I’m working on a biology multi-part question and need support to help me study.For the chemical reaction A ⇌ B, the equilibrium constant Keq = 0.02 at 25°C. For the chemical reaction B ⇌ C, the equilibrium constant at 25°C is Keq = 1000Determine the standard state Gibbs free energy (ΔG°’) for both these reactions. (Hint: note that the temperature is 25°C, which is 298.15 K)
Determine the equilibrium constant Keq and standard state Gibbs free energy (ΔG°’) for the chemical reaction A ⇌ C
The reaction pyruvate + ATP ⇌ ADP + PEP is catalyzed by the enzyme pyruvate kinase. ΔG°’ for this reaction is +31.4 kJ/mol.Does this reaction move forward (from left to right) or backward under conditions of the standard state? What is meant by “standard state conditions” anyway?
Calculate the equilibrium constant (Keq) for this reaction at 25°C.
The concentrations of reactants and products of this reaction are measured in a particular cell at 37°C and found to be: pyruvate (24.9 mM); ATP (12.5 mM); ADP (0.14 mM); and PEP (0.01 mM). Calculate the Gibbs free energy for this reaction under these conditions.
Will the reaction proceed spontaneously in the forward direction in this cell? Why or why not?
Imagine that you have 500 mL of pure water. In other words, there is nothing in your beaker except for H2O molecules.What would be the pH of this water after it is allowed to reach equilibrium with the products of its spontaneous ionization H+ and OH–?
What would be the pH of the solution that resulted from dissolving 0.004 moles of NaOH in the water?
Requirements: based on the questions show with work | .doc file
