Synthesis gas, a mixture that includes the fuels CO and H₂,is used to produce liquid hydrocarbons and methanol. It is madeat pressures up to 100 atm by oxidation of methane followed bythe steam re-forming and water-gas shift reactions. Because theprocess is exothermic, temperatures reach 950–1100C, and theconditions are such that the amounts of H₂, CO, CO₂, CH₄, and H₂O leaving the reactor are close to the equilibrium amounts forthe steam re-forming and water-gas shift reactions:CH₄(g) +H₂O(g) ⇌CO(g)+ 3H₂(g) (steam re-forming)CO(g) +H₂O(g) ⇌CO₂(g)+ H₂g) (water-gas shift) (a) At 1000.°C, what are ΔG° and ΔH° for the steam re-formingreaction and for the water-gas shift reaction? (b) By doubling the steam re-forming step and adding it to thewater-gas shift step, we obtain the following combined reaction:2CH₄(g) +3H₂O(g) ⇌CO₂(g) +CO(g)+ 7H₂(g) Is this reaction spontaneous at 1000.°C in the standard state? (c) Is it spontaneous at 98 atm and 50.% conversion (when 50.%of the starting materials have reacted)? (d) Is it spontaneous at 98 atm and 90.% conversion?
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.
Synthesis gas, a mixture that includes the fuels CO and H₂,is used to produce liquid hydrocarbons and methanol. It is madeat pressures up to 100 atm by oxidation of methane followed bythe steam re-forming and water-gas shift reactions. Because theprocess is exothermic, temperatures reach 950–1100C, and theconditions are such that the amounts of H₂, CO, CO₂, CH₄, and H₂O leaving the reactor are close to the equilibrium amounts forthe steam re-forming and water-gas shift reactions:CH₄(g) +H₂O(g) ⇌CO(g)+ 3H₂(g) (steam re-forming)CO(g) +H₂O(g) ⇌CO₂(g)+ H₂g) (water-gas shift) (a) At 1000.°C, what are ΔG° and ΔH° for the steam re-formingreaction and for the water-gas shift reaction? (b) By doubling the steam re-forming step and adding it to thewater-gas shift step, we obtain the following combined reaction:2CH₄(g) +3H₂O(g) ⇌CO₂(g) +CO(g)+ 7H₂(g) Is this reaction spontaneous at 1000.°C in the standard state? (c) Is it spontaneous at 98 atm and 50.% conversion (when 50.%of the starting materials have reacted)? (d) Is it spontaneous at 98 atm and 90.% conversion?
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