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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.
| 5251. |
Standard molar enthalpy of formation of \[C{{O}_{2}}\] is equal to [IIT JEE 1997; BHU 2001] |
| A. | Zero |
| B. | The standard molar enthalpy of combustion of gaseous carbon |
| C. | The sum of standard molar enthalpies of formation of \[CO\] and \[{{O}_{2}}\] |
| D. | The standard molar enthalpy of combustion of carbon (graphite) |
| Answer» E. | |
| 5252. |
\[C+\frac{1}{2}{{O}_{2}}\to CO;\,\Delta H=-42\,kJ\] \[CO+\frac{1}{2}{{O}_{2}}\to C{{O}_{2}};\,\Delta H=-24\,kJ\] The heat of formation of \[C{{O}_{2}}\] is [CPMT 1996] |
| A. | ? 16 kJ |
| B. | + 66 kJ |
| C. | + 16 kJ |
| D. | ? 66 kJ |
| Answer» E. | |
| 5253. |
\[2.2016\,gm\] of acetaldehyde produced \[13.95\,kcal\] of heat on combustion in \[{{O}_{2}}\]. Calculate the heat of combustion of \[C{{H}_{3}}CHO\] [Bihar CEE 1995] |
| A. | 279 kcal |
| B. | 972 kcal |
| C. | 27.9 kcal |
| D. | 2.79 kcal |
| Answer» B. 972 kcal | |
| 5254. |
In an endothermic reaction, the value of \[\Delta H\] is [CBSE PMT 1999; AIIMS 1998; BHU 2000; MP PMT 2000] |
| A. | Zero |
| B. | Positive |
| C. | Negative |
| D. | Constant |
| Answer» C. Negative | |
| 5255. |
The heat of reaction at constant pressure is given by [MP PMT 1997] |
| A. | \[{{E}_{P}}-{{E}_{R}}\] |
| B. | \[{{E}_{R}}-{{E}_{P}}\] |
| C. | \[{{H}_{P}}-{{H}_{R}}\] |
| D. | \[{{H}_{R}}-{{H}_{P}}\] |
| Answer» D. \[{{H}_{R}}-{{H}_{P}}\] | |
| 5256. |
Enthalpy of formation of \[HF\] and \[HCl\] are \[-\,161\,kJ\] and \[-\,92\,kJ\] respectively. Which of the following statements is incorrect [KCET 2003] |
| A. | \[HCl\] is more stable than \[HF\] |
| B. | \[HF\] and \[HCl\] are exothermic compounds |
| C. | The affinity of fluorine to hydrogen is greater than the affinity of chlorine to hydrogen |
| D. | \[HF\] is more stable than \[HCl\] |
| Answer» B. \[HF\] and \[HCl\] are exothermic compounds | |
| 5257. |
The enthalpy of combustion of benzene from the following data will be (i) \[6C(s)+3{{H}_{2}}(g)\to {{C}_{6}}{{H}_{6}}(l);\,\Delta H=+45.9\,kJ\] (ii) \[{{H}_{2}}(g)+\frac{1}{2}{{O}_{2}}(g)\to {{H}_{2}}O(l);\,\Delta H=-285.9\,kJ\] (iii) \[C(s)+{{O}_{2}}(g)\to C{{O}_{2}}(g);\,\Delta H=-393.5\,kJ\] |
| A. | + 3172.8 kJ |
| B. | ? 1549.2 kJ |
| C. | ? 3172.8 kJ |
| D. | ? 3264.6 kJ |
| Answer» E. | |
| 5258. |
The heat change for the following reaction \[C(s)+2S(s)\to C{{S}_{2}}(l)\] is known as [MP PMT 1996] |
| A. | Heat of vaporization |
| B. | Heat of solution |
| C. | Heat of fusion |
| D. | Heat of formation |
| Answer» E. | |
| 5259. |
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 [NCERT 1978; MP PET 1990; JIPMER 2001] |
| A. | 816.15 kJ |
| B. | 1632.3 kJ |
| C. | 6528.2 kJ |
| D. | 2448.45 kJ |
| Answer» C. 6528.2 kJ | |
| 5260. |
When water is added to quick lime, the reaction is [MP PMT 1995] |
| A. | Exothermic |
| B. | Endothermic |
| C. | Explosive |
| D. | None of these |
| Answer» B. Endothermic | |
| 5261. |
Carbon and carbon monoxide burn in oxygen to form carbon dioxide according to the following reactions \[C+{{O}_{2}}\to C{{O}_{2}};\,\Delta H=-394\,kJ\,mo{{l}^{-1}}\] \[2CO+{{O}_{2}}\to 2C{{O}_{2}};\,\Delta H=-569\,kJ\,mo{{l}^{-1}}\] The heat of formation of \[1\,mol\]of carbon monoxide is thus [MP PET 1995] |
| A. | \[-219.0\,kJ\,mo{{l}^{-1}}\] |
| B. | \[-109.5\,kJ\,mo{{l}^{-1}}\] |
| C. | \[-175.0\,kJ\,mo{{l}^{-1}}\] |
| D. | \[-87.5\,kJ\,mo{{l}^{-1}}\] |
| Answer» C. \[-175.0\,kJ\,mo{{l}^{-1}}\] | |
| 5262. |
Heat of formation in the reaction \[{{H}_{2}}+C{{l}_{2}}\to 2HCl+44\,kcal\] is [MP PMT 1995] |
| A. | 44 kcal |
| B. | 44000 kcal |
| C. | 22 kcal |
| D. | 11 kcal |
| Answer» D. 11 kcal | |
| 5263. |
If enthalpies of formation of \[{{C}_{2}}{{H}_{4}}(g),\,C{{O}_{2}}(g)\] and \[{{H}_{2}}O(l)\] at \[{{25}^{o}}C\] and \[1\,atm\] pressure be 52, ? 394 and \[-286\,kJ\,mo{{l}^{-1}}\] respectively, the enthalpy of combustion of \[{{C}_{2}}{{H}_{4}}(g)\] will be [CBSE PMT 1995; AIIMS 1998; Pb. PMT 1999] |
| A. | \[+1412\,kJ\,mo{{l}^{-1}}\] |
| B. | \[-1412\,kJ\,mo{{l}^{-1}}\] |
| C. | \[+141.2\,kJ\,mo{{l}^{-1}}\] |
| D. | \[-141.2\,kJ\,mo{{l}^{-1}}\] |
| Answer» C. \[+141.2\,kJ\,mo{{l}^{-1}}\] | |
| 5264. |
Complete combustion of \[C{{H}_{4}}\] gives [BHU 1995] |
| A. | \[C{{O}_{2}}+{{H}_{2}}O\] |
| B. | \[C{{O}_{2}}+{{H}_{2}}\] |
| C. | \[COC{{l}_{2}}\] |
| D. | \[CO+C{{O}_{2}}+{{H}_{2}}O\] |
| Answer» B. \[C{{O}_{2}}+{{H}_{2}}\] | |
| 5265. |
In the combustion of \[2.0\,gm\] of methane \[25\,kcal\] heat is liberated, heat of combustion of methane would be [MP PMT 1994] |
| A. | \[100\,kcal\] |
| B. | \[200\,kcal\] |
| C. | \[300\,kcal\] |
| D. | \[400\,kcal\] |
| Answer» C. \[300\,kcal\] | |
| 5266. |
The energy evolved is highest for which of the following reactions [MP PET 1994] |
| A. | \[F+{{e}^{-}}\to {{F}^{-1}}\] |
| B. | \[Cl+{{e}^{-}}\to C{{l}^{-}}\] |
| C. | \[S+2{{e}^{-}}\to {{S}^{2-}}\] |
| D. | \[O+2{{e}^{-}}\to {{O}^{2-}}\] |
| Answer» C. \[S+2{{e}^{-}}\to {{S}^{2-}}\] | |
| 5267. |
For an exothermic reaction [MP PET 1994; Manipal MEE 1995] |
| A. | \[H\] of the products is less than \[H\] of the reactants |
| B. | \[H\] of the products is more than \[H\] of the reactants |
| C. | \[H\] of the products is equal to \[H\] of the reactants |
| D. | \[\Delta H\] is always positive |
| Answer» B. \[H\] of the products is more than \[H\] of the reactants | |
| 5268. |
An exothermic reaction is one in which the reacting substances [CPMT 1974, 79; Bihar MEE 1982; KCET 1992; JIPMER 2001] |
| A. | Have more energy than the products |
| B. | Have less energy than the products |
| C. | Are at a higher temperature than the product |
| D. | None of the above |
| Answer» B. Have less energy than the products | |
| 5269. |
For the allotropic change represented by equation \[C(diamond)\to C(graphite)\]; the enthalpy change is \[\Delta H=-1.89\,kJ\]. If \[6\,g\] of diamond and \[6\,g\] of graphite are separately burnt to yield carbon dioxide, the heat liberated in the first case is [KCET 1988; DPMT 2000] |
| A. | Less than in the second case by \[1.89\,kJ\] |
| B. | More than in the second case by \[1.89\,kJ\] |
| C. | Less than in the second case by \[11.34\,kJ\] |
| D. | More than in the second case by \[0.945\,kJ\] |
| Answer» E. | |
| 5270. |
Heat of transition is the heat evolved or absorbed when a substance is converted from [KCET 1984] |
| A. | Solid to liquid |
| B. | Solid to vapour |
| C. | Liquid to vapour |
| D. | One allotropic form to another allotropic form |
| Answer» E. | |
| 5271. |
Based on the following thermochemical equations \[{{H}_{2}}O(g)+C(s)\to CO(g)+{{H}_{2}}(g);\,\Delta H=131\,kJ\] \[CO(g)+\frac{1}{2}{{O}_{2}}(g)\to C{{O}_{2}}(g);\Delta H=-282\,kJ\] \[{{H}_{2}}(g)+\frac{1}{2}{{O}_{2}}(g)\to {{H}_{2}}O(g);\,\Delta H=-242\,kJ\] \[C(s)+{{O}_{2}}(g)\to C{{O}_{2}}(g);\,\Delta H=X\,kJ\] The value of \[X\] is [CBSE PMT 1992] |
| A. | \[-393\,kJ\] |
| B. | \[-\,655\,kJ\] |
| C. | \[+\,393\,kJ\] |
| D. | \[+655\,kJ\] |
| Answer» B. \[-\,655\,kJ\] | |
| 5272. |
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 [KCET 1990] |
| A. | \[21.16\,kJ\] |
| B. | \[-21.10\,kJ\] |
| C. | \[-13.62\,kJ\] |
| D. | \[13.6\,kJ\] |
| Answer» C. \[-13.62\,kJ\] | |
| 5273. |
Which of the following equations correctly represents the standard heat of formation \[(\Delta H_{f}^{o})\] of methane [IIT JEE (Screening) 1992] |
| A. | \[C(diamond)\,+2{{H}_{2}}(g)=C{{H}_{4}}(g)\] |
| B. | \[C(graphite)+2{{H}_{2}}(g)=C{{H}_{4}}(l)\] |
| C. | \[C(graphite)+2{{H}_{2}}(g)=C{{H}_{4}}(g)\] |
| D. | \[C(graphite)+4H=C{{H}_{4}}(g)\] |
| Answer» D. \[C(graphite)+4H=C{{H}_{4}}(g)\] | |
| 5274. |
Which of the following values of heat of formation indicates that the product is least stable [MP PMT 1991] |
| A. | \[-94\,kcal\] |
| B. | \[-\,231.6\,kcal\] |
| C. | \[+21.4\,kcal\] |
| D. | \[+\,64.8\,kcal\] |
| Answer» E. | |
| 5275. |
\[C\](diamond) \[+{{C}_{2}}(g)\to C{{O}_{2}}(g);\,\Delta H=-395\] kJ \[C\] (graphite) \[+{{O}_{2}}(g)\to C{{O}_{2}}(g);\,\Delta H=-393.5\] kJ From the data, the \[\Delta H\] when diamond is formed from graphite, is [CBSE PMT 1989; BHU 1987] |
| A. | \[-1.5\,kJ\] |
| B. | \[+\,1.5\,kJ\] |
| C. | \[+\,3.0\,kJ\] |
| D. | \[-3.0\,kJ\] |
| Answer» C. \[+\,3.0\,kJ\] | |
| 5276. |
The difference between heats of reaction at constant pressure and at constant volume for the reaction \[2{{C}_{6}}{{H}_{6}}(l)+15{{O}_{2}}(g)\to 12C{{O}_{2}}(g)+6{{H}_{2}}O(l)\]at \[{{25}^{o}}C\]in kJ is [IIT JEE 1991; Kerala PMT 2004] |
| A. | ?7.43 |
| B. | + 3.72 |
| C. | ?3.72 |
| D. | + 7.43 |
| Answer» B. + 3.72 | |
| 5277. |
The standard heats of formation in kcal \[mo{{l}^{-1}}\] of \[N{{O}_{2}}(g)\] and \[{{N}_{2}}{{O}_{4}}(g)\] are 8.0 and 2.0 respectively. The heat of dimerization of \[N{{O}_{2}}\] in \[kcal\] is \[2N{{O}_{2}}(g)={{N}_{2}}{{O}_{4}}(g)\] [NCERT 1983] |
| A. | 10.0 |
| B. | ? 6.0 |
| C. | ? 12.0 |
| D. | ? 14.0 |
| Answer» E. | |
| 5278. |
The molar neutralization heat for \[KOH\] and \[HN{{O}_{3}}\] as compared to molar neutralization heat of \[NaOH\] and \[HCl\] [MP PMT 1989] |
| A. | Less |
| B. | More |
| C. | Equal |
| D. | Depends on pressure |
| Answer» D. Depends on pressure | |
| 5279. |
In the combustion of hydrocarbons, \[\Delta H\] is [BHU 1981] |
| A. | Negative |
| B. | Zero |
| C. | Positive |
| D. | Undeterminate |
| Answer» B. Zero | |
| 5280. |
In the reaction for the transition of carbon in the diamond form to carbon in the graphite form, \[\Delta H\] is \[-453.5\,cal\]. This points out that [BHU 1981; KCET 1986, 89] |
| A. | Graphite is chemically different from diamond |
| B. | Graphite is as stable as diamond |
| C. | Graphite is more stable than diamond |
| D. | Diamond is more stable than graphite |
| Answer» D. Diamond is more stable than graphite | |
| 5281. |
The formation of water from \[{{H}_{2}}(g)\] and \[{{O}_{2}}(g)\] is an exothermic reaction because [MP PMT/PET 1988] |
| A. | The chemical energy of \[{{H}_{2}}(g)\] and \[{{O}_{2}}(g)\] is more than that of water |
| B. | The chemical energy of \[{{H}_{2}}(g)\] and \[{{O}_{2}}(g)\] is less than that of water |
| C. | Not dependent on energy |
| D. | The temperature of \[{{H}_{2}}(g)\] and \[{{O}_{2}}(g)\] is more than that of water |
| Answer» B. The chemical energy of \[{{H}_{2}}(g)\] and \[{{O}_{2}}(g)\] is less than that of water | |
| 5282. |
The heat of combustion of benzene determined in a bomb calorimeter is \[-870\,kcal\,mo{{l}^{-1}}\] at \[{{25}^{o}}C\]. The value of \[\Delta E\] for the reaction is |
| A. | \[-1740\,kcal\] |
| B. | \[-870\,kcal\] |
| C. | \[-872\,kcal\] |
| D. | \[-874\,kcal\] |
| Answer» C. \[-872\,kcal\] | |
| 5283. |
The enthalpy of formation of ammonia is \[-46.0\,kJ\,mo{{l}^{-1}}\]. The enthalpy change for the reaction \[2N{{H}_{3}}(g)\to 2{{N}_{2}}(g)+3{{H}_{2}}(g)\] is |
| A. | 46.0 kJ \[mo{{l}^{-1}}\] |
| B. | 92.0 kJ \[mo{{l}^{-1}}\] |
| C. | ? 23.0 kJ \[mo{{l}^{-1}}\] |
| D. | ? 92.0 kJ \[mo{{l}^{-1}}\] |
| Answer» C. ? 23.0 kJ \[mo{{l}^{-1}}\] | |
| 5284. |
Which of the following reaction can be used to define the heat of formation of \[C{{O}_{2}}(g)\] [MP PMT 1989; MH CET 2001] |
| A. | \[C\text{(graphite)}+{{O}_{2}}(g)=C{{O}_{2}}(g)\] |
| B. | \[C{{H}_{4}}(g)+2{{O}_{2}}(g)=C{{O}_{2}}(g)+2{{H}_{2}}O(l)\] |
| C. | \[CO(g)+\frac{1}{2}{{O}_{2}}(g)=C{{O}_{2}}(g)\] |
| D. | \[{{C}_{6}}{{H}_{6}}(l)+7\frac{1}{2}{{O}_{2}}(g)=6C{{O}_{2}}+3{{H}_{2}}O(l)\] |
| Answer» B. \[C{{H}_{4}}(g)+2{{O}_{2}}(g)=C{{O}_{2}}(g)+2{{H}_{2}}O(l)\] | |
| 5285. |
\[{{H}_{2}}+\frac{1}{2}{{O}_{2}}\to {{H}_{2}}O;\,\Delta H=-68.39\,kcal\] \[K+{{H}_{2}}O+\]Water \[\to KOH(aq)+\frac{1}{2}{{H}_{2}};\,\Delta H=-48\,kcal\] \[KOH+\]Water \[\to KOH(aq);\,\Delta H=-14\,kcal\] The heat of formation of \[KOH\] is (in kcal) [CPMT 1988] |
| A. | \[-68.39+48-14\] |
| B. | \[-68.39-48+14\] |
| C. | \[68.39-48+14\] |
| D. | 68.39 + 48 + 14 |
| Answer» C. \[68.39-48+14\] | |
| 5286. |
Which of the following statements is correct about heat of combustion [MADT Bihar 1982] |
| A. | It may be exothermic in some cases and endothermic in other cases |
| B. | It is applicable to gaseous substances only |
| C. | It is always an exothermic reaction |
| D. | Its value does not change with temperature |
| Answer» D. Its value does not change with temperature | |
| 5287. |
One of the phenomena which cannot be described as combustion is [EAMCET 1979] |
| A. | Oxidation of coal in air |
| B. | Burning of magnesium in nitrogen |
| C. | Reaction of antimony in chlorine |
| D. | Lighting of an electric lamp |
| Answer» E. | |
| 5288. |
Which of the following is an endothermic reaction [EAMCET 1980; MP PMT 1980; IIT JEE 1989; JIPMER 2002] |
| A. | \[2{{H}_{2}}+{{O}_{2}}\to 2{{H}_{2}}O\] |
| B. | \[{{N}_{2}}+{{O}_{2}}\to 2NO\] |
| C. | \[2NaOH+{{H}_{2}}S{{O}_{4}}\to N{{a}_{2}}S{{O}_{4}}+2{{H}_{2}}O\] |
| D. | \[3{{O}_{2}}+{{C}_{2}}{{H}_{5}}OH\to 2C{{O}_{2}}+3{{H}_{2}}O\] |
| Answer» C. \[2NaOH+{{H}_{2}}S{{O}_{4}}\to N{{a}_{2}}S{{O}_{4}}+2{{H}_{2}}O\] | |
| 5289. |
From Kirchhoff's equation which factor affects the heat of reaction [MP PMT 1990] |
| A. | Pressure |
| B. | Temperature |
| C. | Volume |
| D. | Molecularity |
| Answer» C. Volume | |
| 5290. |
A reaction that takes place with the absorption of energy is [EAMCET 1977] |
| A. | Burning of a candle |
| B. | Rusting of iron |
| C. | Electrolysis of water |
| D. | Digestion of food |
| Answer» D. Digestion of food | |
| 5291. |
If a chemical reaction is accompanied by the evolution of heat, it is [BHU 1979] |
| A. | Catalytic |
| B. | Photochemical |
| C. | Endothermic |
| D. | Exothermic |
| Answer» E. | |
| 5292. |
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 [EAMCET 1998] |
| A. | \[-4.0\,kcal\] |
| B. | \[+40\,kcal\] |
| C. | \[-80\,kcal\] |
| D. | \[+80\,kcal\] |
| Answer» D. \[+80\,kcal\] | |
| 5293. |
The heat of formation is the change in enthalpy accompanying the formation of a substance from its elements at 298 K and 1 atm pressure. Since the enthalpies of elements are taken to be zero, the heat of formation \[(\Delta H)\] of compounds [NCERT 1978; KCET 1993] |
| A. | Is always negative |
| B. | Is always positive |
| C. | May be negative or positive |
| D. | Is zero |
| Answer» D. Is zero | |
| 5294. |
All reactions with chemical dissociation are [MP PMT 1990] |
| A. | Reversible |
| B. | Reversible and endothermic |
| C. | Exothermic |
| D. | Reversible or irriversible and endothermic or exothermic |
| Answer» C. Exothermic | |
| 5295. |
Reaction, \[{{H}_{2}}(g)+{{I}_{2}}(g)\to 2HI(g)\] \[\Delta H=-12.40\,kcal\]. According to this, the heat of formation of HI will be [MP PET 1990] |
| A. | 12.4 kcal |
| B. | ? 12.4 kcal |
| C. | ? 6.20 kcal |
| D. | 6.20 kcal |
| Answer» D. 6.20 kcal | |
| 5296. |
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 \[HCl\] [CPMT 1990] |
| A. | \[22.5\,kJ\,mo{{l}^{-1}}\] |
| B. | \[57.1\,kJ\,mo{{l}^{-1}}\] |
| C. | \[14.3\,kJ\,mo{{l}^{-1}}\] |
| D. | \[28.6\,kJ\,mo{{l}^{-1}}\] |
| Answer» D. \[28.6\,kJ\,mo{{l}^{-1}}\] | |
| 5297. |
The lowest value of heat of neutralization is obtained for [KCET 1988; MP PMT 1990] |
| A. | \[HCl+NaOH\] |
| B. | \[C{{H}_{3}}COOH+N{{H}_{4}}OH\] |
| C. | \[N{{H}_{4}}OH+HCl\] |
| D. | \[NaOH+C{{H}_{3}}COOH\] |
| Answer» C. \[N{{H}_{4}}OH+HCl\] | |
| 5298. |
If \[{{H}^{+}}+O{{H}^{-}}\to {{H}_{2}}O+13.7\,kcal\], then the heat of neutralization for complete neutralization of one mole of \[{{H}_{2}}S{{O}_{4}}\] by base will be [MP PMT 1990] |
| A. | 13.7 kcal |
| B. | 27.4 kcal |
| C. | 6.85 kcal |
| D. | 3.425 kcal |
| Answer» B. 27.4 kcal | |
| 5299. |
The compound with negative heat of formation are known as [DPMT 1981] |
| A. | Endothermic compound |
| B. | Exothermic compound |
| C. | Heat of formation compound |
| D. | None of the above |
| Answer» C. Heat of formation compound | |
| 5300. |
If \[S+{{O}_{2}}\to S{{O}_{2}};\,(\Delta H=-298.2)\] \[S{{O}_{2}}+\frac{1}{2}{{O}_{2}}\to S{{O}_{3}};\,(\Delta H=-98.2)\] \[S{{O}_{3}}+{{H}_{2}}O\to {{H}_{2}}S{{O}_{4}};\,(\Delta H=-130.2)\] \[{{H}_{2}}+\frac{1}{2}{{O}_{2}}\to {{H}_{2}}O;\,(\Delta H=-287.3)\] then the enthalpy of formation of \[{{H}_{2}}S{{O}_{4}}\] at 298K will be [DPMT 1983; Orissa JEE 2005] |
| A. | \[-433.7\,kJ\] |
| B. | \[-650.3\,kJ\] |
| C. | \[+320.5\,kJ\] |
| D. | \[-813.9\,kJ\] |
| Answer» E. | |