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?

Expert Solution

queen_honey_blossom answered 2 years ago

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...

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]=5.9 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 ?

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 ?

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 ?

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 ?

Chemical kinetics For the reaction 2A + B → C + D + 2E, data for...

Chemical kinetics For the reaction 2A + B → C + D + 2E, data for a run with [A]0 = 800 mmol/L and [B]0 = 2.00 mmol/L are t/ks 8 14 20 30 50 90 [B]/[B]0 0.836 .745 .680 .582 .452 .318 and data for a run with [A]0 = 600 mmol/L and [B]0 = 2.00 mmol/L are t/ks 8 20 50 90 [B]/[B]0 0.901 0.787 0.598 0.453 Find the order with respect to each reactant (A and B)...

Chemical species A, B, C, D and E are involved in a reaction. They may represent...

Chemical species A, B, C, D and E are involved in a reaction. They may represent reactants, products, intermediates, catalysts or inhibitors. The rate of change in the concentration for each of them is given below: d[A]/dt = -k1[A][B] + k-1[C][B] + k2[C][D] - k-2[A][E] d[B]/dt = 0 d[C]/dt = k1[A][B] - k-1[C][B] - k2[C][D] + k-2[A][E] d[D]/dt = -k2[C][D] + k-2[A][E] d[E]/dt = k2[C][D] - k-2[A][E] a) Write down the elementary steps in the proposed reaction mechanism that are...

Given K = 3.58 at 45°C for the reaction A(g) + B(g) equilibrium reaction arrow C(g)...

Given K = 3.58 at 45°C for the reaction A(g) + B(g) equilibrium reaction arrow C(g) and K = 7.06 at 45°C for the reaction 2 A(g) + D(g) equilibrium reaction arrow C(g) what is the value of K at the same temperature for the following reaction? C(g) + D(g) equilibrium reaction arrow 2 B(g) What is the value of Kp at 45°C for the same reaction? Starting with 1.46 atm partial pressures of both C and D, what is...

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