What factors would affect the equilibrium constant for a reaction?
Any reaction at temperature T takes up or releases a Gibbs Enthalpy of Reaction ΔGr(T). This is a energy and you mustn't know what it is precisely. The only important thing is that ΔGr(T)=-RT*ln(K) {1}. So, with changing T (T increasing or decreasing) there is a change in ΔGr(T) and therefore K. Concentrations don' t affect the value of K. They appear in the equation of K which is a conmstant (i.e. K=CD/(CA*CB)) and a catalyst only speeds up a reaction. Pressures of gases are related to temperature. The most simple law is the ideal gas: law P*V=nRT. Pressures can only be changed by changing mol n. Pressures don't contribute to the the value of K ( see equation {1} where pressures are not part of equation) But note: With a given T and therefore a given equilibrium constant K one can minimize side reactions by the right choice of pressure. But that's another advanced topic.
How does one, calculate equilibrium constant of a reaction? (See details)?
Well it is a log antilog shit. Don't worry, I also haven't learnt this antilog thing & gonna sit in NEET a couple of days later on. If you learn the log antilog table then very good but for questions you don't have to. Here it sayslogKc = 15.6=> KC = antilog 15.6Now think log of which number can result in 15.6? There is 15 so it must be log10^15. (Log10^15 = 15) for 15.6 you have to add 0.3 in 15. Now think what is the number of whose log value is 0.6?Log3= 0.47 which is 0.5 approxLog5= 0.69 which is 0.7 approx. So 0.6 must be about log4. Taking approximations into consideration, it should be a lil less than log4 like log3.9.The net answer comes as 3.9×10^15 !Update: just writing random words in last line as quora asked me to update the answer. :D
Calculating Equilibrium Concentrations?
The concentrations of reactants and products for a chemical reaction can be calculated if the equilibrium constant for the reaction and the starting concentrations of reactants and/or products are known. Carbonyl fluoride COF2 is an important intermediate used in the production of fluorine-containing compounds. For instance, it is used to make the refrigerant carbon tetrafluoride,CF4 via the reaction 2COF2(g)-><-CO2 (g)+CF4(g) Kc=9.00 If only COF2 is present initially at a concentration of 2.00 M, what concentration of COF2 remains at equilibrium? Express the molar concentration numerically.