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In a reaction, the change in entropy is given as 2.4 cal/K and the change in Gibbs free energy is given as 3.4 kcal, calculate the change in heat at the temperature of 20-degree centigrade?
- a)3.4 kcal
- b)3.4 cal
- c)3.4 kJ
- d)3.4 J
Correct answer is option 'A'. Can you explain this answer?
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Most Upvoted Answer
In a reaction, the change in entropy is given as 2.4 cal/K and the cha...
Using the equation ΔG = ΔH – TΔS, where G is represented by the Gibbs free energy, H is represented by the change in enthalpy, T is represented by the temperature and S is represented by the entropy. ΔH = ΔG + TΔS = 3.4 kcal – 293 x 2.4 cal/K = 3.4 kcal.
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In a reaction, the change in entropy is given as 2.4 cal/K and the cha...
Given:
Change in entropy (ΔS) = 2.4 cal/K
Change in Gibbs free energy (ΔG) = 3.4 kcal
To find:
Change in heat (ΔQ) at 20 degrees Celsius
Solution:
We know that Gibbs free energy change (ΔG) is related to entropy change (ΔS) and heat change (ΔQ) by the equation:
ΔG = ΔQ - TΔS
Where:
ΔG = Change in Gibbs free energy
ΔQ = Change in heat
ΔS = Change in entropy
T = Temperature in Kelvin
Step 1: Convert the given temperature from Celsius to Kelvin.
The temperature is given as 20 degrees Celsius. To convert it to Kelvin, we add 273.15 to the Celsius temperature.
Temperature in Kelvin = 20 + 273.15 = 293.15 K
Step 2: Substitute the given values into the equation and solve for ΔQ.
ΔG = ΔQ - TΔS
3.4 kcal = ΔQ - (293.15 K)(2.4 cal/K)
3.4 kcal = ΔQ - 703.56 cal
Step 3: Convert the units of ΔG and ΔQ to the same unit (kcal or cal).
Since the given value of ΔG is in kcal, we need to convert ΔQ to kcal as well.
1 kcal = 1000 cal
So,
3.4 kcal = ΔQ - 703.56 cal
3.4 kcal = ΔQ - 0.70356 kcal
ΔQ = 3.4 kcal + 0.70356 kcal
ΔQ = 4.10356 kcal
Step 4: Round the final answer to the appropriate number of significant figures.
The answer is rounded to one decimal place since the given value of ΔG is given to one decimal place.
ΔQ = 4.1 kcal
Answer:
The change in heat at 20 degrees Celsius is 4.1 kcal.
Change in entropy (ΔS) = 2.4 cal/K
Change in Gibbs free energy (ΔG) = 3.4 kcal
To find:
Change in heat (ΔQ) at 20 degrees Celsius
Solution:
We know that Gibbs free energy change (ΔG) is related to entropy change (ΔS) and heat change (ΔQ) by the equation:
ΔG = ΔQ - TΔS
Where:
ΔG = Change in Gibbs free energy
ΔQ = Change in heat
ΔS = Change in entropy
T = Temperature in Kelvin
Step 1: Convert the given temperature from Celsius to Kelvin.
The temperature is given as 20 degrees Celsius. To convert it to Kelvin, we add 273.15 to the Celsius temperature.
Temperature in Kelvin = 20 + 273.15 = 293.15 K
Step 2: Substitute the given values into the equation and solve for ΔQ.
ΔG = ΔQ - TΔS
3.4 kcal = ΔQ - (293.15 K)(2.4 cal/K)
3.4 kcal = ΔQ - 703.56 cal
Step 3: Convert the units of ΔG and ΔQ to the same unit (kcal or cal).
Since the given value of ΔG is in kcal, we need to convert ΔQ to kcal as well.
1 kcal = 1000 cal
So,
3.4 kcal = ΔQ - 703.56 cal
3.4 kcal = ΔQ - 0.70356 kcal
ΔQ = 3.4 kcal + 0.70356 kcal
ΔQ = 4.10356 kcal
Step 4: Round the final answer to the appropriate number of significant figures.
The answer is rounded to one decimal place since the given value of ΔG is given to one decimal place.
ΔQ = 4.1 kcal
Answer:
The change in heat at 20 degrees Celsius is 4.1 kcal.
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