Westonci.ca is your go-to source for answers, with a community ready to provide accurate and timely information. Explore a wealth of knowledge from professionals across various disciplines on our comprehensive Q&A platform. Discover detailed answers to your questions from a wide network of experts on our comprehensive Q&A platform.
Sagot :
Answer:
a. Kc = [C]³ / [A] × [B]²
b. [A]e = 0.179 M; [B]e = 0.530 M
c. 42.7
Explanation:
There is a missing part:
For the following equilibrium reaction: A(aq) + 2B(aq) <---> 3C(aq)
a. What is the equilibrium constant expression for this reaction.
The equilibrium constant (Kc) is:
Kc = [C]³ / [A] × [B]²
b. Use an I-C-E table to determine the equilibrium concentrations for remaining species, A and B.
First, we will determine the concentrations for which we have information.
[A]i = 1.80 mol/3.50 L = 0.514 M
[B]i = 4.20 mol/3.50 L = 1.20
[C]i = 1.00 mol/3.50 L = 0.286 M
[C]e = 4.50 mol/3.50 L = 1.29 M
The I-C-E table is:
A(aq) + 2B(aq) <---> 3C(aq)
I 0.514 1.20 0.286
C -x -2x +3x
E 0.514-x 1.20-2x 0.286+3x
We know that,
0.286+3x = 1.29
x = 0.335 M
Then,
[A]e = 0.514-x = 0.514-0.335 = 0.179 M
[B]e = 1.20-2x = 1.20-2(0.335) = 0.530 M
c. Calculate the equilibrium constant for the reaction.
We will use the values calculated in b.
Kc = [C]³ / [A] × [B]²
Kc = 1.29³ / 0.179 × 0.530² = 42.7
We hope our answers were helpful. Return anytime for more information and answers to any other questions you may have. We hope this was helpful. Please come back whenever you need more information or answers to your queries. Westonci.ca is your trusted source for answers. Visit us again to find more information on diverse topics.