MCQOPTIONS
Saved Bookmarks
MCQOPTIONS
This section includes 11242 Mcqs, each offering curated multiple-choice questions to sharpen your Joint Entrance Exam - Main (JEE Main) knowledge and support exam preparation. Choose a topic below to get started.
| 5901. |
The free energy change for the following reactions are given below, \[{{C}_{2}}{{H}_{2}}(g)+\frac{5}{2}{{O}_{2}}(g)\,\to \]\[2C{{O}_{2}}(g)+{{H}_{2}}O(l);\,\Delta {{G}^{o}}=-1234\,kJ\] \[C(s)+{{O}_{2}}(g)\,\to C{{O}_{2}}(g)\,\,\Delta {{G}^{o}}=-394\,kJ\] \[{{H}_{2}}(g)+\frac{1}{2}{{O}_{2}}(g)\,\to \,{{H}_{2}}O(l)\,\,\,\Delta {{G}^{o}}=-237kJ\] What is the standard free energy change for the reaction \[{{H}_{2}}(g)+2\,C\,(s)\to {{C}_{2}}{{H}_{2}}(g)\] [Kerala (Med.) 2002] |
| A. | ? 209 kJ |
| B. | ? 2259 kJ |
| C. | + 2259 kJ |
| D. | 209 kJ |
| Answer» E. | |
| 5902. |
The equilibrium concentration of the species in the reaction \[A+B\equiv C+D\] are 3, 5, 10 and 15 \[mole\,{{L}^{-1}}\] respectively at \[300\,K\] the \[\Delta G\] for the reaction is [Pb. PMT 2004] |
| A. | 13.81 |
| B. | ? 1381.8 |
| C. | ? 138.18 |
| D. | 1391.6 |
| Answer» C. ? 138.18 | |
| 5903. |
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 \[(\Delta {{G}^{o}})\] is equal to 1895 J \[mo{{l}^{-1}}\], the pressure at which graphite will be transformed diamond at 298 K is [CBSE PMT 2003] |
| A. | \[9.92\times {{10}^{5}}Pa\] |
| B. | \[9.92\times {{10}^{8}}Pa\] |
| C. | \[9.92\times {{10}^{7}}Pa\] |
| D. | \[9.92\times {{10}^{6}}Pa\] |
| Answer» C. \[9.92\times {{10}^{7}}Pa\] | |
| 5904. |
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 [AIEEE 2003] |
| A. | \[{{(dS)}_{V,\,E}}<0,\,{{(dG)}_{T,\,P}}<0\] |
| B. | \[{{(dS)}_{V,\,E}}>0,\,{{(dG)}_{T,\,P}}<0\] |
| C. | \[{{(dS)}_{V,\,E}}=0,\,{{(dG)}_{T,\,P}}=0\] |
| D. | \[{{(dS)}_{V,\,E}}=0,\,{{(dG)}_{T,\,P}}>0\] |
| Answer» C. \[{{(dS)}_{V,\,E}}=0,\,{{(dG)}_{T,\,P}}=0\] | |
| 5905. |
For a spontaneous change, free energy change \[\Delta G\] is [MNR 1983; BHU 1981, 95; AMU 1999; DCE 2000, 01; BHU 2000; MP PMT 2003] |
| A. | Positive |
| B. | Negative |
| C. | Zero |
| D. | Can be positive or negative |
| Answer» C. Zero | |
| 5906. |
The essential condition for the feasibility of a reaction is that [JIPMER 2002] |
| A. | The reaction should be exothermic |
| B. | The entropy of products must be larger than that of reactants |
| C. | The reaction is to be accompanied with free energy decrease |
| D. | The reaction has to possess high activation energy |
| Answer» D. The reaction has to possess high activation energy | |
| 5907. |
The correct relationship between free energy change in a reaction and the corresponding equilibrium constant \[{{K}_{c}}\] is [AIEEE 2003] |
| A. | \[\Delta G=RT\ln {{K}_{c}}\] |
| B. | \[-\Delta G=RT\ln {{K}_{c}}\] |
| C. | \[\Delta {{G}^{o}}=RT\ln {{K}_{c}}\] |
| D. | \[-\Delta {{G}^{o}}=RT\ln {{K}_{c}}\] |
| Answer» E. | |
| 5908. |
Gibbs free energy G, enthalpy H and entropy S are interrelated as in [MP PMT 2002] |
| A. | \[G=H+TS\] |
| B. | \[G=H-TS\] |
| C. | \[G-TS=H\] |
| D. | \[G=S=H\] |
| Answer» C. \[G-TS=H\] | |
| 5909. |
Born-Haber cycle is used to determine [UPSEAT 2001] |
| A. | Crystal energy |
| B. | Electron affinity |
| C. | Lattice energy |
| D. | All of these |
| Answer» E. | |
| 5910. |
For a reaction at \[{{25}^{o}}C\] enthalpy change and entropy changes are \[-11.7\times {{10}^{3}}J\,mo{{l}^{-1}}\] and \[-105\,J\,mo{{l}^{-1}}{{K}^{-1}}\] respectively. What is the Gibbs free energy [BHU 2001] |
| A. | 15.05 kJ |
| B. | 19.59 kJ |
| C. | 2.55 kJ |
| D. | 22.55 kJ |
| Answer» C. 2.55 kJ | |
| 5911. |
The standard enthalpy of the decomposition of \[{{N}_{2}}{{O}_{4}}\] to \[N{{O}_{2}}\] is 58.04 kJ and standard entropy of this reaction is 176.7 J/K. The standard free energy change for this reaction at \[{{25}^{o}}C\] is [AIIMS 1999] |
| A. | 539 kJ |
| B. | ? 539 kJ |
| C. | ? 5.39 kJ |
| D. | 5.39 kJ |
| Answer» E. | |
| 5912. |
Spontaneity of a chemical reaction is decided by the negative change in [MP PET 2001] |
| A. | Internal energy |
| B. | Enthalpy |
| C. | Entropy |
| D. | Free energy |
| Answer» E. | |
| 5913. |
\[\Delta {{G}^{o}}\] for the reaction \[X+Y\]⇌ Z is ? 4.606 kcal . The value of equilibrium constant of the reaction at \[{{227}^{o}}C\] is \[(R=2.0\,cal.\,mo{{l}^{-1}}{{K}^{-1}})\] [Roorkee 1999] |
| A. | 100 |
| B. | 10 |
| C. | 2 |
| D. | 0.01 |
| Answer» B. 10 | |
| 5914. |
What is the free energy change \[\Delta G\] when \[1.0\,mole\] of water at \[{{100}^{o}}C\] and \[1\,atm\] pressure is converted into steam at \[{{100}^{o}}C\] and \[1\,atm\] pressure [MP PET/PMT 1998] |
| A. | \[540\,cal\] |
| B. | \[-9800\,cal\] |
| C. | \[9800\,cal\] |
| D. | \[0\,cal\] |
| Answer» E. | |
| 5915. |
For the change \[{{H}_{2}}O(l)\to {{H}_{2}}O(g);\,P=1\,atm\], \[T=373\,K\], the free energy change \[\Delta G=0\]. This indicates that |
| A. | \[{{H}_{2}}O(l)\] is in equilibrium with \[{{H}_{2}}O(g)\] |
| B. | Water boils spontaneously at \[373\,K\] |
| C. | Water does not boil spontaneously at \[373\,K\] |
| D. | Condensation of water vapour occurs spontaneously at \[373\,K\] |
| Answer» B. Water boils spontaneously at \[373\,K\] | |
| 5916. |
The free energy change for a reversible reaction at equilibrium is [NCERT 1984; Kurukshetra CEE 1998; AMU 1999] |
| A. | Large positive |
| B. | Small negative |
| C. | Small positive |
| D. | 0 |
| Answer» E. | |
| 5917. |
For the reaction \[{{N}_{2}}+3{{H}_{2}}\]⇌\[2N{{H}_{3}};\,\Delta H=\] [Roorkee 2000; CBSE PMT 1991, 2002] |
| A. | \[\Delta E-RT\] |
| B. | \[\Delta E-2RT\] |
| C. | \[\Delta E+RT\] |
| D. | \[\Delta E+2RT\] |
| Answer» C. \[\Delta E+RT\] | |
| 5918. |
The law of Lavoisier and Laplace illustrates [KCET 1989] |
| A. | The principle of conservation of energy |
| B. | Equivalence of mechanical and thermal energy |
| C. | The principle of conservation of matter |
| D. | Equivalence of mechanical and chemical energy |
| Answer» B. Equivalence of mechanical and thermal energy | |
| 5919. |
For the reaction of one mole of zinc dust with one mole of sulphuric acid in a bomb calorimeter, \[\Delta \text{U}\] and w correspond to [AIIMS 2005] |
| A. | \[\Delta \text{U}<0,\ w=0\] |
| B. | \[\Delta \text{U}=0,\ w<0\] |
| C. | \[\Delta \text{U}>0,\ w=0\] |
| D. | \[\Delta \text{U}<0,\ w>0\] |
| Answer» B. \[\Delta \text{U}=0,\ w<0\] | |
| 5920. |
Which is not the correct relation between enthalpy \[(\Delta H)\]and intrinsic energy \[(\Delta E)\] [EAMCET 1992] |
| A. | \[\Delta H=\Delta E+\,P\,\Delta V\] |
| B. | \[\Delta H\,=\,\Delta E\,+\,n\,RT\] |
| C. | \[\Delta H=\Delta E\,-\,P\,\Delta V\] |
| D. | \[\Delta E=\Delta H\,-\,P\,\Delta V\] |
| Answer» D. \[\Delta E=\Delta H\,-\,P\,\Delta V\] | |
| 5921. |
For the reaction, \[{{A}_{(s)}}+2{{B}_{(g)}}\to 4{{C}_{(s)}}+{{D}_{(l)}}\]. \[\Delta H\] and \[\Delta U\] are related as ??? [Orissa JEE 2004] |
| A. | \[\Delta H=\Delta U\] |
| B. | \[\Delta H=\Delta U+3RT\] |
| C. | \[\Delta H=\Delta U+RT\] |
| D. | \[\Delta H=\Delta U-3RT\] |
| Answer» E. | |
| 5922. |
For which of the reaction \[\Delta H=\Delta E\] [MP PET 2004] |
| A. | \[{{N}_{2}}+3{{H}_{2}}\]⇌\[2N{{H}_{3}}\] |
| B. | \[{{N}_{2}}+{{O}_{2}}\to 2NO\] |
| C. | \[2Na+C{{l}_{2}}\to 2NaCl\] |
| D. | \[PC{{l}_{5}}\to PC{{l}_{3}}+C{{l}_{2}}\] |
| Answer» C. \[2Na+C{{l}_{2}}\to 2NaCl\] | |
| 5923. |
The work done during the expansion of a gas from a volume of \[4d{{m}^{3}}\] to \[6d{{m}^{3}}\] against a constant external pressure of \[3atm\] is (\[1L\,atm\,=101.32\,J\]) [CBSE PMT 2004] |
| A. | + 304 J |
| B. | ?304 J |
| C. | ? 6 J |
| D. | ?608 J |
| Answer» E. | |
| 5924. |
Internal energy is [AFMC 2004] |
| A. | Partly potential and partly kinetic |
| B. | Totally kinetic |
| C. | Totally potential |
| D. | None of these |
| Answer» B. Totally kinetic | |
| 5925. |
An ideal gas expands in volume from \[1\times {{10}^{-3}}{{m}^{3}}\] to \[1\times {{10}^{-2}}{{m}^{3}}\] at 300 K against a constant pressure of \[1\times {{10}^{5}}N{{m}^{-2}}\]. The work done is [AIEEE 2004] |
| A. | 270 kJ |
| B. | ?900 kJ |
| C. | ?900 J |
| D. | 900 kJ |
| Answer» D. 900 kJ | |
| 5926. |
\[2C+{{O}_{2}}\to 2CO;\,\,\Delta H=-220\,kJ\] Which of the following statement is correct for this reaction [BVP 2004] |
| A. | Heat of combustion of carbon is 110 kJ |
| B. | Reaction is exothermic |
| C. | Reaction needs no initiation |
| D. | All of these are correct |
| Answer» C. Reaction needs no initiation | |
| 5927. |
For the gaseous reaction, \[{{N}_{2}}{{O}_{4}}\to 2N{{O}_{2}}\] [Pb. CET 2003] |
| A. | \[\Delta H<\Delta E\] |
| B. | \[\Delta H=\Delta E\] |
| C. | \[\Delta H=0\] |
| D. | \[\Delta H>\Delta E\] |
| Answer» E. | |
| 5928. |
Which of the following is correct regarding the internal energy of a substance [Pb. CET 2002] |
| A. | It is a state function |
| B. | It increases with increase in temperature |
| C. | It can be calculated by experiment |
| D. | It remains unaffected with change in temperature |
| Answer» B. It increases with increase in temperature | |
| 5929. |
One mole of an ideal gas is allowed to expand reversibly and adibatically from a temperature of \[{{27}^{o}}C\]. If the work done during the process is \[3\,kJ\], then final temperature of the gas is \[({{C}_{V}}=20\,J/K)\] [Pb. CET 2002] |
| A. | 100 K |
| B. | 150 K |
| C. | 195 K |
| D. | 255 K |
| Answer» C. 195 K | |
| 5930. |
At constant T and P, which one of the following statements is correct for the reaction, \[CO(g)+\frac{1}{2}{{O}_{2}}(g)\to C{{O}_{2}}(g)\] [AIIMS 1982, 83; KCET 1988; BHU 1995; MP PET 1997, 99] |
| A. | \[\Delta H\] is independent of the physical state of the reactants of that compound |
| B. | \[\Delta H\,>\,\Delta E\] |
| C. | \[\Delta H\,<\,\Delta E\] |
| D. | \[\Delta H=\Delta E\] |
| Answer» D. \[\Delta H=\Delta E\] | |
| 5931. |
\[\Delta {{E}^{o}}\] of combustion of isobutylene is \[-X\,kJ\,mo{{l}^{-1}}\]. The value of \[\Delta {{H}^{o}}\] is [DCE 2004] |
| A. | \[=\Delta {{E}^{o}}\] |
| B. | \[>\Delta {{E}^{o}}\] |
| C. | \[=0\] |
| D. | \[<\Delta {{E}^{o}}\] |
| Answer» E. | |
| 5932. |
Enthalpy \[(H)\] is equal to [MH CET 2004] |
| A. | Internal energy E |
| B. | Product of pressure (P) and volume (V) of gas |
| C. | Internal energy E+PV |
| D. | Work (W) done by a system |
| Answer» D. Work (W) done by a system | |
| 5933. |
For the reaction \[PC{{l}_{5}}(g)\to PC{{l}_{3}}(g)+C{{l}_{2}}(g)\] [MH CET 2004] |
| A. | \[\Delta H=\Delta E\] |
| B. | \[\Delta H>\Delta E\] |
| C. | \[\Delta H<\Delta E\] |
| D. | None of these |
| Answer» C. \[\Delta H<\Delta E\] | |
| 5934. |
If gas, at constant temperature and pressure expands then its [MH CET 2003] |
| A. | Entropy increases and then decreases |
| B. | Internal energy increases |
| C. | Internal energy remains the same |
| D. | Internal energy decreases |
| Answer» D. Internal energy decreases | |
| 5935. |
Work done during isothermal expansion of one mole of an ideal gas from 10 atom. to 1 atm at 300K is [BHU 2004] |
| A. | 4938.8 J |
| B. | 4138.8 J |
| C. | 5744.1 J |
| D. | 6257.2 J |
| Answer» D. 6257.2 J | |
| 5936. |
A system absorb 600J of heat and work equivalent to 300J on its surroundings. The change in internal energy is [Pb. PMT 2004] |
| A. | 300 J |
| B. | 400 J |
| C. | 500 J |
| D. | 600 J |
| Answer» B. 400 J | |
| 5937. |
The work done by a system is 8 joule, when 40 joule heat is supplied to it. What is the increase in internal energy of system [BHU 2001] |
| A. | 25 J |
| B. | 30 J |
| C. | 32 J |
| D. | 28 J |
| Answer» D. 28 J | |
| 5938. |
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 \[(R=2)\] [BHU 2001] |
| A. | 0, ? 965.84 cal |
| B. | ? 965.84 cal, + 965.84 cal |
| C. | + 865.58 cal, ? 865.58 cal |
| D. | ? 865.58 cal, ? 865.58 cal |
| Answer» B. ? 965.84 cal, + 965.84 cal | |
| 5939. |
One mole of an ideal gas is allowed to expand freely and adiabatically into vacuum until its volume has doubled. A statement which is not true concerning this expression is [Pb. PMT 1998] |
| A. | \[\Delta H=0\] |
| B. | \[\Delta S=0\] |
| C. | \[\Delta E=0\] |
| D. | \[W=0\] |
| Answer» E. | |
| 5940. |
For which of the following \[\Delta E=\Delta H\] [MP PET 2003] |
| A. | \[{{N}_{2}}{{O}_{4}}(g)\] ⇌ \[2N{{O}_{2}}(g)\] |
| B. | \[2S{{O}_{2}}(g)+{{O}_{2}}(g)\] ⇌ \[2S{{O}_{3}}(g)\] |
| C. | \[{{H}_{2}}(g)+C{{l}_{2}}(g)\] ⇌ \[2HCl(g)\] |
| D. | \[{{H}_{2}}(g)+\frac{1}{2}{{O}_{2}}(g)\] ⇌ \[{{H}_{2}}O(l)\] |
| Answer» D. \[{{H}_{2}}(g)+\frac{1}{2}{{O}_{2}}(g)\] ⇌ \[{{H}_{2}}O(l)\] | |
| 5941. |
The relation between \[\Delta E\] and \[\Delta H\] is [MP PET 1992; MP PMT 1996; MP PET/PMT 1998] |
| A. | \[\Delta H=\Delta E-P\,\Delta V\] |
| B. | \[\Delta H=\Delta E+P\,\Delta V\] |
| C. | \[\Delta E=\Delta V+\Delta H\] |
| D. | \[\Delta E=\Delta H+P\,\Delta V\] |
| Answer» C. \[\Delta E=\Delta V+\Delta H\] | |
| 5942. |
The value of \[\Delta H-\Delta E\] for the following reaction at \[{{27}^{o}}C\] will be \[2N{{H}_{3}}(g)\,\to \,{{N}_{2}}(g)+3{{H}_{2}}(g)\] [Kerala (Med.) 2002] |
| A. | \[8.314\times 273\times (-2)\] |
| B. | \[8.314\times 300\times (-2)\] |
| C. | \[8.314\times 27\times (-2)\] |
| D. | \[8.314\times 300\times (2)\] |
| Answer» E. | |
| 5943. |
According to Hess?s law, the heat of reaction depends upon [MP PMT 2003] |
| A. | Initial condition of reactants |
| B. | Initial and final conditions of reactants |
| C. | Intermediate path of the reaction |
| D. | End conditions of reactants |
| Answer» C. Intermediate path of the reaction | |
| 5944. |
For the reaction, \[{{C}_{3}}{{H}_{8}}(g)+5{{O}_{2}}(g)\to \,\,3C{{O}_{2}}(g)+4{{H}_{2}}O(l)\] at constant temperature, \[\Delta H-\Delta E\] is [CBSE PMT 2003] |
| A. | ? RT |
| B. | + RT |
| C. | ? 3RT |
| D. | + 3RT |
| Answer» D. + 3RT | |
| 5945. |
Hess law is based on [MH CET 2002] |
| A. | Law of conservation of mass |
| B. | Law of conservation of energy |
| C. | Enthalpy is a state function |
| D. | None of these |
| Answer» C. Enthalpy is a state function | |
| 5946. |
In a closed insulated container, a liquid is stirred with a paddle to increase its temperature. In this process, which of the following is true [CBSE PMT 2002] |
| A. | \[\Delta E=W=Q=0\] |
| B. | \[\Delta E\ne 0,\,Q=W=0\] |
| C. | \[\Delta E=W\ne 0,\,Q=0\] |
| D. | \[\Delta E=Q\ne 0,\,W=0\] |
| Answer» D. \[\Delta E=Q\ne 0,\,W=0\] | |
| 5947. |
For the reaction \[C{{H}_{3}}COOH(l)+2{{O}_{2}}(g)\] ⇌ \[2C{{O}_{2}}(g)+2{{H}_{2}}O(l)\] at \[{{25}^{o}}C\] and 1 atm. pressure, \[\Delta H=-874\,kJ.\] Then the change in internal energy \[(\Delta E)\] is ?. [Orissa JEE 2002] |
| A. | ? 874 kJ |
| B. | ? 871.53 kJ |
| C. | ? 876.47 kJ |
| D. | + 874 kJ |
| Answer» B. ? 871.53 kJ | |
| 5948. |
In an adiabatic expansion of an ideal gas [KCET (Med.) 2001; MH CET 2000] |
| A. | \[W=-\Delta E\] |
| B. | \[W=\Delta E\] |
| C. | \[\Delta E=0\] |
| D. | \[W=0\] |
| Answer» C. \[\Delta E=0\] | |
| 5949. |
In which of the following \[\Delta E=\Delta H\] [MP PMT 2001] |
| A. | \[{{N}_{2}}{{O}_{4}}(g)\] ⇌ \[2N{{O}_{2}}(g)\] |
| B. | \[2S{{O}_{2}}(g)+{{O}_{2}}(g)\] ⇌ \[2S{{O}_{3}}(g)\] |
| C. | \[{{H}_{2}}(g)+{{I}_{2}}(g)\] ⇌ \[2HI(g)\] |
| D. | \[{{H}_{2}}(g)+\frac{1}{2}{{O}_{2}}(g)\] ⇌ \[{{H}_{2}}O(l)\] |
| Answer» D. \[{{H}_{2}}(g)+\frac{1}{2}{{O}_{2}}(g)\] ⇌ \[{{H}_{2}}O(l)\] | |
| 5950. |
Joule-Thomson expansion is [JIPMER 2000] |
| A. | Isobaric |
| B. | Isoenthalpic |
| C. | Isothermal |
| D. | None of these |
| Answer» C. Isothermal | |