3-34 Consider the reaction X and 5 , respectively. Using the equations below and

Question

3-34 Consider the reaction X and 5 , respectively. Using the equations below and your new knowledge, answer the following questions Y in a cell at 37°C At equilibrium, the concentrations of X and are 50 M G'--0.6 16 In Kea Recall that the natural log of a number z will have a negative value when z 1, and 0 when = 1. A. What is the value of Keq for this reaction'? B. Is the standard free-energy change of this reaction positive or negative? Is the reaction X-Y an energetically favorable or unfavorable reaction under standard conditions? What is the value of the standard free energy? Refer to Table 3-1 in the textbook or use a calculator. Imagine circumstances in which the concentration of X is 1000 and that of Y is l pM conversion of X to Y favorable? Will it happen quickly? C. . Is D. E. Imagine starting conditions in which the reaction X- Y is unfavorable, yet the cell needs to produce more Y. Describe two ways in which this may be accomplished

Explanation / Answer

1 . the Keq = X/Y Keq = 5 um/50um Keq=0.1um 2.standard free energy is positive because when delta G is negative ,the exponent becomes positive(because it is multipled by -1).the above reaction is favourable in the above conditions because the delta G* for this reaction is negative

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