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The standard free energy change (ΔG°) for 50% dissociation of N2O4 into NO2 at 27°C and 1 atm pressure is -x J mol-1. The value of x is _________. (Nearest Integer)
[Given: R = 8.31 J K-1 mol-1, log 1.33 = 0.1239 In 10 = 2.3]
[Given: R = 8.31 J K-1 mol-1, log 1.33 = 0.1239 In 10 = 2.3]
Correct answer is '710'. Can you explain this answer?
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The standard free energy change (ΔG°) for 50% dissociation o...
ΔG) is a thermodynamic parameter that measures the spontaneity and directionality of a chemical reaction. It is defined as the difference between the standard enthalpy change (ΔH) and the product of the absolute temperature (T) and the standard entropy change (ΔS):
ΔG = ΔH - TΔS
Where:
ΔG = standard free energy change
ΔH = standard enthalpy change
T = absolute temperature
ΔS = standard entropy change
The standard free energy change is a powerful tool in determining whether a reaction will occur spontaneously or not. If ΔG is negative, the reaction is exergonic (spontaneous) and will proceed in the forward direction. If ΔG is positive, the reaction is endergonic (non-spontaneous) and will not occur spontaneously. If ΔG is zero, the reaction is at equilibrium.
The standard free energy change can also be used to calculate the equilibrium constant (K) for a chemical reaction using the equation:
ΔG = -RT ln(K)
Where:
R = gas constant (8.314 J/mol·K)
T = absolute temperature
K = equilibrium constant
Overall, the standard free energy change provides valuable information about the energy changes associated with a chemical reaction and helps predict its spontaneity and directionality.
ΔG = ΔH - TΔS
Where:
ΔG = standard free energy change
ΔH = standard enthalpy change
T = absolute temperature
ΔS = standard entropy change
The standard free energy change is a powerful tool in determining whether a reaction will occur spontaneously or not. If ΔG is negative, the reaction is exergonic (spontaneous) and will proceed in the forward direction. If ΔG is positive, the reaction is endergonic (non-spontaneous) and will not occur spontaneously. If ΔG is zero, the reaction is at equilibrium.
The standard free energy change can also be used to calculate the equilibrium constant (K) for a chemical reaction using the equation:
ΔG = -RT ln(K)
Where:
R = gas constant (8.314 J/mol·K)
T = absolute temperature
K = equilibrium constant
Overall, the standard free energy change provides valuable information about the energy changes associated with a chemical reaction and helps predict its spontaneity and directionality.
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The standard free energy change (ΔG°) for 50% dissociation o...
= -710 J/mol
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The standard free energy change (ΔG°) for 50% dissociation of N2O4into NO2at 27°C and 1 atm pressure is -x J mol-1. The value of x is _________. (Nearest Integer)[Given: R = 8.31 J K-1mol-1, log 1.33 = 0.1239 In 10 = 2.3]Correct answer is '710'. Can you explain this answer?
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The standard free energy change (ΔG°) for 50% dissociation of N2O4into NO2at 27°C and 1 atm pressure is -x J mol-1. The value of x is _________. (Nearest Integer)[Given: R = 8.31 J K-1mol-1, log 1.33 = 0.1239 In 10 = 2.3]Correct answer is '710'. Can you explain this answer? for JEE 2025 is part of JEE preparation. The Question and answers have been prepared according to the JEE exam syllabus. Information about The standard free energy change (ΔG°) for 50% dissociation of N2O4into NO2at 27°C and 1 atm pressure is -x J mol-1. The value of x is _________. (Nearest Integer)[Given: R = 8.31 J K-1mol-1, log 1.33 = 0.1239 In 10 = 2.3]Correct answer is '710'. Can you explain this answer? covers all topics & solutions for JEE 2025 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for The standard free energy change (ΔG°) for 50% dissociation of N2O4into NO2at 27°C and 1 atm pressure is -x J mol-1. The value of x is _________. (Nearest Integer)[Given: R = 8.31 J K-1mol-1, log 1.33 = 0.1239 In 10 = 2.3]Correct answer is '710'. Can you explain this answer?.
The standard free energy change (ΔG°) for 50% dissociation of N2O4into NO2at 27°C and 1 atm pressure is -x J mol-1. The value of x is _________. (Nearest Integer)[Given: R = 8.31 J K-1mol-1, log 1.33 = 0.1239 In 10 = 2.3]Correct answer is '710'. Can you explain this answer? for JEE 2025 is part of JEE preparation. The Question and answers have been prepared according to the JEE exam syllabus. Information about The standard free energy change (ΔG°) for 50% dissociation of N2O4into NO2at 27°C and 1 atm pressure is -x J mol-1. The value of x is _________. (Nearest Integer)[Given: R = 8.31 J K-1mol-1, log 1.33 = 0.1239 In 10 = 2.3]Correct answer is '710'. Can you explain this answer? covers all topics & solutions for JEE 2025 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for The standard free energy change (ΔG°) for 50% dissociation of N2O4into NO2at 27°C and 1 atm pressure is -x J mol-1. The value of x is _________. (Nearest Integer)[Given: R = 8.31 J K-1mol-1, log 1.33 = 0.1239 In 10 = 2.3]Correct answer is '710'. Can you explain this answer?.
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