Question

Kinetics For H2 +I2 ->2HI 103k (1/0Cs)      0.54               2.5               &

Kinetics

For H2 +I2 ->2HI

103k (1/0Cs)      0.54               2.5                   14                    25                    64

T (K)               599                  629                  666                  683                  700

Find Ea and A

Homework Answers

Answer #1

from the data take first two rate constant values and first two temperatures.

when two tempareture are given the Arrehenius equation

K1-------------- rate constant at T1 temperature (low T) = 0.54

K2-------------- rate constant at T2 temperature (high T) = 2.5

T1= 599K

T2=629K

log(k2/k1) =( Ea/2.303R)[1/T1-1/T2]

     log (2.5/0.54) =( Ea/2.303x 8.314 x10^-3)[1/599-1/629]

Ea= 160 kJ/mol

another equation

K= A . e ^-Ea/RT

take first rate constant and temperature

0.54 = A . e ^-160/8.314 x10^-3 x599

A= 4.87 x1013

A= 4.87 x1013 rate constant units

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
For the reaction H2 + I2 (g)2HI (g) with Kc = 54.3 at 698 K, if...
For the reaction H2 + I2 (g)2HI (g) with Kc = 54.3 at 698 K, if the initial amounts were 0.800 mole H2 and 0.500 mole I2 in a 5.25-L vessel at 698 K, write the ICE table, and what will be the amounts of reactants and products (in mole(s)) when equilibrium is attained?
K c is 1.29 × 102 for this reaction: H2(g) + I2(g) ↔ 2HI(g). If 0.18...
K c is 1.29 × 102 for this reaction: H2(g) + I2(g) ↔ 2HI(g). If 0.18 M H2 is initially mixed with 1.20 M I2, what is the concentration of H2 at equilibrium?
For the reaction   2HI(g) ⇌H2(g)+I2(g), Kc= 0.290   at 400 K. If the initial concentration of  HI ...
For the reaction   2HI(g) ⇌H2(g)+I2(g), Kc= 0.290   at 400 K. If the initial concentration of  HI  is  4.0×10−3M and the initial concentrations of  H2, and the initial concentrations of  H2, and I2 are both  1.50×10–3M  at  400 K, which one of the following statements is correct? a. The concentrations of HI and I2 will increase as the system is approaching equilibrium. b. The concentrations of H2 and I2 will increase as the system is approaching equilibrium. c. The system is...
Hydrogen iodide decomposes according to the equation 2HI (g)<---> H2 (g) + I2 (g) for which...
Hydrogen iodide decomposes according to the equation 2HI (g)<---> H2 (g) + I2 (g) for which K= .0156 at 400 degrees celsius. If 0.550 mol of HI was injected into 2.00L reaction vessel at 400 degrees celsuis. Calculate the concentration of H2 at equilibrium?
H2(g) + I2(g) <-> 2HI(g) Kp= 0.456 at 398K Assume that initially there are n moles...
H2(g) + I2(g) <-> 2HI(g) Kp= 0.456 at 398K Assume that initially there are n moles of HI in a varaible volume priston and no moles of H2 and I2 are present. a) Find the partial pressures of HI, HI2, and I2 when the piston is set to give 1.00 bar total pressure. b) Find ΔrGo
A student ran the following reaction in the laboratory at 742 K: H2(g) + I2(g) <<------->>>2HI(g)...
A student ran the following reaction in the laboratory at 742 K: H2(g) + I2(g) <<------->>>2HI(g) When she introduced 0.202 moles of H2(g) and 0.225 moles of I2(g) into a 1.00 liter container, she found the equilibrium concentration of HI(g) to be 0.331 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc =
Consider the chemical equation and equilibrium constant at 25∘C: H2(g)+I2(g)⇌2HI(g) , K=6.2×102 Calculate the equilibrium constant...
Consider the chemical equation and equilibrium constant at 25∘C: H2(g)+I2(g)⇌2HI(g) , K=6.2×102 Calculate the equilibrium constant for the following reaction at 25∘C: HI(g)⇌12H2(g)+12I2(g)
The decomposition of hydrogen iodide, 2HI(g)= H2(g)+I2(g), has a rate constant of 9.51*10-9 L/mol*s at 500K...
The decomposition of hydrogen iodide, 2HI(g)= H2(g)+I2(g), has a rate constant of 9.51*10-9 L/mol*s at 500K and Ea of 176 kJ/mol. At what temperature will the rate constant be 1.10*10-5 L/mol*s?
At a certain temperature, the equilibrium constant, Kc for this reaction is 53.3. H2(g)+I2(g) = 2HI(g)...
At a certain temperature, the equilibrium constant, Kc for this reaction is 53.3. H2(g)+I2(g) = 2HI(g) At this temperature, 0.300 mol of H2 and 0.300 mol of I2 were placed in a 1.00 L container to react. What concentration of HI is present at equilibrium? View comments (1)
-Consider the following reaction: 2HI(g) H2(g) + I2(g) If 3.69 moles of HI(g), 0.570 moles of...
-Consider the following reaction: 2HI(g) H2(g) + I2(g) If 3.69 moles of HI(g), 0.570 moles of H2, and 0.558 moles of I2 are at equilibrium in a 16.6 L container at 818 K, the value of the equilibrium constant, Kc, is_____________ .Consider the following reaction: 2NH3(g) N2(g) + 3H2(g) If 1.31×10-3 moles of NH3(g), 0.681 moles of N2, and 0.495 moles of H2 are at equilibrium in a 18.6 L container at 893 K, the value of the equilibrium constant,...