What is ΔH in the equation ΔG = ΔH - TΔS?
A. The change in specific heat between the products and the reactants
B. The change in enthalpy between products and reactants in a reaction
C. The change in entropy between products and reactants in a reaction
D. The change in free energy between the products and the reactants
H is enthalpy
but I do physics, not chemistry.
answer is c
Well, well, well! It seems we've stumbled upon a thermodynamics equation. Time to get into the heat of things!
Now, in the equation ΔG = ΔH - TΔS, ΔH stands for the change in enthalpy. So, the answer you're looking for is B, my friend! It represents the change in enthalpy between the products and reactants in a reaction.
But hey, don't worry if it still feels a bit hazy. Thermodynamics can be quite a hot mess!
The correct answer is B. ΔH represents the change in enthalpy between the products and the reactants in a reaction.
To understand how to get this answer, let's break down the equation ΔG = ΔH - TΔS:
- ΔG represents the change in free energy between the products and the reactants. It measures the spontaneity of a reaction.
- ΔH represents the change in enthalpy between the products and the reactants. Enthalpy is a measure of the heat energy exchanged during a reaction. It tells us whether a reaction is exothermic (releasing heat) or endothermic (absorbing heat).
- T represents the temperature in Kelvin.
- ΔS represents the change in entropy between the products and the reactants. Entropy is a measure of the disorder or randomness in a system. It tells us whether a reaction will increase or decrease the disorder.
So, in the given equation, the term ΔH specifically refers to the change in enthalpy between the products and the reactants.