Open Question
What rate law corresponds to the proposed mechanism for the formation of hydrogen iodide, which can be written in simplified form as: I2 Δk1k-1 2I (Fast), I + H2 Δk2k-2 H2I (Fast), H2I + I ¡k3 2HI (Slow)?
Ch.14 - Chemical Kinetics
Chapter 14, Problem 111
The energy of activation for the decomposition of 2 mol of HI to H2 and I2 in the gas phase is 185 kJ. The heat of formation of HI(g) from H2(g) and I2(g) is -5.65 kJ/mol. Find the energy of activation for the reaction of 1 mol of H2 and 1 mol of I2 to form 2 mol of HI in the gas phase.
Verified step by step guidance1
Identify the given data: the activation energy for the decomposition of 2 mol of HI is 185 kJ, and the heat of formation of HI is -5.65 kJ/mol.
Understand that the activation energy for the reverse reaction (formation of HI) can be found using the relationship between the activation energies of the forward and reverse reactions and the enthalpy change of the reaction.
Calculate the enthalpy change (ΔH) for the formation of 2 mol of HI using the given heat of formation: ΔH = 2 mol × (-5.65 kJ/mol).
Use the equation for the activation energy of the reverse reaction: E_a(reverse) = E_a(forward) - ΔH, where E_a(forward) is the activation energy for the decomposition of HI.
Substitute the known values into the equation to find the activation energy for the formation of HI.
Related Practice
Textbook Question
A certain substance X decomposes. Fifty percent of X remains after 100 minutes. How much X remains after 200 minutes if the reaction order with respect to X is (c) second order?
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Textbook Question
The half-life for radioactive decay (a first-order process) of plutonium- 239 is 24,000 years. How many years does it take for one mole of this radioactive material to decay until just one atom remains?
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Open Question
Ethyl chloride vapor decomposes by the first-order reaction: C2H5Cl -> C2H4 + HCl. The activation energy is 249 kJ/mol, and the frequency factor is 1.6 * 10^14 s^-1. Find the temperature at which the rate of the reaction would be twice as fast.
Textbook Question
Ethyl chloride vapor decomposes by the first-order reaction: C2H5Cl → C2H4 + HCl The activation energy is 249 kJ/mol, and the frequency factor is 1.6⨉1014 s-1. Find the value of the rate constant at 710 K.
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Textbook Question
Ethyl chloride vapor decomposes by the first-order reaction: C2H5Cl → C2H4 + HCl The activation energy is 249 kJ/mol, and the frequency factor is 1.6⨉1014 s-1. What fraction of the ethyl chloride decomposes in 15 minutes at this temperature?
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