Question

In: Chemistry

Kc for the following reaction is 0.35. H2 (g) + I2 (g) 2 HI (g). If...

Kc for the following reaction is 0.35. H2 (g) + I2 (g) 2 HI (g). If 1.0 mol of I2 and 1.0 mol of H2 are placed in a 1.0 L vessel, the equilibrium concentration of HI is :

The answer is 0.46 M, please explain how this value was reached. Thanks!

Expert Solution

Find out the initial concentration of the reactants as below.

[H₂] = (mol H₂)/(volume of container) = (1.0 mol)/(1.0 L) = 1.0 M

[I₂] = (mol I₂)/(volume of container) = (1.0 mol)/(1.0 L) = 1.0 M

Set up the ICE chart for the reaction as below.

H₂ (g) + I₂ (g) <=====> 2 HI (g)

initial 1.0 1.0 0.0

change -x -x +2x

equilibrium (1.0 – x) (1.0 – x) 2x

The equilibrium constant is given as

K_c = [HI]²/[H₂][I₂] = (2x)²/(1 – x).(1- x)

====> 0.35 = 4x²/(1 – x)²

====> 4x² = 0.35*(1 – x)²

Take the positive square root.

2x = 0.5916*(1 – x)

===> 2x = 0.5916 – 0.5916x

===> 2.5916x = 0.5916

===> x = (0.5916)/(2.5916) = 0.2283

The equilibrium concentration of HI is given as 2x = 2*(0.2283) M = 0.4566 M ≈ 0.46 M (ans).

queen_honey_blossom answered 2 years ago

The equilibrium constant Kc for the reaction H2(g) + I2(g) ⇌ 2 HI(g) is 54.3 at 430 ℃

The equilibrium constant Kc for the reaction H2(g) + I2(g) ⇌ 2 HI(g) is 54.3 at 430 ℃ Calculate the equilibrium concentrations of H2, I2, and HI at 430 ℃ if the initial concentrations are [H2] = [I2] = 0.222 M and [HI] = 0 M.[H2]eq = M[I2]eq = M[HI]eq = M

For the following reaction: H2(g) + I2(g)<--->2HI(g) ; Kc=49.5 The beginning concentrations are: H2: 0.10M, I2:...

For the following reaction: H2(g) + I2(g)<--->2HI(g) ; Kc=49.5 The beginning concentrations are: H2: 0.10M, I2: 0.050M, and HI:0 Assume this reaction is not at equilibrium. When it does reach equilibrium, what will the concentrations be?

Consider the equilibrium reaction. H2(g) + I2(g) ⇌ 2 HI(g) In this case, 1.000 M H2...

Consider the equilibrium reaction. H2(g) + I2(g) ⇌ 2 HI(g) In this case, 1.000 M H2 reacts with 2.000 M of I2 at a temperature of 441°C. The value of Kc = 67. Determine the equilibrium concentrations of H2, I2, and HI.

For the following reaction: 2HI (g) ----> H2(g) + I2(g), the rate law is rate= k[HI]^2....

For the following reaction: 2HI (g) ----> H2(g) + I2(g), the rate law is rate= k[HI]^2. You are starting with 1.0M HI. How long will the first half-life reaction be? (The professor adds: Note that since you don't know the value for the rate constant k, just leave it in your answers.)

The equilibrium constant Kc is 54.3 at 430°C for the following reaction: H2(g) + I2(g) ⇌...

The equilibrium constant Kc is 54.3 at 430°C for the following reaction: H2(g) + I2(g) ⇌ 2HI(g) Initially, 0.90 M H2, I2, and HI are introduced into a 5.0-L flask and allowed to come to equilibrium. What are the equilibrium concentrations of H2, I2, and HI in the flask? (10 points) (Does the size of flask matter since Molarity is given?)

1. Consider the reaction for the production of HI from H2 and I2. H2 (g)+...

1. Consider the reaction for the production of HI from H2 and I2. H2 (g)+ I2(g) D 2HI(g) a) What is the initial concentration of HI? b) What is the equilibrium concentration of HI? c) How is the change in concentration of HI calculated? Explain: d) How are the changes in concentration for H2 and I2 calculated? Explain e) How are the equilibrium concentrations of H2 and I2 calculated? Explain

The activation energy for the reaction H2(g) + I2(g) ? 2 HI(g) is 167 kJ/mol, and...

The activation energy for the reaction H2(g) + I2(g) ? 2 HI(g) is 167 kJ/mol, and ?E for the reaction is +28 kJ/mol. What is the activation energy for the decomposition of HI?

Kc for the reaction of hydrogen and iodine to produce hydrogen iodide. H2(g) + I2(g) ⇌...

Kc for the reaction of hydrogen and iodine to produce hydrogen iodide. H2(g) + I2(g) ⇌ 2HI(g) is 54.3 at 430°C. Calculate the equilibrium concentrations of H2, I2, and HI at 430°C if the initial concentrations are [H2] = [I2] = 0 M, and [HI] = 0.547 M. [H2]= [I2]= [HI]=

At a certain temperature, the equilibrium constant, Kc, for this reaction is 53.3. H2(g) + I2...

At a certain temperature, the equilibrium constant, Kc, for this reaction is 53.3. H2(g) + I2 (g) ---> 2 HI (g) Kc= 53.3 At this temperature, 0.600 mol of H2 and 0.600 mol of I 2 were placed in a 1.00-L container to react. What concentration of HI is present at equilibrium?

For the reaction H2(g)+I2(g)⇌2HI(g), Kc = 55.3 at 700 K. In a 2.00-L flask containing an...

For the reaction H2(g)+I2(g)⇌2HI(g), Kc = 55.3 at 700 K. In a 2.00-L flask containing an equilibrium mixture of the three gases, there are 0.057 g H2 and 4.39 g I2. Part A What is the mass of HI in the flask? Express your answer to two significant figures and include the appropriate units.