Which of the following is true about exothermic reactions?
Which of the following is true about reactions that increase entropy?
What does a negative ΔG indicate?
What does a positive ΔG indicate?
When is a reaction at equilibrium?
When is a reaction considered under non-standard conditions?
How does the Gibbs free energy change when the reactants are increased compared to the products?
How does the Gibbs free energy change when the reactants are reduced compared to the products?
What is the rationale for why the body phosphorylates ATP as a source of energy currency?
Do enzymes themselves drop the ΔG?
Which one of these is the definition of a closed system?
Which one of these is the definition of an open system?
According to the first law of thermodynamics, what happens to the total amount of energy in the universe during a chemical change?
What does the term 'enthalpy' refer to?
How is the change in enthalpy (ΔH) measured in a chemical reaction?
What is the ΔH value for an exothermic reaction?
What is the ΔH value for an endothermic reaction?
What is the ΔH value for an isothermic reaction?
According to the second law of thermodynamics, what happens to the total entropy of the universe?
What does an increase in entropy (S) indicate?
A positive ΔH can sometimes will cause a spontaneus reaction if ΔS is...
A negative ΔS can sometimes cause a spontaneous reaction if ΔH is...
A reaction will never be spontaneous if...
If the [Products] is higher than the [Reactants] the reaction is less likely to be..
A reaction will always be spontaneous if...
Test your knowledge of thermodynamics and the definitions of open and closed systems with this quiz. Learn about the first law of thermodynamics and how it applies to chemical reactions.
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