Can anyone tell me the best way to calculate the euilibrium constant please?
the hydrolysis reaction of phosphocreatine in aqueous solution can be written as:
phosphocreatine = creatine + Pi
1) calculate the value of the equilibrium constant at 310 K, give that the change is standard gibbs free energy for the reaction at this temperature is -37.6kj mol^-1
2) a solution contains 0.0001 mol dm^-3 phosphocreatine, 0.01 mol dm^-3 creatine, and 0.0005 mol dm^-3 inorganic phosphate Pi
a) calculate the reaction quotient for the reaction under these conditions
b) is the reaction at equilibrium? if not, state whether the reaction will move to the left or the right as it proceed to equilibrium
Answer:
1) Delta G = - RT ln K
Delta G = Standard Gibbs Free Energy
R= Gas Constant (8.31J/molxK)
T=Temperature in Kevlin (298K since it's standard)
ln= Natural Log
K=Equilibrium Constant
-37600J=(-8.31J/molk)(298k)ln K
15.18=ln K
K=e^15.18
K=3927262.8 = 3.93e6
2)(a) Reaction Quotient = [Product]/[Reactant]
If creatine + Pi is product and phosphocreatine is reactant, then it would be
Q=[1e-4]^3X[0.01]^3/[5e-4]^3= 8e-9
(b) For the reaction to be equilibruim, Q=K but from #1 and #2a show Q<K, making it reactant-favored, (not sure if it's suppose to move left or right since i missed that lecture) but i think it should move right
don't have a clue to your question, just felt sorry for you cos no-one had answered your question and i didn't want you to feel left out.
yes the best way is to ask the equelibrium const to calculate himself
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phosphocreatine = creatine + Pi
1) calculate the value of the equilibrium constant at 310 K, give that the change is standard gibbs free energy for the reaction at this temperature is -37.6kj mol^-1
2) a solution contains 0.0001 mol dm^-3 phosphocreatine, 0.01 mol dm^-3 creatine, and 0.0005 mol dm^-3 inorganic phosphate Pi
a) calculate the reaction quotient for the reaction under these conditions
b) is the reaction at equilibrium? if not, state whether the reaction will move to the left or the right as it proceed to equilibrium
Answer:
1) Delta G = - RT ln K
Delta G = Standard Gibbs Free Energy
R= Gas Constant (8.31J/molxK)
T=Temperature in Kevlin (298K since it's standard)
ln= Natural Log
K=Equilibrium Constant
-37600J=(-8.31J/molk)(298k)ln K
15.18=ln K
K=e^15.18
K=3927262.8 = 3.93e6
2)(a) Reaction Quotient = [Product]/[Reactant]
If creatine + Pi is product and phosphocreatine is reactant, then it would be
Q=[1e-4]^3X[0.01]^3/[5e-4]^3= 8e-9
(b) For the reaction to be equilibruim, Q=K but from #1 and #2a show Q<K, making it reactant-favored, (not sure if it's suppose to move left or right since i missed that lecture) but i think it should move right
don't have a clue to your question, just felt sorry for you cos no-one had answered your question and i didn't want you to feel left out.
yes the best way is to ask the equelibrium const to calculate himself
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