If anyone could please explain to me step by step how this isdone, it would be very much appreciated!
The Gibbs Free Energy for the reaction A + 2B = C was measured as a function of temperature: Calculate the enthalpy and entropy changes for the reaction Comment on the signs of the change in entropy, enthalpy and the effect of temperature. Predict the equilibrium constant at 80degreeC. If the concentrations are [A] = 0.02 mol L-1, [B] = 0.0015 mol L-1, [C] = 2 mol L-1 at 80degreeC. will the system produce reactants or products as the reaction comes to equilibrium?
After completing the calculations answer the following questions separately for each experiment:
Is the dissolving exothermic or endothermic?
Does the entropy decreases or increases during dissolving?
Is the Gibbs free energy positive or negative? Is the process of dissolving spontaneous?
Using data in the appendix in your textbook, calculate Gibbs free energy for the reaction of dissolving
lithium phosphate, Li3PO4, in water at 25 °C. Do the calculations in two ways:
1) Use standard enthalpy of formation (ÎH) and entropy (S) from the appendix in your textbook, and use the same formula as you did in the lab experiments: ÎG = ÎH â TÎS. Remember that both ÎH and ÎS has to include three lithium ions.
2) Use standard free energies of formation from Appendix 6 (ÎG) and equation
