Asked by Jennifer
a. Calculate the delta H, delta G, and equilibrium constant for the reaction of methane with Cl2 to give CH3Cl and HCl. Use the following information for your calculations:
Bond Dissociation Energies:
CH3-H (104.8kcal/mol), Cl-Cl(59.0 kcal/mol), CH3-Cl(85.0 kcal/mol), and H-Cl (103.2 kcal/mol).
Thermodynamic data:
DeltaSrxn= + 0.29 x 10^.3 kcal/mol K, T=0 degrees celcius, and R= 1.987 cal/mol
find what K=
Bond Dissociation Energies:
CH3-H (104.8kcal/mol), Cl-Cl(59.0 kcal/mol), CH3-Cl(85.0 kcal/mol), and H-Cl (103.2 kcal/mol).
Thermodynamic data:
DeltaSrxn= + 0.29 x 10^.3 kcal/mol K, T=0 degrees celcius, and R= 1.987 cal/mol
find what K=
Answers
Answered by
Jennifer
I got that delta H=-24.4 and delta G=-24.3... But keep getting the equilibrium constant (K) wrong... Can someone please help...
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