Experiment 15: The Law of Chemical Equilibrium and Le Chatelier's Principle
Pre-Lab Questions
For the reaction at 20°C, NH3(aq) + H+(aq) ⇌ NH4+(aq), the equilibrium constant is calculated to be K = 4.5 x 10^8.
Write the equilibrium expression for this reaction.
Keq = [NH4+]/[NH3][H+]
From the size of the number for Keq, does the equilibrium lie to the left or to the right?
If the reaction between iron(III) ion and thiocyanate ion, Fe3+(aq) + SCN-(aq) ⇌ FeSCN2+(aq), yielded an equilibrium concentration of 0.10 M for each of the two ions, what is the equilibrium concentration of the red iron(III)-thiocyanate complex ion, FeSCN2+? (HINT: the equilibrium constant for the equilibrium is in the Background section in the lab manual.)
Here is the equilibrium constant for the equilibrium: K = [FeSCN2+]/[Fe3+][SCN^-] OR K = [products]/[reactants]
Show your work. Answer only will not earn any credit! You can take a photo of your work and insert your photo here.
In the reaction below, NH3(g) + H2O(l) ⇌ NH2- + H3O+, the equilibrium constant is 10^-34. Is this reaction likely to take place? Explain your answer.