.95 kcal of heat on combustion in O2. Calculate the heat of combustion of CH3CHO
  • 279 Kcal
  • 972 Kcal
  • 27.9 Kcal
  • 2.79 Kcal

Chemistry-Thermodynamics-8958.png

  • Chemistry-Thermodynamics-8959.png
  • 2)
    Chemistry-Thermodynamics-8960.png

  • Chemistry-Thermodynamics-8961.png

  • Chemistry-Thermodynamics-8962.png

Chemistry-Thermodynamics-8963.png
  • -14.6 kJ mol-1
  • -16.8 kJ mol-1
  • +16.8 kJ mol-1
  • +244.8 kJ mol-1

Chemistry-Thermodynamics-8965.png
  • ∆H1 < ∆H2
  • ∆H1 + ∆H2 = 0
  • ∆H1 > ∆H2
  • ∆H1 = ∆H2
Consider the following Ellingham's diagram for carbon.
Chemistry-Thermodynamics-8966.png
  • Upto 710°C, the reaction of formation of CO2 is energetically more favourable but above 710°C, the formation of CO is preferred
  • Carbon can be used to reduce any metal oxide at a sufficiently high temperature
  • Carbon reduces many oxides at elevated temperature because ∆G° vs temperature line has a negative slope

  • Chemistry-Thermodynamics-8967.png
The incorrect expression among the following is

  • Chemistry-Thermodynamics-8969.png
  • 2)
    Chemistry-Thermodynamics-8970.png

  • Chemistry-Thermodynamics-8971.png

  • Chemistry-Thermodynamics-8972.png
∆G for the reaction Ag2O→ 2Ag + 1⁄2 O2 at a certain temperature is found to be -10.0 kJ mol-1 , which one of the following statements is correct at this temperature ?
  • Silver oxide decomposes to give silver and oxygen
  • Silver and oxygen combine to form silver oxide
  • The reaction is in equilibrium
  • The reaction can neither occur in the forward direction nor in the backward direction

Chemistry-Thermodynamics-8975.png
  • - 209 kJ
  • - 2259 kJ
  • + 2259 kJ
  • 209 kJ
For the reaction CO(g ) + 1⁄2 O2(g) → CO2 (g), ∆H and ∆S are - 283 kJ, - 87 JK-1 , respectively. It was intended to carry out this reaction at 1000, 1500, 3000 and 3500 K. At which of these temperatures would this reaction be thermodynamically spontaneous ?
  • 1500 and 3500 K
  • 3000 and 3500 K
  • 1000, 1500 and 3000 K
  • 1500, 3000 and 3500 K
  • At all the above temperatures
The entropy change for the reaction
H2 + Cl2 (g) → 2HCl (g) will be
[ Given that, S° (HCl ) = 187 JK-1 mol-1
S° (H2) = 131 JK-1 mol-1 and
S° (Cl2 ) = 223 JK-1 mol-1 ]
  • 20 JK-1 mol-1
  • - 20 JK-1 mol-1
  • 167 JK-1 mol-1
  • - 167 JK-1 mol-1
Which one of the following is spontaneous at all temperatures ?
  • H2 (g) → 2H (atom); ∆H° = 436 kJ, ∆S° = 90.7 eu
  • 2)
    Chemistry-Thermodynamics-8976.png
  • 2NO2 (g) → N2O4 (g); ∆H° = -56.0 kJ, ∆S° = -17.7 eu

  • Chemistry-Thermodynamics-8977.png
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