Consider the combustion of liquid methanol, CH3OH(l):
CH3OH(l) + 3/2 O2(g)→ CO2(g) + 2 H2O(l)
ΔH = –726.5 kJ
(a) What is the enthalpy change for the reverse reaction? (b) Balance the forward reaction with whole-number coefficients. What is ΔH for the reaction represented by this equation? (c) Which is more likely to be thermodynamically favored, the forward reaction or the reverse reaction? (d) If the reaction were written to produce H2O(g) instead of H2O(l), would you expect the magnitude of ΔH to increase, decrease, or stay the same? Explain.
Chemistry 1 12: General C hemistry II Week 1 1, April 0th ‐ April 14th, 017 Exam 3 ednesday, April 1 9th, 2017 18.2: K and Solubility Calcula埶���ons: SP ‐ Reaction Q uotient ( ) is calculated li , but states the situa埶��� s it currently is rather t han at equilibrium. ‐ Q = K: aturated solu埶���on, no p recipitate ‐ Q < K: Unsaturated solu埶���on, no precipitate ‐ Q > K: Supersaturated s olu埶���on, yes precipitate! Ex . Will a precipitate form when 25mL of 0.01M NaOH is added to 75mL of 0.10M MgCl 2 Mg(OH) ⇆ 2 Mg + H 2 O KSP .5E‐11 Q [ Mg OH Total Volume = 25mL + 75mL ‐ New C oncentration OH = 0.025 .01M / 0.10L = .0025M O H 2+ 2+ New Concentration Mg = 0.075 x 0.10M / 0.10L = 0.075M Mg Use These ^^ F or Q! Q [ 0.07 0.0025 ] Q = 4.69E‐7 Q > K: Precipitate orms! 18.3: Lewis Acid‐Base Complexes and Ion Equilibria : ‐ Lewis Acid = species that ccepts a air f electrons,