Question

In: Chemistry

The gas phase decomposition of hydrogen iodide to hydrogen gas and iodine gas occurs with a...

The gas phase decomposition of hydrogen iodide to hydrogen gas and iodine gas occurs with a rate of 2.35x10^-7 M^-1s^-1 at 283 degree C and 1.62x10^-3 M^-1s^-1 at 427 degree C.

A. What is the activation energy of this reaction in kJ/mole?

B. What is the temperature in Celsius of a reaction that has a rate constant of 2.91x10^-4 M^-1s^-1?

Solutions

Expert Solution

A) 2HI(g)H2(g)+I2(g)

rate of reaction=r=-d[HI]/dt=k[HI]^2, k=rate constant

given

r1=-d[HI]/dt=k1[HI]^2=2.35*10^-7 (at 283k)

r2=-d[HI]/dt=k2[HI]^2=1.62*10^-3 (at 427k)

taking ratio,

r1/r2=k1/k2=2.35*10^-7/1.62*10^-3 =1.45*10^-4

A) Arrhenius equation,

lnK=lnA-Ea/RT

so ln(k1/k2)=Ea/R(1/T2-1/T1)

T1=283+273=556K , T2= 427+273=700K T=temperature,Ea=activation energy,R=gas constant

ln(1.45*10^-4)=Ea/8.314J/K mol(1/700-1/556)

-8.873=Ea/8.314J/K mol(0.00143-0.00180)

-8.873=Ea/8.314J/K mol(-0.00037)

Ea=-8.873*8.314J/K mol/(-0.00037)=199378.708 J/mol=199.379 KJ/mol

B)k3=2.91*10^-4

let T=T3 for this reaction

k1/k3=2.35*10^-7/2.91*10^-4=0.807*10^-3

ln(k1/k3)=Ea/R(1/T3-1/T1)

ln(0.807*10^-3)=199378.708 J/mol/8.314J/k mol(1/T3-1/556)

-7.122=23981.081(1/T3-0.00180)

-2.970*10^-4=(1/T3-0.00180)

1/T3=-2.970*10^-4+0.00180=0.00150

T3=666.667K

queen_honey_blossom answered 1 year ago

Next > < Previous

Related Solutions

A) For the gas phase decomposition of hydrogen iodide at 700 K 2 HIH2 + I2...

A) For the gas phase decomposition of hydrogen iodide at 700 K 2 HIH2 + I2 the average rate of disappearance of HI over the time period from t = 0 s to t = 1446 s is found to be 5.67×10-4 M s-1. The average rate of formation of H2 over the same time period is M s-1. B) The rearrangement of cyclopropane to propene at 500 °C (CH2)3CH3CH=CH2 is first order in (CH2)3 with a rate constant of...

Hydrogen iodide gas decomposes into hydrogen gas and iodine gas at 453°C. If a 2.00 L...

Hydrogen iodide gas decomposes into hydrogen gas and iodine gas at 453°C. If a 2.00 L flask is filled with 0.200 mol of hydrogen iodide gas, 0.156 mol hydrogen iodide remains at equilibrium. What is the equilibrium constant, Kc, for the reaction at this temperature? 2 HI (g) ⇌ H2 (g) + I2 (g)

Rate constants for the gas-phase decomposition of hydrogen iodide, 2 HI(g) → H2 (g) + I2...

Rate constants for the gas-phase decomposition of hydrogen iodide, 2 HI(g) → H2 (g) + I2 (g), are listed in the following table: Temperature (Celcius) k(M-1s-1) 283 3.52*10-7 356 3.02*10-5 393 2.19*10-4 427 1.16*10-3 508 3.95*10-2 (a) Find the activation energy (in kJ/mol) using all five data points. (b) Calculate Ea from the rate constants at 283 °C and 508 °C. (c) Given the rate constant at 283 °C and the value of Ea obtained in part (b), what is...

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]=

The decomposition of solid ammonium hydrogen sulfide to form ammonia gas and hydrogen sulfide gas is...

The decomposition of solid ammonium hydrogen sulfide to form ammonia gas and hydrogen sulfide gas is an endothermic process.A 6.1589-g sample of the solid is placed in an evacuated 4.000-L vessel at 24.00C.After equilibrium is established, the total pressure inside the vessel is 0.709 bar and some of the solid remains in the vessel. a.Calculate KP for the reaction. b.Calculate the percent of the solid that has decomposed. c.If the system was at equilibrium and the volume of the container...

The activation energy for the decomposition of hydrogen iodide is found to be 180 kJ mol–1...

The activation energy for the decomposition of hydrogen iodide is found to be 180 kJ mol–1 and the rate constant for this reaction is reported to be 0.24 mol–1 L min–1at 540 °C. What is k for this reaction at 30 °C? Please show all workings

The following shows the gas phase decomposition of hydrogen peroxide (H2O2) at 400 °C: 2H2O2(g)2H2O(g) +...

The following shows the gas phase decomposition of hydrogen peroxide (H2O2) at 400 °C: 2H2O2(g)2H2O(g) + O2(g) This reaction is second order in H2O2 with a rate constant of 0.650 M-1s-1 and the initial concentration of H2O2 is 0.600 M. a) What is the concentration of H2O2 after 40 second? (extra credit) What is the concentration of O2 at that time? b) Calculate the first and second half-life of this reaction. Are the values same or different? Explain your answer.

Decomposition of NI3 produces nitrogen gas and iodine. How many grams of the reactant would be...

Decomposition of NI3 produces nitrogen gas and iodine. How many grams of the reactant would be required to react completely to give 4.23 g of the iodine?

a) How many grams of hydrogen gas (H2) is produced by the decomposition of 43.7g of...

a) How many grams of hydrogen gas (H2) is produced by the decomposition of 43.7g of ammonia gas (NH3)? b) If 12.0 moles of H2 were produced, how many grams of NH3 was decomposed? c) If 12.0 moles of H2 were produced, how many moles of N2 were produced?

A student obtained the following data for the gas phase decomposition of nitrosyl chloride at 400...

A student obtained the following data for the gas phase decomposition of nitrosyl chloride at 400 K. NOCl(g)NO(g) + ½ Cl2(g) [NOCl], M 8.40×10-2 4.20×10-2 2.10×10-2 1.05×10-2 seconds 0 2.78×104 8.33×104 1.94×105 (1) What is the half-life for the reaction starting at t=0 s? s What is the half-life for the reaction starting at t=2.78×104 s? s Does the half-life increase, decrease or remain constant as the reaction proceeds? (2) Is the reaction zero, first, or second order? (3) Based...

Subjects