04:19Chemical Equations | Environmental Chemistry | Chemistry | FuseSchoolFuseSchool - Global Education770views
05:43Chemical reactions introduction | Chemistry of life | Biology | Khan AcademyKhan Academy1205views
Multiple ChoiceWhich 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.4785views37rank
Multiple ChoiceWhich statement describes a reversible reaction that has reached chemical equilibrium? 1501views
Multiple ChoiceWhen one molecule is broken down into six component molecules, which of the following will always be true? 839views
Multiple ChoiceWhich part of the equation ΔG = ΔH – TΔS tells you if a process is spontaneous? 781views
Multiple ChoiceMolecules 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? 993views
Multiple ChoiceWhat do the sign and magnitude of the ΔG of a reaction tell us about the speed of the reaction? and 1888views1rank
Multiple ChoiceA chemical reaction is designated as exergonic rather than endergonic when __________. and 973views1rank
Textbook QuestionWhich 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.875views
Textbook QuestionWhich 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.849views
Textbook QuestionUsing 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.'1085views
01:56
