In which of the following conditions is the Gibbs free energy negative? O reaction is at equilibrium process is spontaneous O reaction is exothermic O process is not spontaneous
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- Figure 6.8 Look at each of the processes shown, and decide if it is endergonic or exergonic. In each case, does enthalpy increase or decrease, and does entropy increase or decrease?Which of the following is not an assumption made when evaluating Michaelis Menton kinetics? the reaction is happening at body temperature the substrate is in great excess of the catalyst measurement of initial velocity of the reaction reaction conditions are occurring under steady stateWhich of the following relationships is (are) correct? (Select all that apply.) DG is equal to -TDSuniv DG > 0 represents a spontaneous process in the reverse direction. None of these DG < O represents a spontaneous process in the forward direction. DG < 0 indicates the reaction will reach equilibrium quickly.
- Which of the following describe(s) an exergonic reaction? energy is released non-spontaneous energy is absorbed spontaneousWhich of the statement is true regarding equilibrium? The rate of the forward reaction exceeds the rate of the reverse reaction The concentration of the reactants and the concentration of the products remains constant The value of equilibrium constant will change if a catalyst is present O Increasing the concentration of reactants increase the equilibrium constantTERMS BOX Endothermic Exothermic Catabolic Terms that describe this reaction Spontaneous Terms that describe this reaction Anabolic AG = positive Non-Spontaneous For each reaction below USE FIVE TERMS from the box above that describe the reaction AG = negative Produces Energy Uses Energy 6 CO₂ + H₂O → C6H12O6 + O₂
- Which one of the following statements is completely TRUE? O When AG > 0, the reaction is BOTH product-favored (spontaneous) AND endergonic. When AG 0, the reaction is BOTH reactant-favored (nonspontaneous) AND endergonic. When AG > 0, the reaction is BOTH product-favored (spontaneous) AND exergonic. When AG > 0, the reaction is BOTH reactant-favored (nonspontaneous) AND exergonic. When AG < 0, the reaction is BOTH reactant-favored (nonspontaneous) AND exergonic.Which of the following steps should be followed when performing kinetics experiments? the michaelis constant must be known the enzyme and substrate should not be mixed until just before the absorbance readings are taken reaction rates must be taken until reaction completion enzyme concentration must remain constantWhich of the following statements is true? (a) The largerthe Q, the larger the ΔG°. (b) If Q = 0, the system is at equilibrium.(c) If a reaction is spontaneous under standardconditions, it is spontaneous under all conditions. (d) Thefree-energy change for a reaction is independent of temperature.(e) If Q > 1, ΔG > ΔG°.
- Which of the following steps should be followed when performing kinetics experiments? Choose all that apply, partial positive and negative mark are given for correct and incorrect answers. enzyme concentration is kept constant for all reactions the enzyme and substrate should be mixed only when the reaction is initiated (when the absorbance readings are taken) the michaelis constant must be known reaction rates must be taken until reaction completionIn a transition state diagram, which of the following are features of the transition state (TS)? There may be more than one correct answer, select all that apply. The change in energy in ground state to the transition state represents the Gibbs Free Energy If the reaction is reversible, the TS will only progress forward to form products The TS occupies a trough The TS is associated with the highest energy The TS occupies the highest peakFor a reaction to be spontaneous, which of the following factors should have a negative sign? A Enthalpy and A Entropy A Temperature A Gibbs Free Energy and A Enthalpy AGibb's Free Energy, AEnthalpy and A Entropy Sell
