For an exothermic reaction at 100 C , the equilibrium concentration of the products equals the equilibrium concentration of the reactants. What is true at 25 C?
A. Keq > 1 : [Products]> [Reactants]
b. Keq > 1 : [Products]< [Reactants]
c.Keq < 1 : [Products] > [Reactants]
d.Keq < 1 : [Products] <[Reactants]
ok , I 'm a little confused here. Answer is A
How is it possible to have a 1/1 ratio of Keq when heat is added into the system. Also, in this case how do we know which side is favored to remove excess heat. Is the system going to favor products ( to cool off the effect of heat) or would it prefer to go to the left and favor reactants?
I understand that if the products are favored to give release heat into the system, then if we cool this system, we would want to go to the products side (and thus release more heat). which would make the Equil K to be greater than 1 as more products are made. I just dont understand HOW you can tell that heat is given off in the forward direction. Please help!!!
A. Keq > 1 : [Products]> [Reactants]
b. Keq > 1 : [Products]< [Reactants]
c.Keq < 1 : [Products] > [Reactants]
d.Keq < 1 : [Products] <[Reactants]
ok , I 'm a little confused here. Answer is A
How is it possible to have a 1/1 ratio of Keq when heat is added into the system. Also, in this case how do we know which side is favored to remove excess heat. Is the system going to favor products ( to cool off the effect of heat) or would it prefer to go to the left and favor reactants?
I understand that if the products are favored to give release heat into the system, then if we cool this system, we would want to go to the products side (and thus release more heat). which would make the Equil K to be greater than 1 as more products are made. I just dont understand HOW you can tell that heat is given off in the forward direction. Please help!!!