7. Energy and Metabolism

Chemical Reactions

Open Question
Which of the following statements correctly describes any chemical reaction that has reached equilibrium?(A)The concentrations of products and reactants are equal.(B)The reaction is now irreversible.(C)Both forward and reverse reactions have halted.(D)The rates of the forward and reverse reactions are equal.
Multiple Choice
Which of the following statements is true for all exergonic reactions?
a) The products have more total energy than the reactants.
b) The reaction proceeds with a net loss of free energy.
c) The reaction goes only in a forward direction: all reactants will be converted to products.
d) A net input of energy from the surroundings is required for the reactions to proceed.
Multiple Choice
Which statement is true about chemical reactions?
Multiple Choice
Which statement describes a reversible reaction that has reached chemical equilibrium?
Multiple Choice
An exergonic (spontaneous) reaction is a chemical reaction that __________.
Multiple Choice
Which of the following reactions would be endergonic?
Multiple Choice
When one molecule is broken down into six component molecules, which of the following will always be true?
Multiple Choice
Which part of the equation ΔG = ΔH – TΔS tells you if a process is spontaneous?
Multiple Choice
If, during a process, the system becomes more ordered, then __________.
Multiple Choice
From the equation ΔG = ΔH – TΔS it is clear that __________.
Multiple Choice
Molecules A and B contain 110 kcal/mol of free energy, and molecules B and C contain 150 kcal/mol of energy. A and B are converted to C and D. What can be concluded?
Multiple Choice
Which of the following determines the sign of ΔG for a reaction?
Multiple Choice
What do the sign and magnitude of the ΔG of a reaction tell us about the speed of the reaction? and
Multiple Choice
A chemical reaction is designated as exergonic rather than endergonic when __________. and
Open Question
Which of the following correctly describe an exergonic reaction? Select True or False for each statement.T/F The products have lower Gibbs free energy than the reactants.T/F Activation energy is required for the reaction to proceed.T/F The products always have lower entropy than the reactants.T/F The reaction always occurs quickly.