Sketch the reaction profile for a reaction having Ea = 50 kJ/mol and (change in)Hrxn = -75 kJ/mol. Suppose that in the presence of a catalyst the activation energy is reduced to 25 kJ/mol. Sketch the reaction profile of the catalyzed reaction on the same sketch you drew for the uncatalyzed reaction. Make sure to label each axis, (change in)H for the reaction, and Ea for the catalyzed and uncatalyzed reactions in both the forward and reverse directions.

The activation energy for the gas phase isomerization of dimethyl maleate is 111 k). cis-CH300CCH=CHCO0OCH3→trans-CH300CCH=CHCOOCH3 The rate constant at 678 K is 3.77×10 4 /s. The rate constant will be 3.08×103/s at K.

Examine the 2-step mechanism below and identify the substance that appears to be a catalyst and anintermediate, respectively.Step 1. A + BC → AC + BStep 2. AC + D → A + CD(a) A = catalyst, AC = intermediate(b) AC = catalyst, A = intermediate(c) A = catalyst, B = intermediate(d) D = catalyst, AC = intermediate

A certain catalyzed reaction is known to have an activation energy E=66.0 kJ/mol. Furthermore, the rate of this reaction is measured at 351. K and found to be 1.5x 10-2M/s. Use this information to answer the questions in the table below. Suppose the concentrations of all reactants is kept the same, but the temperature is lowered by 10% from 351. K to 316. K. How will the rate of the reaction change? Suppose the concentrations of all reactants is kept the same, but the catalyst is removed, which has the effect of raising the activation energy by 10%, from 66.0 kJ/mol to 72.6 kJ/mol. How will the rate of the reaction change? The rate will The rate will choose one choose one stay the same rise about 10% rise more than 10% rise less than 10% fall about 10% fall more than 10% fall less than 10%

Calculate the activation energy for the reaction (in kj/mol) when at 795 K the rate constant for the reaction shown below is 0.0000650, and at 370 K the rate constant is 0.00000300. 2N2O5(g) to 4NO(g) + 3O2(g)

Calculate the activation energy for the reaction (in kJ/mol) when at 675 K the rate constant for the reaction shown below is 0.0000860, and at 424 K the rate constant is 0.00000200 . 2N2O5(g)→4NO(g)+3O2(g)

At 10oC and 50oC the first-order rate constants of a reaction are 9.88 x 10-4 and 9.45 x 10-2 s-1 respectively. What is the activation energy (kJ/mole)? (R = 8.31 J/mole oK). 87.2 78.2 27.8 28.7

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= O KINETICS AND EQUILIBRIUM Using the Arrhenius equation to calculate Ea from k versus T data The rate constant k for a certain reaction is measured at two different temperatures: k 81.0 °C 4.0×10¹¹ 137.0 °C 1.6x10¹2 temperature Assuming the rate constant obeys the Arrhenius equation, calculate the activation energy E for this reaction. Round your answer to 2 significant digits. E = 0 mol x10 X 1/5

Which of the following statements is  true?     A catalyst raises the activation energy of a reaction.     The addition of a homogeneous catalyst does not change the activation energy of a given reaction.     The rate constant does not depend on the activation energy for a reaction where the products are lower in energy than the reactants.     Rate constants are temperature dependent.     None of the above are true.