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.)

Expert Solution

1)
ICE Table:

[HI] [H2] [I2]

initial 0.69 0 0

change -2x +1x +1x

equilibrium 0.69-2x +1x +1x

Equilibrium constant expression is
Kc = [H2]*[I2]/[HI]^2
0.016 = (1*x)^2/(0.69-2*x)^2
sqrt(0.016) = (1*x)/(0.69-2*x)
0.1265 = (1*x)/(0.69-2*x)
0.08728-0.25298*x = 1*x
0.08728-1.25298*x = 0
x = 0.06966

At equilibrium:
[H2] = x = 0.06966 M

Answer: 0.070 M

Only 1 question at a time please

queen_honey_blossom answered 2 years ago

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).

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?

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?

H2 + I2 yields 2HI At the start of the reaction 1 mole of I2 and...

H2 + I2 yields 2HI At the start of the reaction 1 mole of I2 and 1 mole of H2 are put into a 10 liter container. There is no HI present. At the reaction temperature Keq is 64 What is the equilibrium concentrations for H2, I2 and HI?

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)...

A student ran the following reaction in the laboratory at 720 K: H2(g) + I2(g) 2HI(g)...

A student ran the following reaction in the laboratory at 720 K: H2(g) + I2(g) 2HI(g) When she introduced 0.189 moles of H2(g) and 0.218 moles of I2(g) into a 1.00 liter container, she found the equilibrium concentration of I2(g) to be 6.05×10-2 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc =

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. The following reaction was performed in a sealed vessel at 732 ∘C : H2(g)+I2(g)⇌2HI(g) Initially,...

1. The following reaction was performed in a sealed vessel at 732 ∘C : H2(g)+I2(g)⇌2HI(g) Initially, only H2 and I2 were present at concentrations of [H2]=3.25M and [I2]=3.00M. The equilibrium concentration of I2 is 0.0600 M . What is the equilibrium constant, Kc, for the reaction at this temperature? Express your answer numerically. 2. The decomposition of HI(g) is represented by the equation: 2HI(g)⇌H2(g)+I2(g) The following experiment was devised to determine the equilibrium constant of the reaction. HI(g) is introduced...

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...

Consider the reaction: H2(g)+I2(g)⇌2HI(g) A reaction mixture in a 3.65 L flask at a certain temperature...

Consider the reaction: H2(g)+I2(g)⇌2HI(g) A reaction mixture in a 3.65 L flask at a certain temperature initially contains 0.764 g H2 and 97.0 g I2. At equilibrium, the flask contains 90.5 g HI. Calculate the equilibrium constant (Kc) for the reaction at this temperature. Kc = ?

Question