A chemical reaction is designated as exergonic rather than endergonic when __________. and

From the equation ΔG = ΔH – TΔS it is clear that __________.

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?

Which of the following determines the sign of ΔG for a reaction?

What do the sign and magnitude of the ΔG of a reaction tell us about the speed of the reaction? and

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.

What factors determine whether a chemical reaction is spontaneous or not?

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.

Using what you have learned about changes in Gibbs free energy, would you predict the ∆G value of catabolic reactions to be positive or negative? What about anabolic reactions? Justify your answers using the terms 'enthalpy' and 'entropy.'