Consider a reaction with a large negative Gibbs energy change, as shown below: YZ, AG/ - 42.6 kJ mol The reaction is initiated by adding 16 mmol of compound Y into the flask, in the absence of compound Z is present. After 48 hours, analysis reveals the presence of 4 mmol of Z and 12 mmol of Y. Which is the most likely explanation? Y and Z have reached equilibrium concentrations. An enzyme has shifted the equilibrium toward Y. Formation of Z is kinetically slow; equilibrium has not been reached by 48 hours. Formation of Z is thermodynamically unfavorable. OTwo of the above explanations are reasonable.

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Chapter1: Chemical Foundations
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Consider
a reaction with a large negative Gibbs energy change, as shown below:
42.6 kJ mol-1
Y Z , AG°/
=
The reaction is initiated by adding 16 mmol of compound Y into the flask, in the
absence of compound Z is present. After 48 hours, analysis reveals the presence of
4 mmol of Z and 12 mmol of Y. Which is the most likely explanation?
▪▪▪▪▪▪
-
OY and Z have reached equilibrium concentrations.
An enzyme has shifted the equilibrium toward Y.
Formation of Z is kinetically slow; equilibrium has not been reached by 48 hours.
Formation of Z is thermodynamically unfavorable.
Two of the above explanations are reasonable.
Transcribed Image Text:Consider a reaction with a large negative Gibbs energy change, as shown below: 42.6 kJ mol-1 Y Z , AG°/ = The reaction is initiated by adding 16 mmol of compound Y into the flask, in the absence of compound Z is present. After 48 hours, analysis reveals the presence of 4 mmol of Z and 12 mmol of Y. Which is the most likely explanation? ▪▪▪▪▪▪ - OY and Z have reached equilibrium concentrations. An enzyme has shifted the equilibrium toward Y. Formation of Z is kinetically slow; equilibrium has not been reached by 48 hours. Formation of Z is thermodynamically unfavorable. Two of the above explanations are reasonable.
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