Heat is transferred directly from a heat reservoir at 200 C to another heat reservoir at 5C. If the amount of heat transferred i
s 100kJ, what is the total entropy change as a result of this process? Draw a schematic to represent the heat exchange
1 answer:
Answer:
ΔS=0.148 KJ/K
Explanation:
Given that
Q = 100 KJ
T₁=200°C
T₁=200+273 = 437 K
T₂=5°C
T₂=5 + 273 = 278 K
Reservoir 1 is rejecting heat that is why it taken as negative while the reservoir 2 is gaining the heat that is why it is taken as positive.
So the total change in entropy given as
ΔS= - Q/T₁ + Q/T₂
ΔS= - 100/473 + 100/278 KJ/K
ΔS=0.148 KJ/K
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Answer: Option (D) is the correct answer.
Explanation:
Enthalpy is defined as the amount of energy needed or removed from a substance. It is represented by .
Basically, it is the change in enthalpy and it represents the difference between the energy used in breaking bonds and the energy released in formation of bonds in a chemical reaction.
It is also known as heat of reaction. When value of is positive then it means heat is absorbed in the chemical reaction.
When value of is negative then it means that heat is released in the chemical reaction.
Whereas entropy means the measure of randomness. It is represented by . We cannot calculate entropy but we can measure the change in entropy.
Thus, we can conclude that all of the statements regarding the symbol "ΔH" are correct except it that can be called entropy change.