Hydrogen peroxide decomposes spontaneously to yield water and oxygen gas according to the reaction equation 2 Н,О, (aq) — 2 Н,0() + 0,(g) The activation energy for this reaction is 75 kJ-mol-!. In the presence of a metal catalyst, the activation energy is lowered to 49 kJ-mol-1. At what temperature would the non-catalyzed reaction need to be run to have a rate equal to that of the metal-catalyzed reaction at 25 °C? T = K

A certain reaction has an activation energy of 39.57 kJ/mol. At what Kelvin temperature will the reaction proceed 5.50 times faster than it did at 337 K? T = K

The decomposition reaction on N2O5 in carbon tetrachloride is 2 N2 O5-----> 4NO2 + O2. The rate law is first order in N2O5. At 64 °C the rate constant is 4.82 X 10-3s-1 (a) write the rate law for the reaction.  (b) what is the rate when the concentration of N2O5  is doubled from 0.0240 M to 0.0480 M?   Group of answer choices A) (a) rate= k[N2O5] (b) the rate doubles to 1.16 x 10E(-4) M/sec   B.) (a) rate= k[N2O5] (b) the rate is halved to 5.8 x 10E(-5) M/sec   C.) (a) rate= k[N2O5] (b) the rate doubles to 2.32 x 10E(-4) M/sec   D.) (a) rate= k[N2O5]0 (b) the rate stays the same

A certain reaction has an activation energy of 60.65 kJ/mol. At what Kelvin temperature will the reaction proceed 3.50 times faster than it did at 357 K? T = K

2a) Briefly explain, in your own words, the difference between the "activation energy" of a reaction and the "net free energy change" of a reaction.

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Rates of Reactions Consider reactions of the type: Reactant 1 + Reactant 2– Products The activation energy, temperature and initial reactant concentrations of four such reactions are as follows: Activation Concentration Concentration Temperature Energy of Reactant 1 of Reactant 2 Reaction A: 40 kJ/mol 15°C 1 M 1 M Reaction B: 40 kJ/mol 40°C 1 M 2 М Reaction C: 40 kJ/mol 15°C 1 M 2 М Reaction D: 50 kJ/mol 15°C 1 M 1 M For each of the following pairs of the above reactions, select the letter label associated with the slower reaction. O A B O B A Ов Assume that the reaction rate is proportional to the product of the reactant concentrations. Any factors affecting reaction rate which are not included in the table are assumed to be the same in all four cases. No calculations are needed. You should arrive at your conclusions from simple inspection of the table entries.

The reaction   C4H8(g)⟶2C2H4(g)   has an activation energy of 262 kJ/mol. At 600.0 K, the rate constant, ? is 6.1×10−8 s−1. What is the value of the rate constant at 770.0 K? k=  ? S^-1

NEED AS SOON AS POSSIBLE   A catalyst decreases the activation energy of a particular exothermic reaction by 20 kJ/mol, to 36 kJ/mol. Assuming that the mechanism has only one step, and that the products are 51 kJ lower in energy than the reactants, sketch approximate energy-level diagrams for the catalyzed and uncatalyzed reactions. What is the activation energy for the uncatalyzed reverse reaction?

Catalysts are used to speed up chemical reactions. Based on the graph above how do they do this?