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Heat of reaction is the change in enthalpy or internal energy as represented by a balanced thermochemicalequation. The amount of energy released during a chemical change depends upon the state of reactantsand products, the conditions of pressure and volume at which reaction is carried out, and temperature.The variation of heat of reaction (ΔH or ΔE) with temperature is given as ΔH2 – ΔH1 = ΔCp [T2 – T1] or ΔE2– ΔE1 = ΔCv (T2 – T1). Standard heat enthalpy of elements in their most stable state is assumed to be zerowhereas standard heat enthalpy of compound is referred as heat of formation of that compound at 1 atmpressure and 25°C. Oxidation of N2 to N2O, NO, NO2 shows absorption of energy whereas heat of combustionof N2 is exothermic like other heat of combustion.Q. Which statements regarding the formation of NO and NO2respectively from N2and O2are correct:(A) Heat of formation of NO is exothermic(B) Heat of formation of NO2is exothermic(C) The oxidation of N2to NO and NO2is favoured at high temperature.(D) If heat of formation of NO and NO2are 21.55 and 8.50 kcal, heat of reaction forNO + ½O2→ NO2is -13.05 kcala)1,2b)3,4c)1,2,4d)1,2,3Correct answer is option 'B'. Can you explain this answer? for JEE 2024 is part of JEE preparation. The Question and answers have been prepared according to the JEE exam syllabus. Information about Heat of reaction is the change in enthalpy or internal energy as represented by a balanced thermochemicalequation. The amount of energy released during a chemical change depends upon the state of reactantsand products, the conditions of pressure and volume at which reaction is carried out, and temperature.The variation of heat of reaction (ΔH or ΔE) with temperature is given as ΔH2 – ΔH1 = ΔCp [T2 – T1] or ΔE2– ΔE1 = ΔCv (T2 – T1). Standard heat enthalpy of elements in their most stable state is assumed to be zerowhereas standard heat enthalpy of compound is referred as heat of formation of that compound at 1 atmpressure and 25°C. Oxidation of N2 to N2O, NO, NO2 shows absorption of energy whereas heat of combustionof N2 is exothermic like other heat of combustion.Q. Which statements regarding the formation of NO and NO2respectively from N2and O2are correct:(A) Heat of formation of NO is exothermic(B) Heat of formation of NO2is exothermic(C) The oxidation of N2to NO and NO2is favoured at high temperature.(D) If heat of formation of NO and NO2are 21.55 and 8.50 kcal, heat of reaction forNO + ½O2→ NO2is -13.05 kcala)1,2b)3,4c)1,2,4d)1,2,3Correct answer is option 'B'. Can you explain this answer? covers all topics & solutions for JEE 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for Heat of reaction is the change in enthalpy or internal energy as represented by a balanced thermochemicalequation. The amount of energy released during a chemical change depends upon the state of reactantsand products, the conditions of pressure and volume at which reaction is carried out, and temperature.The variation of heat of reaction (ΔH or ΔE) with temperature is given as ΔH2 – ΔH1 = ΔCp [T2 – T1] or ΔE2– ΔE1 = ΔCv (T2 – T1). Standard heat enthalpy of elements in their most stable state is assumed to be zerowhereas standard heat enthalpy of compound is referred as heat of formation of that compound at 1 atmpressure and 25°C. Oxidation of N2 to N2O, NO, NO2 shows absorption of energy whereas heat of combustionof N2 is exothermic like other heat of combustion.Q. Which statements regarding the formation of NO and NO2respectively from N2and O2are correct:(A) Heat of formation of NO is exothermic(B) Heat of formation of NO2is exothermic(C) The oxidation of N2to NO and NO2is favoured at high temperature.(D) If heat of formation of NO and NO2are 21.55 and 8.50 kcal, heat of reaction forNO + ½O2→ NO2is -13.05 kcala)1,2b)3,4c)1,2,4d)1,2,3Correct answer is option 'B'. Can you explain this answer?.

Solutions for Heat of reaction is the change in enthalpy or internal energy as represented by a balanced thermochemicalequation. The amount of energy released during a chemical change depends upon the state of reactantsand products, the conditions of pressure and volume at which reaction is carried out, and temperature.The variation of heat of reaction (ΔH or ΔE) with temperature is given as ΔH2 – ΔH1 = ΔCp [T2 – T1] or ΔE2– ΔE1 = ΔCv (T2 – T1). Standard heat enthalpy of elements in their most stable state is assumed to be zerowhereas standard heat enthalpy of compound is referred as heat of formation of that compound at 1 atmpressure and 25°C. Oxidation of N2 to N2O, NO, NO2 shows absorption of energy whereas heat of combustionof N2 is exothermic like other heat of combustion.Q. Which statements regarding the formation of NO and NO2respectively from N2and O2are correct:(A) Heat of formation of NO is exothermic(B) Heat of formation of NO2is exothermic(C) The oxidation of N2to NO and NO2is favoured at high temperature.(D) If heat of formation of NO and NO2are 21.55 and 8.50 kcal, heat of reaction forNO + ½O2→ NO2is -13.05 kcala)1,2b)3,4c)1,2,4d)1,2,3Correct answer is option 'B'. Can you explain this answer? in English & in Hindi are available as part of our courses for JEE. Download more important topics, notes, lectures and mock test series for JEE Exam by signing up for free.

Here you can find the meaning of Heat of reaction is the change in enthalpy or internal energy as represented by a balanced thermochemicalequation. The amount of energy released during a chemical change depends upon the state of reactantsand products, the conditions of pressure and volume at which reaction is carried out, and temperature.The variation of heat of reaction (ΔH or ΔE) with temperature is given as ΔH2 – ΔH1 = ΔCp [T2 – T1] or ΔE2– ΔE1 = ΔCv (T2 – T1). Standard heat enthalpy of elements in their most stable state is assumed to be zerowhereas standard heat enthalpy of compound is referred as heat of formation of that compound at 1 atmpressure and 25°C. Oxidation of N2 to N2O, NO, NO2 shows absorption of energy whereas heat of combustionof N2 is exothermic like other heat of combustion.Q. Which statements regarding the formation of NO and NO2respectively from N2and O2are correct:(A) Heat of formation of NO is exothermic(B) Heat of formation of NO2is exothermic(C) The oxidation of N2to NO and NO2is favoured at high temperature.(D) If heat of formation of NO and NO2are 21.55 and 8.50 kcal, heat of reaction forNO + ½O2→ NO2is -13.05 kcala)1,2b)3,4c)1,2,4d)1,2,3Correct answer is option 'B'. Can you explain this answer? defined & explained in the simplest way possible. Besides giving the explanation of Heat of reaction is the change in enthalpy or internal energy as represented by a balanced thermochemicalequation. The amount of energy released during a chemical change depends upon the state of reactantsand products, the conditions of pressure and volume at which reaction is carried out, and temperature.The variation of heat of reaction (ΔH or ΔE) with temperature is given as ΔH2 – ΔH1 = ΔCp [T2 – T1] or ΔE2– ΔE1 = ΔCv (T2 – T1). Standard heat enthalpy of elements in their most stable state is assumed to be zerowhereas standard heat enthalpy of compound is referred as heat of formation of that compound at 1 atmpressure and 25°C. Oxidation of N2 to N2O, NO, NO2 shows absorption of energy whereas heat of combustionof N2 is exothermic like other heat of combustion.Q. Which statements regarding the formation of NO and NO2respectively from N2and O2are correct:(A) Heat of formation of NO is exothermic(B) Heat of formation of NO2is exothermic(C) The oxidation of N2to NO and NO2is favoured at high temperature.(D) If heat of formation of NO and NO2are 21.55 and 8.50 kcal, heat of reaction forNO + ½O2→ NO2is -13.05 kcala)1,2b)3,4c)1,2,4d)1,2,3Correct answer is option 'B'. Can you explain this answer?, a detailed solution for Heat of reaction is the change in enthalpy or internal energy as represented by a balanced thermochemicalequation. The amount of energy released during a chemical change depends upon the state of reactantsand products, the conditions of pressure and volume at which reaction is carried out, and temperature.The variation of heat of reaction (ΔH or ΔE) with temperature is given as ΔH2 – ΔH1 = ΔCp [T2 – T1] or ΔE2– ΔE1 = ΔCv (T2 – T1). Standard heat enthalpy of elements in their most stable state is assumed to be zerowhereas standard heat enthalpy of compound is referred as heat of formation of that compound at 1 atmpressure and 25°C. Oxidation of N2 to N2O, NO, NO2 shows absorption of energy whereas heat of combustionof N2 is exothermic like other heat of combustion.Q. Which statements regarding the formation of NO and NO2respectively from N2and O2are correct:(A) Heat of formation of NO is exothermic(B) Heat of formation of NO2is exothermic(C) The oxidation of N2to NO and NO2is favoured at high temperature.(D) If heat of formation of NO and NO2are 21.55 and 8.50 kcal, heat of reaction forNO + ½O2→ NO2is -13.05 kcala)1,2b)3,4c)1,2,4d)1,2,3Correct answer is option 'B'. Can you explain this answer? has been provided alongside types of Heat of reaction is the change in enthalpy or internal energy as represented by a balanced thermochemicalequation. The amount of energy released during a chemical change depends upon the state of reactantsand products, the conditions of pressure and volume at which reaction is carried out, and temperature.The variation of heat of reaction (ΔH or ΔE) with temperature is given as ΔH2 – ΔH1 = ΔCp [T2 – T1] or ΔE2– ΔE1 = ΔCv (T2 – T1). Standard heat enthalpy of elements in their most stable state is assumed to be zerowhereas standard heat enthalpy of compound is referred as heat of formation of that compound at 1 atmpressure and 25°C. Oxidation of N2 to N2O, NO, NO2 shows absorption of energy whereas heat of combustionof N2 is exothermic like other heat of combustion.Q. Which statements regarding the formation of NO and NO2respectively from N2and O2are correct:(A) Heat of formation of NO is exothermic(B) Heat of formation of NO2is exothermic(C) The oxidation of N2to NO and NO2is favoured at high temperature.(D) If heat of formation of NO and NO2are 21.55 and 8.50 kcal, heat of reaction forNO + ½O2→ NO2is -13.05 kcala)1,2b)3,4c)1,2,4d)1,2,3Correct answer is option 'B'. Can you explain this answer? theory, EduRev gives you an ample number of questions to practice Heat of reaction is the change in enthalpy or internal energy as represented by a balanced thermochemicalequation. The amount of energy released during a chemical change depends upon the state of reactantsand products, the conditions of pressure and volume at which reaction is carried out, and temperature.The variation of heat of reaction (ΔH or ΔE) with temperature is given as ΔH2 – ΔH1 = ΔCp [T2 – T1] or ΔE2– ΔE1 = ΔCv (T2 – T1). Standard heat enthalpy of elements in their most stable state is assumed to be zerowhereas standard heat enthalpy of compound is referred as heat of formation of that compound at 1 atmpressure and 25°C. Oxidation of N2 to N2O, NO, NO2 shows absorption of energy whereas heat of combustionof N2 is exothermic like other heat of combustion.Q. Which statements regarding the formation of NO and NO2respectively from N2and O2are correct:(A) Heat of formation of NO is exothermic(B) Heat of formation of NO2is exothermic(C) The oxidation of N2to NO and NO2is favoured at high temperature.(D) If heat of formation of NO and NO2are 21.55 and 8.50 kcal, heat of reaction forNO + ½O2→ NO2is -13.05 kcala)1,2b)3,4c)1,2,4d)1,2,3Correct answer is option 'B'. Can you explain this answer? tests, examples and also practice JEE tests.