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 =

Solutions

Expert Solution

H2(g) + I2(g) <=====> 2HI(g)

I 0.189 0.218 0

C -x -x 2x

E 0.189-x 0.218 -x 2x

but he has given equilibrium concentration I2 = 0.0605

0.218 -x = 0.0605

x = 0.218 - 0.0605 = 0.1575

[H2] = 0.189-x = 0.189 - 0.1575 = 0.0315 M

[HI] = 2x = 2 x 0.1575 = 0.315

Kc = [HI]2 / [H2] [I2]

Kc = [0.315]2 / [0.0315] [ 0.0605]

Kc = 0.099225 / 0.00190 = 52.066

queen_honey_blossom answered 1 year ago

Next > < Previous

Related Solutions

The following reaction was performed in a sealed vessel at 720 ∘C : H2(g)+I2(g)⇌2HI(g) Initially, only...

The following reaction was performed in a sealed vessel at 720 ∘C : H2(g)+I2(g)⇌2HI(g) Initially, only H2 and I2 were present at concentrations of [H2]=3.50M and [I2]=2.90M. The equilibrium concentration of I2 is 0.0600 M . What is the equilibrium constant, Kc, for the reaction at this temperature?

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.)

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?

A student ran the following reaction in the laboratory at 445 K : PCl5(g)-------> PCl3(g) +...

A student ran the following reaction in the laboratory at 445 K : PCl5(g)-------> PCl3(g) + Cl2(g) When she introduced 1.28 moles of PCl5(g) into a 1.00 liter container, she found the equilibrium concentration of PCl5(g) to be 1.24 M. Calculate the equilibrium constant, Kc, she obtained for this reaction.

1. A student ran the following reaction in the laboratory at 582 K: CO(g) + Cl2(g)...

1. A student ran the following reaction in the laboratory at 582 K: CO(g) + Cl2(g) COCl2(g) When she introduced 0.380 moles of CO(g) and 0.403 moles of Cl2(g) into a 1.00 liter container, she found the equilibrium concentration of COCl2(g) to be 0.342 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. 2. The equilibrium constant, Kc, for the following reaction is 1.29×10-3 at 540 K. COCl2(g) CO(g) + Cl2(g) When a sufficiently large sample of COCl2(g)...

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 684 K: N2(g) + 3H2(g) 2NH3(g)...

A student ran the following reaction in the laboratory at 684 K: N2(g) + 3H2(g) 2NH3(g) When she introduced 3.26×10-2 moles of N2(g) and 6.07×10-2 moles of H2(g) into a 1.00 liter container, she found the equilibrium concentration of H2(g) to be 5.83×10-2 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc = __

-A student ran the following reaction in the laboratory at 1143 K: 2SO2(g) + O2(g) 2SO3(g)...

-A student ran the following reaction in the laboratory at 1143 K: 2SO2(g) + O2(g) 2SO3(g) When she introduced 8.19×10-2 moles of SO2(g) and 8.56×10-2 moles of O2(g) into a 1.00 liter container, she found the equilibrium concentration of O2(g) to be 6.08×10-2 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc =____________ -A student ran the following reaction in the laboratory at 363 K: CH4(g) + CCl4(g) 2CH2Cl2(g) When she introduced 4.64×10-2 moles of CH4(g) and...

A student ran the following reaction in the laboratory at 291 K: 2CH2Cl2(g) CH4(g) + CCl4(g)...

A student ran the following reaction in the laboratory at 291 K: 2CH2Cl2(g) CH4(g) + CCl4(g) When she introduced 6.63×10-2 moles of CH2Cl2(g) into a 1.00 liter container, she found the equilibrium concentration of CH2Cl2(g) to be 4.92×10-3 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc = _____

A student ran the following reaction in the laboratory at 610 K: CO(g) + Cl2(g) COCl2(g)...

A student ran the following reaction in the laboratory at 610 K: CO(g) + Cl2(g) COCl2(g) When she introduced 0.183 moles of CO(g) and 0.211 moles of Cl2(g) into a 1.00 liter container, she found the equilibrium concentration of Cl2(g) to be 6.72×10-2 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. 2.A student ran the following reaction in the laboratory at 546 K: COCl2(g) CO(g) + Cl2(g) When she introduced 0.854 moles of COCl2(g) into a 1.00...

Subjects