For the chemical reaction system described by the diagram below, which statement
ID: 506770 • Letter: F
Question
For the chemical reaction system described by the diagram below, which statement is true? A. The forward reaction is endothermic B. The activation energy for the forward reaction is greater than the activation energy for the reverse reaction. C. At equilibrium, the activation energy for the forward reaction is equal to the activation energy for the reverse reaction. D. The activation energy for the reverse reaction is greater than the activation energy for the forward reaction. E. The reverse reaction is exothermic. When the temperature of a gas whose activation energy is 55 kJ/mol is increased from 300 K to 320 K, the fraction of collisions with sufficient energy to react. A. decreases by a factor of 2. B. decreases by a factor of 4. C increases by a factor of 2. D. increases by a factor of 4. Which general rate law below corresponds to an elementary bimolecular reaction? A. Rate = k[A] B. Rate = k[A][B][C] C. Rate = k [A]2[B] D. Rate = k[A][B]Explanation / Answer
From the diagram, we know that activation energy for the reverse reaction is greater than that of forward reaction.
Also from the graph, energy of product is less than that of reactant which means the forward reaction is exothermic. At equilibrium, activation energy of forward reaction is equal to that of reverse reaction.
Ans 15
When the temperature increases the rate of the reaction increases.A rise in 100 temperature double the fraction of collision with sufficient energy to react. Therefore increasing temperature from 300K to 320K will increase it by a factor of 4.
Ans 16
In a bimolecular reaction, the rate of reaction depends on the product of concentration of both the species involved in the reaction.
Therefore rate= k[A][B]