Question

In: Chemistry

The dissociation of molecular iodine into iodine atoms is represented as I2(g) ⇌ 2I(g)

The dissociation of molecular iodine into iodine atoms is represented as

I₂(g) ⇌ 2I(g)

At 1000 K, the equilibrium constant K_c for the reaction is 3.80

×

10⁻⁵. Suppose you start with 0.0461 mol of I₂ in a 2.27−L flask at 1000 K. What are the concentrations of the gases at equilibrium?

What is the equilibrium concentration of I₂?

M

What is the equilibrium concentration of I?

M

Expert Solution

I₂(g) ⇌ 2I(g)

I 0.0461 0

C -x 2x

E 0.0461-x 2x

[I-] = 2x/2.27

[I2] = 0.0461-x/2.27

KC = [I-]^2/[I2]

3.8*10^-5 = (2x/2.27)^2/ 0.0461-x/2.27

3.8*10^-5 = 4x^2/2.27(0.0461-x)

3.8*10^-5 *(0.0461-x)*2.27 = 4x^2

x = 0.000986

[I-] = 2x/2.27 = 2*0.000986/2.27 = 0.000868M

[I2] = 0.0461-x/2.27 = 0.0461-0.000986/2.27 = 0.0451/2.27 = 0.0198M

queen_honey_blossom answered 2 years ago

Consider the gas phase dissociation of iodine I2(g)↔2I(g) A. Calculate the thermal wavelength of 127I at...

Consider the gas phase dissociation of iodine I2(g)↔2I(g) A. Calculate the thermal wavelength of 127I at T=298K. B. Calculate the translational partition function of 127I at T=298K. Assume P=1.00atm and V=24.4L. C. Calculate the rotational partition function of I2 at T=298K. Assume θrot=0.0537K D. Calculate the vibrational partition function of I2 atT=298K if teh vibrational temperature of I2 is θvib=308K E. Using the result from Part B, calculate the partition function of I. Assume the ground electronic state degeneracy of...

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]=

Some free radical chemical reactions start with the photodissociation of I2 molecules into Iodine atoms (gas...

Some free radical chemical reactions start with the photodissociation of I2 molecules into Iodine atoms (gas phase) by light with a wavelength shorter than about 792nm. A 100.0mL glass tube, pressure= 55.7mtorr and temperature 25.0C contains I2 molecules What minimum amount of energy must be absorbed by the iodine in the tube to dissociate 15% of the the molecules?

Consider the sublimation of iodine at 25.0 °C. I2(s) → I2(g) a. Find ΔG°rxn at 25.0...

Consider the sublimation of iodine at 25.0 °C. I2(s) → I2(g) a. Find ΔG°rxn at 25.0 °C. b. Find ΔGrxn at 25.0 °C under the following nonstandard conditions: i. PI2 = 1.00 mmHg ii. PI2 = 0.100 mmHg c. Explain why iodine spontaneously sublimes in open air at 25 °C. 2) Balance the following redox reaction in basic aqueous solution. Cl2(g) → Cl– (aq) + ClO– (aq)

Iodine and bromine react to give iodine monobromide, IBr I2+Br2 is in equilibrium to yield 2IBr...

Iodine and bromine react to give iodine monobromide, IBr I2+Br2 is in equilibrium to yield 2IBr What is the equilibrium composition of a mixture at 115°C that initially contained 1.30 x 10 to the negative third 1.30 mol each of iodine and bromine in a 5.00 L vessel? The equilibrium constant Kc for this reaction at 115°C is 55.8. I2 = M ? Br2= M ? IBr= M ?

The consumption function for a certain economy is given by C = I2 + 15 2I...

The consumption function for a certain economy is given by C = I2 + 15 2I + 10 where C and I are both in billions of dollars. Find and interpret both MPC and MPS when I = 55.

Part A Calculate Kc for the reaction below. I2(g)⇌2I(g)Kp=6.26×10−22 (at 298 K) Express your answer using...

Part A Calculate Kc for the reaction below. I2(g)⇌2I(g)Kp=6.26×10−22 (at 298 K) Express your answer using three significant figures. Kc=? Part B Calculate Kc for the reaction below. CH4(g)+H2O(g)⇌CO(g)+3H2(g)Kp=7.7×1024 (at 298 K) Express your answer using two significant figures. Kc=

Using the following reduction potentials: I2(s) + 2e- <---> 2I-(aq) E0 = 0.535 V I2 (aq)...

Using the following reduction potentials: I2(s) + 2e- <---> 2I-(aq) E0 = 0.535 V I2 (aq) +2e- <---> 2I-(aq) E0 = 0.620 V I3-(aq) + 2e- <---> 3I-(aq) E0 = 0.535 V a) Calculate the equilibrium constant for I2(aq) + I-(aq) <---> I3-(aq) b) Calculate the equilibrium constant for I2(s) + I-(aq) <---> I3-(aq) c) Calculate the solubility (g/L) of I2(s) in water.

Consider the reaction of I2 (g) described by I2 (g) = 2 I (g). The total...

Consider the reaction of I2 (g) described by I2 (g) = 2 I (g). The total pressure and partial pressure of I2 (g) at 14000C have been measured to be 36.0 torr and 28.1 torr, respectively. Use these data to calculate KP0, K0c, and Kx at 14000C. Calculate xI under these conditions? What would X1 be if we decreased the total pressure to 36.0×10-6 torr? What would X1 be if we increased the total pressure to 36.0 atm?

Sulfide in a water sample is coulometrically titrated with iodine (H2S + I2 ----> S +...

Sulfide in a water sample is coulometrically titrated with iodine (H2S + I2 ----> S + 2H+ + 2I-). If a 10.00 mL aliquot of the water sample requires a current of 0.75 A for 5.4 minutes to reach the end point, what is the molarity of the sulfide in the water sample? (A) 0.5036 (B) 0.1259 (C) 0.0051 (D) 0.0013