Consider the hypothetical reaction A2(g) + B2(g) ⟶ 2AB(g), where the rate law is:
The value of the rate constant at 302°C is 2.45 × 10−4 L/mol s, and at 508°C the rate constant is 0.891 L/mol· s. What is the activation energy for this reaction? What is the value of the rate constant for this reaction at 375°C?
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Chapter 11 Solutions
EBK CHEMISTRY: AN ATOMS FIRST APPROACH
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- The following rate constants were obtained in an experiment in which the decomposition of gaseous N2O; was studied as a function of temperature. The products were NO, and NO,. Temperature (K) 3.5 x 10_i 298 2.2 x 10"4 308 6.8 X IO-4 318 3.1 x 10 1 328 Determine Etfor this reaction in kj/mol.arrow_forwardThe following statements relate to the reaction for the formation of HI: H2(g) + I2(g) -* 2 HI(g) Rate = it[HJ [I2J Determine which of the following statements are true. If a statement is false, indicate why it is incorrect. The reaction must occur in a single step. This is a second-order reaction overall. Raising the temperature will cause the value of k to decrease. Raising the temperature lowers the activation energy' for this reaction. If the concentrations of both reactants are doubled, the rate will double. Adding a catalyst in the reaction will cause the initial rate to increase.arrow_forwardBased on the kinetic theory of matter, what would the action of a catalyst do to a reaction that is the reverse of some reaction that we say is catalyzed?arrow_forward
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