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question_answer1)
Any series of operations so carried out that at the end, the system is back to its initial state is called
A)
Boyle's cycle done
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B)
Reversible process done
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C)
Adiabatic process done
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D)
Cyclic process done
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question_answer2)
Energy equivalent to one erg, one joule and one calorie is in the order
A)
\[1\,erg\,>\,1\,joule\,>\,1\,calorie\] done
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B)
\[1\,erg\,>\,1\,calorie\,>\,1\,joule\] done
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C)
\[1\,calorie\,>\,1\,joule\,>\,1\,erg\] done
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D)
\[1\,joule\,>\,1\,calorie\,>\,1\,erg\] done
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question_answer3)
In thermodynamics which one of the following is not an intensive property
A)
Pressure done
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B)
Density done
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C)
Volume done
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D)
Temperature done
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question_answer4)
At constant T and P, which one of the following statements is correct for the reaction, \[CO(g)+\frac{1}{2}{{O}_{2}}(g)\to C{{O}_{2}}(g)\]
A)
\[\Delta H\] is independent of the physical state of the reactants of that compound done
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B)
\[\Delta H\,>\,\Delta E\] done
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C)
\[\Delta H\,<\,\Delta E\] done
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D)
\[\Delta H=\Delta E\] done
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question_answer5)
Which of the following expressions represents the first law of thermodynamics
A)
\[\Delta E=-q+W\] done
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B)
\[\Delta E=q-W\] done
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C)
\[\Delta E=q+W\] done
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D)
\[\Delta E=-q-W\] done
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question_answer6)
According to Hesss law, the heat of reaction depends upon
A)
Initial condition of reactants done
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B)
Initial and final conditions of reactants done
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C)
Intermediate path of the reaction done
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D)
End conditions of reactants done
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question_answer7)
Internal energy is
A)
Partly potential and partly kinetic done
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B)
Totally kinetic done
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C)
Totally potential done
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D)
None of these done
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question_answer8)
Which of the following is zero during adiabatic expansion of the gas
A)
\[\Delta T\] done
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B)
\[\Delta S\] done
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C)
\[\Delta E\] done
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D)
None of these done
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question_answer9)
When the value of entropy is greater, then the ability of work
A)
Is maximum done
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B)
Is minimum done
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C)
Is medium done
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D)
None of these done
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question_answer10)
The volume of a gas decreases from \[500\,cc\] to \[300\,cc\] when a sample of gas is compressed by an average pressure of 0.6 atm. During this process 10 J of heat is liberated. The change in internal energy is
A)
- 2.16 J done
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B)
12.156 J done
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C)
2.16 J done
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D)
101.3 J done
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question_answer11)
For a carnot engine, the source is at \[500K\] and the sink at \[300K\]. What is efficiency of this engine
A)
0.2 done
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B)
0.4 done
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C)
0.6 done
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D)
0.3 done
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question_answer12)
The heat evolved in the combustion of benzene is given by |
\[{{C}_{6}}{{H}_{6}}+7\frac{1}{2}{{O}_{2}}\to 6C{{O}_{2}}(g)+3{{H}_{2}}O(l);\,\Delta H=-3264.6\,kJ\] |
Which of the following quantities of heat energy will be evolved when \[39\,g\,{{C}_{6}}{{H}_{6}}\] are burnt |
A)
816.15 kJ done
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B)
1632.3 kJ done
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C)
6528.2 kJ done
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D)
2448.45 kJ done
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question_answer13)
The enthalpy of neutralization is about 57.3 kJ for the pair
A)
\[HCl\] and \[N{{H}_{4}}OH\] done
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B)
\[N{{H}_{4}}OH\] and \[HN{{O}_{3}}\] done
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C)
\[HCl\] and \[NaOH\] done
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D)
\[C{{H}_{3}}COOH\] and \[NaOH\] done
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question_answer14)
The heat change for the reaction \[{{H}_{2}}+\frac{1}{2}{{O}_{2}}\to {{H}_{2}}O\] is called
A)
Heat of reaction done
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B)
Heat of formation done
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C)
Heat of vaporisation done
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D)
None of the above done
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question_answer15)
The heat of combustion of \[C{{H}_{4(g)}},\,{{C}_{(\text{graphite})}}\] and \[{{H}_{2(g)}}\] are \[20\,kcal,\,-40\,kcal\] and \[-10\,kcal\] respectively. The heat of formation of methane is
A)
\[-4.0\,kcal\] done
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B)
\[+40\,kcal\] done
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C)
\[-80\,kcal\] done
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D)
\[+80\,kcal\] done
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question_answer16)
Values of heats of formation for \[Si{{O}_{2}}\]and \[MgO\] are \[-48.4\] and \[-34.7\,kJ\] respectively. The heat of the reaction \[2Mg+Si{{O}_{2}}\to 2MgO+Si\] is
A)
\[21.16\,kJ\] done
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B)
\[-21.10\,kJ\] done
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C)
\[-13.62\,kJ\] done
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D)
\[13.6\,kJ\] done
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question_answer17)
In an endothermic reaction, the value of \[\Delta H\] is
A)
Zero done
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B)
Positive done
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C)
Negative done
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D)
Constant done
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question_answer18)
Combustion of glucose takes place according to the equation, |
\[{{C}_{6}}{{H}_{12}}{{O}_{6}}+6{{O}_{2}}\to 6C{{O}_{2}}+6{{H}_{2}}O\],\[\Delta H=-72\,kcal\]. |
How much energy will be required for the production of 1.6 g of glucose (Molecular mass of glucose = 180 g) |
A)
0.064 kcal done
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B)
0.64 kcal done
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C)
6.4 kcal done
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D)
64 kcal done
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question_answer19)
The following thermochemical reactions are given |
\[M+\frac{1}{2}{{O}_{2}}\,\,\to \,\,MO+351.4\,kJ\] |
\[X+\frac{1}{2}{{O}_{2}}\,\,\to \,\,XO+90.8\,kJ\] |
It follows that the heat of reaction for the following process \[M+XO\] \[\rightleftharpoons \] \[MO+X\] is given by |
A)
422.2 kJ done
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B)
268.7 kJ. done
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C)
- 442.2 kJ done
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D)
260.6 kJ done
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question_answer20)
One gram sample of \[N{{H}_{4}}N{{O}_{3}}\] is decomposed in a bomb calorimeter. The temperature of the calorimeter increases by 6.12 K the heat capacity of the system is 1.23 kJ/g/deg. What is the molar heat of decomposition for \[N{{H}_{4}}N{{O}_{3}}\]
A)
- 7.53 kJ/mol done
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B)
- 398.1 kJ/mol done
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C)
- 16.1 kJ/mol done
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D)
- 602 kJ/mol done
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question_answer21)
The bond dissociation energy needed to form benzyl radical from toluene is ..... than the formation of the methyl radical from methane
A)
Less done
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B)
Much done
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C)
Equal done
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D)
None of the above done
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question_answer22)
The \[H-H\] bond energy is 430 kJ \[mol\] and \[Cl-Cl\] bond energy is \[240\,kJ\,mo{{l}^{-1}}.\,\,\Delta H\] for \[HCl\] is \[-90\,kJ\]. The \[H-Cl\] bond energy is about
A)
\[180\,kJ\,mo{{l}^{-1}}\] done
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B)
\[360\,kJ\,mo{{l}^{-1}}\] done
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C)
\[213\,kJ\,mo{{l}^{-1}}\] done
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D)
\[425\,kJ\,mo{{l}^{-1}}\] done
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question_answer23)
The relation between \[\Delta G\] and \[\Delta H\] is
A)
\[\Delta H=\Delta G-T\,\Delta S\] done
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B)
\[\Delta G=\Delta H-T\,\Delta S\] done
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C)
\[T\,\Delta S-\Delta G=\Delta H\] done
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D)
\[\Delta H=T\,\Delta G+\Delta S\] done
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question_answer24)
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 change in entropy \[(dS)\], satisfy the criteria
A)
\[{{(dS)}_{V,\,E}}<0,\,{{(dG)}_{T,\,P}}<0\] done
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B)
\[{{(dS)}_{V,\,E}}>0,\,{{(dG)}_{T,\,P}}<0\] done
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C)
\[{{(dS)}_{V,\,E}}=0,\,{{(dG)}_{T,\,P}}=0\] done
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D)
\[{{(dS)}_{V,\,E}}=0,\,{{(dG)}_{T,\,P}}>0\] done
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question_answer25)
Gibbs free energy \[(G)\] is defined as
A)
\[\Delta G=\Delta H-T\Delta S\] done
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B)
\[\Delta G=\Delta H+\frac{T}{\Delta S}\] done
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C)
\[\Delta H=\Delta G-T\Delta S\] done
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D)
\[\Delta G=\Delta H+T.{{C}_{p}}\] done
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question_answer26)
For spontaneity of a cell, which is correct
A)
\[\Delta G=0,\,\Delta E=0\] done
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B)
\[\Delta G=-ve,\,\Delta E=0\] done
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C)
\[\Delta G=+ve,\,\Delta E=+ve\] done
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D)
\[\Delta G=-ve,\,\Delta E=+ve\] done
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question_answer27)
If a refrigerator's door is opened, then we get
A)
Room heated done
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B)
Room cooled done
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C)
More amount of heat is passed out done
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D)
No effect on room done
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question_answer28)
Which of the following is not a state function
A)
Internal energy done
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B)
Enthalpy done
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C)
Work done
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D)
Entropy done
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question_answer29)
Hess's law of constant heat summation in based on
A)
\[E=m{{c}^{2}}\] done
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B)
Conservation of mass done
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C)
First law of thermodynamics done
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D)
None of the above done
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question_answer30)
Joule-Thomson expansion is
A)
Isobaric done
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B)
Isoenthalpic done
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C)
Isothermal done
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D)
None of these done
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question_answer31)
At \[{{27}^{o}}C,\] one mole of an ideal gas is compressed isothermally and reversibly from a pressure of 2 atm to 10 atm. The values of \[\Delta E\] and q are \[(R=2)\]
A)
0, - 965.84 cal done
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B)
- 965.84 cal, + 965.84 cal done
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C)
+ 865.58 cal, - 865.58 cal done
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D)
- 865.58 cal, - 865.58 cal done
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question_answer32)
\[2C+{{O}_{2}}\to 2CO;\,\,\Delta H=-220\,kJ\] Which of the following statement is correct for this reaction
A)
Heat of combustion of carbon is 110 kJ done
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B)
Reaction is exothermic done
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C)
Reaction needs no initiation done
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D)
All of these are correct done
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question_answer33)
When disorder of a system increases, the change is said to be
A)
Exothermic done
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B)
Non-spontaneous done
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C)
Endothermic done
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D)
Spontaneous done
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question_answer34)
The enthalpy change for the transition of liquid water to steam, \[\Delta {{H}_{vap}}=37.3\,kJ\,mo{{l}^{-1}}\] at \[373\,K\]. The entropy change for the process is
A)
\[111.9\,J\,mo{{l}^{-1}}{{K}^{-1}}\] done
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B)
\[37.3\,J\,mo{{l}^{-1}}\,{{K}^{-1}}\] done
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C)
\[100\,J\,mo{{l}^{-1}}{{K}^{-1}}\] done
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D)
\[74.6\,J\,mo{{l}^{-1}}{{K}^{-1}}\] done
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question_answer35)
One mole of an ideal gas is allowed to expand reversibly and adiabatically from a temperature of \[{{27}^{o}}C\]. If the work done during the process is 3 kJ, the final temperature will be equal to \[({{C}_{v}}=20\,J{{K}^{-1}})\]
A)
150 K done
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B)
100 K done
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C)
\[{{26.85}^{o}}C\] done
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D)
295 K done
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question_answer36)
The molar heat capacity of water at constant pressure is \[75\,\,J{{K}^{-1}}mo{{l}^{-1}}\]. When 1.0 kJ of heat is supplied to 100 g of water which is free to expand the increase in temperature of water is
A)
6.6 K done
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B)
1.2 K done
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C)
2.4 K done
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D)
4.8 K done
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question_answer37)
The enthalpy of vapourization of a liquid is \[30\,kJ\,mo{{l}^{-1}}\] and entropy of vapourization is \[75\,J\,mo{{l}^{-1}}K\]. The boiling point of the liquid at 1 atm is
A)
250K0 done
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B)
400K done
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C)
450K done
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D)
600K done
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question_answer38)
An endothermic reaction is one in which
A)
Heat is converted into electricity done
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B)
Heat is absorbed done
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C)
Heat is evolved done
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D)
Heat is converted into mechanical work done
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question_answer39)
Heat of neutralisation for the given reaction \[NaOH+HCl\to NaCl+{{H}_{2}}O\] is \[57.1\,kJ\,mo{{l}^{-1}}\]. What will be the heat released when \[0.25\,mole\] of \[NaOH\] is titrated against \[0.25\,mole\] of \[HCl\]
A)
\[22.5\,kJ\,mo{{l}^{-1}}\] done
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B)
\[57.1\,kJ\,mo{{l}^{-1}}\] done
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C)
\[14.3\,kJ\,mo{{l}^{-1}}\] done
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D)
\[28.6\,kJ\,mo{{l}^{-1}}\] done
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question_answer40)
For the reaction \[A(g)+2B(g)\to 2C(g)+3D(g)\], the value of \[\Delta E\] at \[{{27}^{o}}C\] is 19.0 kcal. The value of \[\Delta H\] for the reaction would be \[(R=2.0\,cal\,{{K}^{-1}}mo{{l}^{-1}})\]
A)
20.8 kcal done
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B)
19.8 kcal done
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C)
18.8 kcal done
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D)
20.2 kcal done
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