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the value of log10 k for a reaction A=B IS Given delta r H˙298 K = -54.07KJ per mol,Delta r S˙= 10 J PER KELVIN PER MOL and R = 8.314 per joule per kelvin per mol. A)5 B)10 C)95 D)100
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the value of log10 k for a reaction A=B IS Given delta r H˙298 K = -54...
∆G = ∆H – T∆S∆G = –54.070*10³ – 298*10∆G = –57050 Joule∆G= –(2.303)(RT) log{base10}K–57050 = –(2.303) * (8.314) * (298) log Kon solving log K = 9.997 ≈ 10
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the value of log10 k for a reaction A=B IS Given delta r H˙298 K = -54...
Calculation of Log10 K for Reaction A=B
Given:
Delta r H˙298 K = -54.07KJ per mol
Delta r S˙= 10 J PER KELVIN PER MOL
R = 8.314 per joule per kelvin per mol
We need to calculate the value of log10 K for the given reaction A=B.
1. Write the Balanced Chemical Equation
To calculate the value of K, we need to write the balanced chemical equation for the given reaction A=B.
A → B
2. Calculate Delta r G˙ at 298 K
Delta r G˙ can be calculated using the following formula:
Delta r G˙ = Delta r H˙ - T Delta r S˙
where T is the temperature in Kelvin.
Substituting the given values, we get:
Delta r G˙ = -54.07KJ/mol - (298K)(10J/K/mol)
Delta r G˙ = -57.37KJ/mol
3. Calculate the Value of K
The value of K can be calculated using the following formula:
Delta r G˙ = -RT ln K
where R is the gas constant and ln is the natural logarithm.
Substituting the given values, we get:
-57.37KJ/mol = -(8.314 J/K/mol)(298K) ln K
ln K = 21.54
K = e^(21.54)
K = 9.5 x 10^9
4. Calculate Log10 K
Log10 K can be calculated using the following formula:
Log10 K = ln K / ln 10
Substituting the value of K, we get:
Log10 K = ln (9.5 x 10^9) / ln 10
Log10 K = 9.98
Therefore, the value of log10 K for the given reaction A=B is 10 (option B).
Conclusion:
The value of log10 K for the given reaction A=B is 10.
Given:
Delta r H˙298 K = -54.07KJ per mol
Delta r S˙= 10 J PER KELVIN PER MOL
R = 8.314 per joule per kelvin per mol
We need to calculate the value of log10 K for the given reaction A=B.
1. Write the Balanced Chemical Equation
To calculate the value of K, we need to write the balanced chemical equation for the given reaction A=B.
A → B
2. Calculate Delta r G˙ at 298 K
Delta r G˙ can be calculated using the following formula:
Delta r G˙ = Delta r H˙ - T Delta r S˙
where T is the temperature in Kelvin.
Substituting the given values, we get:
Delta r G˙ = -54.07KJ/mol - (298K)(10J/K/mol)
Delta r G˙ = -57.37KJ/mol
3. Calculate the Value of K
The value of K can be calculated using the following formula:
Delta r G˙ = -RT ln K
where R is the gas constant and ln is the natural logarithm.
Substituting the given values, we get:
-57.37KJ/mol = -(8.314 J/K/mol)(298K) ln K
ln K = 21.54
K = e^(21.54)
K = 9.5 x 10^9
4. Calculate Log10 K
Log10 K can be calculated using the following formula:
Log10 K = ln K / ln 10
Substituting the value of K, we get:
Log10 K = ln (9.5 x 10^9) / ln 10
Log10 K = 9.98
Therefore, the value of log10 K for the given reaction A=B is 10 (option B).
Conclusion:
The value of log10 K for the given reaction A=B is 10.
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the value of log10 k for a reaction A=B IS Given delta r H˙298 K = -54.07KJ per mol,Delta r S˙= 10 J PER KELVIN PER MOL and R = 8.314 per joule per kelvin per mol. A)5 B)10 C)95 D)100
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the value of log10 k for a reaction A=B IS Given delta r H˙298 K = -54.07KJ per mol,Delta r S˙= 10 J PER KELVIN PER MOL and R = 8.314 per joule per kelvin per mol. A)5 B)10 C)95 D)100 for NEET 2024 is part of NEET preparation. The Question and answers have been prepared according to the NEET exam syllabus. Information about the value of log10 k for a reaction A=B IS Given delta r H˙298 K = -54.07KJ per mol,Delta r S˙= 10 J PER KELVIN PER MOL and R = 8.314 per joule per kelvin per mol. A)5 B)10 C)95 D)100 covers all topics & solutions for NEET 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for the value of log10 k for a reaction A=B IS Given delta r H˙298 K = -54.07KJ per mol,Delta r S˙= 10 J PER KELVIN PER MOL and R = 8.314 per joule per kelvin per mol. A)5 B)10 C)95 D)100.
the value of log10 k for a reaction A=B IS Given delta r H˙298 K = -54.07KJ per mol,Delta r S˙= 10 J PER KELVIN PER MOL and R = 8.314 per joule per kelvin per mol. A)5 B)10 C)95 D)100 for NEET 2024 is part of NEET preparation. The Question and answers have been prepared according to the NEET exam syllabus. Information about the value of log10 k for a reaction A=B IS Given delta r H˙298 K = -54.07KJ per mol,Delta r S˙= 10 J PER KELVIN PER MOL and R = 8.314 per joule per kelvin per mol. A)5 B)10 C)95 D)100 covers all topics & solutions for NEET 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for the value of log10 k for a reaction A=B IS Given delta r H˙298 K = -54.07KJ per mol,Delta r S˙= 10 J PER KELVIN PER MOL and R = 8.314 per joule per kelvin per mol. A)5 B)10 C)95 D)100.
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