Question

In: Chemistry

The reversible chemical reaction A+B⇌C+D has the following equilibrium constant: Kc=[C][D][A][B]=5.9 Initially, only A and B...

The reversible chemical reaction

A+B⇌C+D

has the following equilibrium constant:

Kc=[C][D][A][B]=5.9

Initially, only A and B are present, each at 2.00 M. What is the final concentration of A once equilibrium is reached?

Part B

What is the final concentration of D at equilibrium if the initial concentrations are [A] = 1.00 M and [B] = 2.00 M ?

Solutions

Expert Solution

A + B <-------------> C + D

2      2                        0     0

2-x   2-x                      x      x

Kc = [C][D] / [A][B]

5.9 = x^2 / (2 -x)^2

x = 1.417

final concentration of A = 2 - x = 2 - 1.417

final concentration of A = 0.583 M

Part B )

A + B <-------------> C + D

1      2                        0     0

1-x   2-x                      x      x

Kc = [C][D] / [A][B]

5.9 = x^2 / (1-x)(2-x)

x = 0.882

final concentration of D = 0.882 M

queen_honey_blossom answered 8 months ago
Next > < Previous

Related Solutions

The reversible chemical reaction A+B⇌C+D has the following equilibrium constant: Kc=[C][D][A][B]=3.4 Initially, only A and B...
The reversible chemical reaction A+B⇌C+D has the following equilibrium constant: Kc=[C][D][A][B]=3.4 Initially, only A and B are present, each at 2.00 M. What is the final concentration of A once equilibrium is reached? What is the final concentration of D at equilibrium if the initial concentrations are [A] = 1.00 M and [B] = 2.00 M ?
The reversible chemical reaction A+B⇌C+D has the following equilibrium constant: Kc=[C][D]/[A][B]=5.4 PART A: Initially, only A...
The reversible chemical reaction A+B⇌C+D has the following equilibrium constant: Kc=[C][D]/[A][B]=5.4 PART A: Initially, only A and B are present, each at 2.00 M . What is the final concentration of A once equilibrium is reached? Express your answer to two significant figures and include the appropriate units. PART B: What is the final concentration of D at equilibrium if the initial concentrations are [A] = 1.00 M and [B] = 2.00 M ? Express your answer to two significant...
The reversible chemical reaction A+B?C+D has the following equilibrium constant: Kc=[C][D][A][B]=3.4 Part A Initially, only A...
The reversible chemical reaction A+B?C+D has the following equilibrium constant: Kc=[C][D][A][B]=3.4 Part A Initially, only A and B are present, each at 2.00 M. What is the final concentration of A once equilibrium is reached? Part B What is the final concentration of D at equilibrium if the initial concentrations are[A] = 1.00M and [B] = 2.00M ?
Using the Equilibrium Constant The reversible chemical reaction A+B⇌C+D has the following equilibrium constant: Kc=[C][D]/[A][B]=4.6 Part...
Using the Equilibrium Constant The reversible chemical reaction A+B⇌C+D has the following equilibrium constant: Kc=[C][D]/[A][B]=4.6 Part A Initially, only A and B are present, each at 2.00 M. What is the final concentration of A once equilibrium is reached? Express your answer to two significant figures and include the appropriate units. Part B What is the final concentration of D at equilibrium if the initial concentrations are [A] = 1.00 M and [B] = 2.00 M ? Express your answer...
1) The reversible chemical reaction A(aq)+B(aq)⇌C(aq)+D(aq) has the following equilibrium constant: K=[C][D][A][B]=5.2 a) Initially, only A...
1) The reversible chemical reaction A(aq)+B(aq)⇌C(aq)+D(aq) has the following equilibrium constant: K=[C][D][A][B]=5.2 a) Initially, only A and B are present, each at 2.00 mol L−1. What is the final concentration of A once equilibrium is reached? b) What is the final concentration of D at equilibrium if the initial concentrations are [A] = 1.00 mol L−1 and [B] = 2.00 mol L−1 ?
he reversible chemical reaction A(aq)+B(aq)⇌C(aq)+D(aq) has the following equilibrium constant: K=[C][D][A][B]=2.4 What is the final concentration...
he reversible chemical reaction A(aq)+B(aq)⇌C(aq)+D(aq) has the following equilibrium constant: K=[C][D][A][B]=2.4 What is the final concentration of D at equilibrium if the initial concentrations are [A] = 1.00 mol⋅L−1 and [B] = 2.00 mol⋅L−1 ?
An elementary reaction A to B is reversible and has an equilibrium constant of 10, and...
An elementary reaction A to B is reversible and has an equilibrium constant of 10, and a forward rate constant of 1.0 d-1. a) Plot the concentrations of A and B as a function of time in a batch reactor that initially contains 10-3 M each of A and B. Show the data from the initial condition until the concentrations are both changing at an instantaneous rate of less than 10-5 M per day. b) Repeat part (a) if the...
What is meant by chemical equilibrium? Given the following reaction: A + B <--> C +D...
What is meant by chemical equilibrium? Given the following reaction: A + B <--> C +D (reversible reaction), how would you drive the following reaction away from equilibrium to produce more of substances A and B?
At 1700 °C, the equilibrium constant, Kc, for the following reaction is 4.10 × 10–4. N2...
At 1700 °C, the equilibrium constant, Kc, for the following reaction is 4.10 × 10–4. N2 (g) +O2 (g) <---> 2NO (g) What percentage of O2 will react to form NO if 0.737 mol of N2 and 0.737 mol of O2 are added to a 0.645-L container and allowed to come to equilbrium at 1700 °C?
At 1700 °C, the equilibrium constant, Kc, for the following reaction is 4.10 × 10–4. N2...
At 1700 °C, the equilibrium constant, Kc, for the following reaction is 4.10 × 10–4. N2 (g) +O2 (g) <---> 2NO (g) What percentage of O2 will react to form NO if 0.737 mol of N2 and 0.737 mol of O2 are added to a 0.645-L container and allowed to come to equilbrium at 1700 °C?
ADVERTISEMENT
Subjects
ADVERTISEMENT
Latest Questions
ADVERTISEMENT