Posted by cateye on Monday, April 23, 2012 at 8:22am.
Answer the following for me.
What's C3H6O? C2H6O? C7H16O2?
How do you know it's exothermic?
I have to use the equation above:following equilibrium system with a Kc of 1.23E-03:
C3H6O (aq) + 2C2H6O (aq)--> C7H16O2 (aq) + 2H2O (l)
to complete the problems..this is what my teacher gave me to go on..So can u please help me out.. Tell me if I am go in the right direction
There isn't enough information to answer 1.
2, 3, are not right.
I need the information for 1 to answer 4 and 6.
5 is 1/1.23E-3 = 1/0.00123 = 813
I hope this will help us figure out now
For questions #1 through #10, refer to the following equilibrium system, with a Kc of 1.23E-03:
C3H6O (aq) + 2C2H6O(aq)----> C7H16O2 (aq) + 2H2O (l)
1. What is the equilibrium expression for this system?
[C7H16O2]/ [C3H6O][C2H6O]2
2.If the molar concentrations of C3H6O2 and C2H6O are both 0.255 at equilibrium, what is the equilibrium concentration of C7H16O2?
2.04E-06
3.What is true about the concentrations of the reactants and products at equilibrium?
The reactant concentrations are increasing, while the products are decreasing
4.What is true about the rate of the forward and reverse reactions at equilibrium?
They are identical
5.Is this an endothermic- or exothermic reaction, as written?
Exothermic
6.How would the equilibrium shift if the pressure of the system were doubled?
To the left
7.How would the equilibrium shift if C7H16O2 were added?
To the right
8.How would the equilibrium shift if the system were cooled?
No change
9.What would the Kc be for the reverse equilibrium? That is, for:
C7H16O2 (aq) + 2H2O (l)---> C3H6O (aq) + 2C2H6O (aq)
813
1.For the reverse equilibrium, as depicted in #9, is this an endo- or exothermic process?
endothermic
For questions #1 through #10, refer to the following equilibrium system, with a Kc of 1.23E-03:
C3H6O (aq) + 2C2H6O(aq)----> C7H16O2 (aq) + 2H2O (l)
1. What is the equilibrium expression for this system?
[C7H16O2]/ [C3H6O][C2H6O]2
ok.
2.If the molar concentrations of C3H6O2 and C2H6O are both 0.255 at equilibrium, what is the equilibrium concentration of C7H16O2?
2.04E-06
OK
3.What is true about the concentrations of the reactants and products at equilibrium?
The reactant concentrations are increasing, while the products are decreasing
With a K of 0.00123 (less than 1), the reaction at equilibrium is far to the left which means that the concentrations of the reactants are much greater than the concentration of the products at equilibrium. Note that this doesn't say anything about the RATE of the forward or the reverse reaction.
4.What is true about the rate of the forward and reverse reactions at equilibrium?
They are identical
Correct, but note that this answer contradicts the incorrect answer you gave for the previous question.
5.Is this an endothermic- or exothermic reaction, as written?
Exothermic
There isn't enough information given to answer.
6.How would the equilibrium shift if the pressure of the system were doubled?
To the left
No change
7.How would the equilibrium shift if C7H16O2 were added?
To the right
When we add a reagent to a system in equilibrium, the system tries to undo what we've done. So if we add the product, the system will try to undo the addition, which means the system will try to use up the added material. It can do that by reacting to the left. If it shifts to the right you add MORE, not less, of the product.
8.How would the equilibrium shift if the system were cooled?
No change
Not enough information to answer
9.What would the Kc be for the reverse equilibrium? That is, for:
C7H16O2 (aq) + 2H2O (l)---> C3H6O (aq) + 2C2H6O (aq)
813
OK
1.For the reverse equilibrium, as depicted in #9, is this an endo- or exothermic process?
endothermic
Not enough information to answer.
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