For the reaction H2(g) + I2(g) ↔ 2HI the value of the equilibrium constant is 25....

For the reaction

H2(g) + I2(g) ↔ 2HI

the value of the equilibrium constant is 25.

Starting with 1.00mol of each reactant in a 10.L vessel, how many moles of HI will be present at equilibrium?

Solutions

Expert Solution

H₂ (g) + I₂ (g) 2 HI (g)

Kc = 25

Initial concentrations,

[H₂] = [I₂] = [HI] = 1.00 / 10.0 = 0.100 M

at equilibrium, [H₂] = [I₂] = 0.100 - x and [HI] = 0.100 + 2x

Equilibrium constant expression can be written as,

Kc = [HI]² / [H₂][I₂]

Kc = ( 0.100 + 2x)² / (0.100 - x)(0.100 - x)

25 ( 0.0100 + x² - 0.200x) = 0.0100 + 4x² + 0.400x

0.250 + 25x² - 5.00x = 0.0100 + 4x² + 0.400x

21x² -5.4x + 0.24x = 0

it is similar to ax² + bx +c = 0

So, on applying quadratic equation,

x = [-(-5.4)((-5.4)² - (4*21*0.24))] / (2 *21)

x = 0.0571 M

So, at equilibrium, [HI] = 0.100 + 2(0.0572) = 0.214 M

But, number of moles = Molarity * volume = 0.214 * 10 = 2.14 mol

queen_honey_blossom answered 1 year ago

Next > < Previous

Related Solutions

At 500K, the equilibrium constant, Keq, is 155 for the reaction H2(g) + I2(g) ↔ 2HI(g)....

At 500K, the equilibrium constant, Keq, is 155 for the reaction H2(g) + I2(g) ↔ 2HI(g). Calculate the equilibrium constant for the reaction 2H2(g) + 2I2(g) ↔ 4HI(g), 1/2H2(g) + 1/2I2(g) ↔ HI(g), and 2HI(g) ↔ H2(g) + I2(g).

At a certain temp, the equilibrium constant for this reaction is 53.3. H2(g)+I2(g)=2HI(g) At this temperature,...

At a certain temp, the equilibrium constant for this reaction is 53.3. H2(g)+I2(g)=2HI(g) At this temperature, 0.7 mol of H2 and 0.7 mol of I2 were placed in a 1 L container. What is the concentration of HI present at equilibrium?

1. For the reaction in the previous problem, that is, 2HI(g) ↔ H2(g) + I2(g) Keq...

1. For the reaction in the previous problem, that is, 2HI(g) ↔ H2(g) + I2(g) Keq = 0.016 Initially a container contains 0.69 M HI and no product. What is the equilibrium concentration of H2? 2. For the reaction: 2HBr(g) ↔ H2(g) + Br2(g) Initially a container contains 0.87 M HBr and no product. What is the equilibrium concentration of HBr if the equilibrium concentration of H2 is 0.16 M? (Hint provided in feedback.)

Consider the following reaction: H2(g)+I2(g)?2HI(g) The data in the table show the equilibrium constant for this...

Consider the following reaction: H2(g)+I2(g)?2HI(g) The data in the table show the equilibrium constant for this reaction measured at several different temperatures. Temperature Kp 150 K 1.4×10?6 175 K 4.6×10?6 200 K 3.6×10?2 225 K 1.1 250 K 15.5 Use the data to find ?H?rxn and ?S?rxn for the reaction.

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?

The rate constant of the elementary reaction 2HI(g) H2(g) +I2(g) is k = 1.97 L mol-1...

The rate constant of the elementary reaction 2HI(g) H2(g) +I2(g) is k = 1.97 L mol-1 s-1 at 604°C, and the reaction has an activation energy of 206 kJ mol-1. (a) Compute the rate constant of the reaction at a temperature of 767°C. L mol-1 s-1 (b) At a temperature of 604°C, 177 s is required for half of the HI originally present to be consumed. How long will it take to consume half of the reactant if an identical...

The equilibrium constant for the following reaction: H2(g) + Br2(g) ↔ 2HBr (g) is 1.95 x...

The equilibrium constant for the following reaction: H2(g) + Br2(g) ↔ 2HBr (g) is 1.95 x 103 at a certain temperature. Find the equilibrium pressure of HBr if 10.70 atm of HBr is introduced into a sealed container at this temperature.

Consider the following reaction: H2(g) + I2(g) ⇌ 2HI(g) At a particular temperature, a reaction mixture...

Consider the following reaction: H2(g) + I2(g) ⇌ 2HI(g) At a particular temperature, a reaction mixture at equilibrium contains pressures of H2 = 0.958 atm, I2 = 0.877 atm, and HI = 0.020 atm. At the same temperature, a second reaction mixture (not at equilibrium) contains pressures of H2 = 0.621 atm, I2 = 0.621 atm, and HI = 0.101 atm. What will be the partial pressure of HI when the second reaction mixture reaches equilibrium? a) 0.0144 atm b)...

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?)

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

Subjects