Gaseous hydrochloric acid is produced from molecular hydrogen and molecular chlorine according to the following three-step mechanism at 20 °C. The enthalpy energetic is based on 0.17 mol starting material. Remember as a rule of thumb that for every 10° increase in temperature, the reaction rate doubles. (Show complete work for full credit) Step 1: (fast) Cl2 (g) 2C1 (g) Et = 80 kJ AH1 = 50 kJ Eacti = 60 kJ Step 2: (fast) H2 (g) Cl (g) = H2CI (g) Ez* = 90 kJ AH2 = -25kJ E act1 kJ +] Step 3: (slow) H2CI (9) • Cl (g) → 2HCI (9) E, = 110kJ AH3 = _ kJ EHCI =- 10 kJ Write the net reaction. What is/are the intermediate(s) for this reaction? What is the catalyst? a. Net Rxn: Intermediates: Catalyst: b. What is the rate constant for this reaction at 20.00 °C? Include the value of K and the units. Use A = 5,550-107 M s!
Catalysis and Enzymatic Reactions
Catalysis is the kind of chemical reaction in which the rate (speed) of a reaction is enhanced by the catalyst which is not consumed during the process of reaction and afterward it is removed when the catalyst is not used to make up the impurity in the product. The enzymatic reaction is the reaction that is catalyzed via enzymes.
Lock And Key Model
The lock-and-key model is used to describe the catalytic enzyme activity, based on the interaction between enzyme and substrate. This model considers the lock as an enzyme and the key as a substrate to explain this model. The concept of how a unique distinct key only can have the access to open a particular lock resembles how the specific substrate can only fit into the particular active site of the enzyme. This is significant in understanding the intermolecular interaction between proteins and plays a vital role in drug interaction.
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