Question

I need help please: General equilibrium

11. Predict the direction of the shift in equilibrium of the reaction, if any, resulting from each of the following actions. In each case, write the equilibrium constant expression and explain your reasoning for the direction of the equilibrium shift. a. The reaction of carbon monoxide and hydrogen proceeds to equilibrium: CO(g)+2H,(8)=CH,OH(g) Argon is then introduced into the system. (1 point) b. The production of glucose by photosynthesis, an endothermic reaction, proceeds to equilibrium: 6CO.(8)+ 6H00)=C,H,0,(*)*60,48) SH - 2801 kJ The temperature is then increased. (1 point)

Answer 1

(a) Cocg) + 2H₂ (9) Chol (g) Realibu ima Lcн, оң) I col [H₂ ] 2 is pressure constant ure. - When Addition of Argon Cinert gas) At Constant Pressure - Whem Pressure is a On addition of inert gas, Volume increases and number of males of reaclant per lenit voulume decreases. So equilibrium will shift towards direction in which there is increases in number of molu. Reaction will shift backward. At Constant volume - At Constant pressure total volleme increases and at Constant volume total pressure increases But Concentration of Product and reactant will not change. So, there is no effect on equillibrium. (b ) Geog (g) + 6H₂ Old) = CH 120 (S) + 60₂ (9) - K= [og 16 - [coag6 As reaction is endothermic it means it requires high temperature. As temperature increases reaction proceeds forward. AG AH - TAS As AH = tve for Spontaneour reaction Au should be -ve. As temperature increases spontaneity increases.