Consider the reaction

x->Y

in a cell at

37\\\\deg C

. At equilibrium, the concentrations of

x

and

Y

are

50\\\\mu M

and

5\\\\mu M

, respectively. Use this information and the equations below to answer questions

1-5

.\

\\\\Delta G\\\\deg =-0.616lnK_(eq)\ \\\\Delta G=\\\\Delta G\\\\deg +0.616ln(Y)/(x)

\ Recall that the natural

log

of a number

z

will have a negative value when

z1

, positive when

z1

, and 0 when

z1

.\ 3. What is the value of

K_(eq)

for this reaction?

Consider the reaction XY in a cell at 37C. At equilibrium, the concentrations of X and Y are 50M and 5M, respectively. Use this information and the equations below to answer questions 15. G=0.616lnKeqG=G+0.616ln[Y]/[X] Recall that the natural log of a number z will have a negative value when z1, positive when z1, and 0 when z1. 3. What is the value of Keq for this reaction