1)As the temperature is decreased, the equilibrium position shifts in favour of the products.
2)The reaction is exothermic
3)The reaction is not spontaneous at any temperature.
4)delt G° is negative at all temperatures.
5)As the reaction proceeds, the system becomes more disordered.
I chosse
1)T, for an endothermic reaction, If we remove heat, the system will respond by shifting right to produce more heat to offset what was removed.
2)False, since the slope is negative deltH is positive, endothermic
3)T, since deltG>0 for all temp. therefore not spontaneous at any temp.
4)F, b=deltS/R, b is negative and R is positive, so deltS is negative. deltG=deltH+T*deltS, deltG is positive for all temp.
5)T, since deltS is negative it will become more disordered.
But not correct. Can you help me find which one is not correct and explain?
TheTemperature Dependence of Chemical Equilibrium For an equilibrium reaction: the following graph was obtained 10 -110 0.002 0.004 0.006 .008 0.01 1/T RT Given the above relationship, use the graph to identify which of the following statements are "true" or "false" in this specific case All statements refer to the forward reaction (proceeding left to right, as given) corresponding to the equilibrium constant K.
