Question

has a standard free-energy change of –3.63 kJ/mol at 25 °C. What are the concentrations of...

has a standard free-energy change of –3.63 kJ/mol at 25 °C. What are the concentrations of A, B, and C at equilibrium if, at the beginning of the reaction, their concentrations are 0.30 M, 0.40 M, and 0 M, respectively?

Please Please Please show all the steps when you are calculating the Ice table calculations

A= ?       B=?     C=?

Homework Answers

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
A reaction A + B <==> C has a standard free-energy change of -4.29 kj/mol at...
A reaction A + B <==> C has a standard free-energy change of -4.29 kj/mol at 25C What are the concentrations of A, B, and C at equilibrium if at the beginning of the reaction their concentrations are 0.30M, 0.40M and 0M respectively? How would your answers above change if the reaction had a standard free-energy change of +4.29 kj/mol? ____ there would be no change to the answers. ____ All concentrations would be lower. ____ All concentrations would be...
The standard free energy change for ATP hydrolysis is -30.5 kJ/mol. Therefore, the free energy change...
The standard free energy change for ATP hydrolysis is -30.5 kJ/mol. Therefore, the free energy change for this reaction in a cell in which the concentration of ATP, ADP, and Pi are 3.1 mM, 2.2 mM and 6.8 mM, respectively, and assuming a physiologically relevant temperature (37 °C), is: Answer -44.25 kJ/mol explain
1) The free energy change for the following reaction at 25 °C, when [Pb2+] = 1.18...
1) The free energy change for the following reaction at 25 °C, when [Pb2+] = 1.18 M and [Cd2+] = 7.90×10-3 M, is -65.9 kJ: Pb2+(1.18 M) + Cd(s)> Pb(s) + Cd2+(7.90×10-3 M) ΔG = -65.9 kJ What is the cell potential for the reaction as written under these conditions? Answer: ___V Would this reaction be spontaneous in the forward or the reverse direction? 2) Use the standard reduction potentials located in the 'Tables' linked above to calculate the standard...
Consider the fructose-1,6-bisphosphatase reaction. Calculate the free energy change if the ratio of the concentrations of...
Consider the fructose-1,6-bisphosphatase reaction. Calculate the free energy change if the ratio of the concentrations of the products to the concentrations of the reactants is 21.3, and the temperature is 37.0 °C? ΔG°\' for the reaction is –16.7 kJ/mol. The constant R = 8.3145 J/(mol·K)
A<->B<->C delta G0 for A<->B =11.4 kJ mol-1 delta G0 for B<->C = -22.8 kJ mol-1...
A<->B<->C delta G0 for A<->B =11.4 kJ mol-1 delta G0 for B<->C = -22.8 kJ mol-1 A. What is the deta G0 for the conversion of A to C? B. Write an equation for the free energy change (delta G) of the first reaction, A to B, taking into account concentrations of reactants and products. C. At equilibrium, what are the concetration ratios of [B]/[A], [C]/[B], and [C]/[A]?
The standard free energy of activation of a reaction A is 88.2 kJ mol–1 (21.1 kcal...
The standard free energy of activation of a reaction A is 88.2 kJ mol–1 (21.1 kcal mol–1) at 298 K. Reaction B is ten million times faster than reaction A at the same temperature. The products of each reaction are 10.0 kJ mol–1 (2.39 kcal mol–1) more stable than the reactants. (a) What is the standard free energy of activation of reaction B? (b) What is the standard free energy of activation of the reverse of reaction A? (c) What...
For the reaction of A + Bà C +D, what is the actual free energy if...
For the reaction of A + Bà C +D, what is the actual free energy if the standard free energy is +5 kJ/mole and the concentrations of A, B, C and D respectively are 0.2, 0.4, 5 and 10 molar? Is this a favorable reaction or not? Why or Why not?
The equilibrium constant of a system, K, can be related to the standard free energy change,...
The equilibrium constant of a system, K, can be related to the standard free energy change, ΔG∘, using the following equation: ΔG∘=−RTlnK where T is a specified temperature in kelvins (usually 298 K) and R is equal to 8.314 J/(K⋅mol). Under conditions other than standard state, the following equation applies: ΔG=ΔG∘+RTlnQ In this equation, Q is the reaction quotient and is defined the same manner as K except that the concentrations or pressures used are not necessarily the equilibrium values....
The equilibrium constant of a system, K, can be related to the standard free energy change,...
The equilibrium constant of a system, K, can be related to the standard free energy change, ΔG∘, using the following equation: ΔG∘=−RTlnK where T is a specified temperature in kelvins (usually 298 K) and R is equal to 8.314 J/(K⋅mol). Under conditions other than standard state, the following equation applies: ΔG=ΔG∘+RTlnQ In this equation, Q is the reaction quotient and is defined the same manner as K except that the concentrations or pressures used are not necessarily the equilibrium values....
The standard Gibbs free energy change for hydrolysis or pure ATP to pure ADP is -31KJ/mol....
The standard Gibbs free energy change for hydrolysis or pure ATP to pure ADP is -31KJ/mol. The reaction is written ATP = ADP +Pi. What is the Gibbs energy of reaction in an environment at 37 C in which the ATP, ADP, and Pi concentrations are all 1mmol/L or 1 µmol/L?
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT