a.) The rate constant for the base-catalyzed hydrolysis of ethyl acetate is 1.78×103 L mol-1 s -1 at 25 °C and 1.38×104 L mol-1 s -1 at 37 °C. Calculate EA, (delta)H‡ , the Arrhenius Constant, and (delta) S ‡ .
b.) The isomerization of HNC into HCN is important in the chemistry of interstellar gas clouds. HNC → HCN Has an activation energy of 210 kJ/mol and an activation entropy of -105 J mol-1 K-1 . Calculate the first-order rate constant at 30 K (temperature of a “hot” gas cloud).
a.) The rate constant for the base-catalyzed hydrolysis of ethyl acetate is 1.78×103 L mol-1 s...
1) Calculate the activation energy in kJ/mol for the following reaction if the rate constant for the reaction increases from 93.5 M-1s-1 at 497.7 K to 1349.3 M-1s-1 at 636.7 K. do not include units, but make sure your answer is in kJ/mol! 2) A chemist constructs a plot of ln k vs. 1/T for a chemical reaction. The slope of the trendline for the data is -746 K. What is the activation energy for this reaction in kJ/mol? R...
for the gas phase decomposition of ethyl chloroformate, CICOOC2H5————-> C2H5CI + CO2 the rate constant at 427 K is 4.20x10^-5 s^-1 and the rate constant at 467 K is 8.17x10^-4 s^-1. what is the activation energy for this reaction? ______kj/mol
There are several factors that affect the rate of a reaction. These factors include temperature, activation energy, steric factors (orientation), and also collision frequency, which changes with concentration and phase. All the factors that affect reaction rate can be summarized in an equation called the Arrhenius equation: k=Ae−Ea/RT, where k is the rate constant, A is the frequency factor, Ea is the activation energy, R=8.314 J mol−1 K−1 is the gas constant, and T is the absolute temperature. A certain...
There are several factors that affect the rate of a reaction. These factors include temperature, activation energy, steric factors (orientation), and also collision frequency, which changes with concentration and phase. All the factors that affect reaction rate can be summarized in an equation called the Arrhenius equation: k=Ae−Ea/RT, where k is the rate constant, A is the frequency factor, Ea is the activation energy, R=8.314 J mol−1 K−1 is the gas constant, and T is the absolute temperature. A certain...
For a certain reaction the specific rate constant, k, is 1.50 x 10-3 L mol-1 s-1 at 27 °C and 1.50 L mol-1 s-1 at 127 °C. For this reaction, the pre-exponential factor, A, in the Arrhenius equation has the value
The lab is the acid catalysed hydrolysis of ethyl acetate. Experimental Pipette 100.0 cm3 of 0.5 M HCl into a conical flask (labeled A) and a further 20.0 cm3 into a second conical flask (labeled B). Prepare 25 cm3 of crushed-ice/water. Pipette 5.0 cm3 of ethyl acetate into flask A, shake well, start the stop watch and immediately withdraw 5.0 cm3 of the solution. Immediately, run this into the crushed-ice water mixture, and swirl to 'stop' the reaction, and as...
1. Pure butanol (A) is fed to a semibatch reactor containing pure ethyl acetate (8) to produce butyl acetate (C) and ethanol (D). The liquid- phase reaction, A + B ㈠ C + D, is elementary and reversible and is carried out isothermally at 300 K. At this temperature, the equilibrium constant, Kc, is 1.08 and the specific reaction rate, k is 9 x 10 5 L mo s1.Initilly, there is 200 L of ethyl acetate in the reactor, and...
For a certain reaction the specific rate constant, k, is 1.50 x 10-3 L mol-1 s-1 at 27 °C and 1.50 L mol-1 s-1 at 127 °C. For this reaction, the pre-exponential factor, A, in the Arrhenius equation has the value A. 8.3 x 103 L mol-1 s-1 B. 1.5 x 109 L mol-1 s-1 C. 1.5 x 106 kJ mol-1 D. 9.7 kJ mol-1 E. 1.5 x 10-3 L mol-1 s-1
For a certain reaction the specific rate constant, k, is 1.50 x 10-3 L mol-1 s-1 at 27 °C and 1.50 L mol-1 s-1 at 127 °C. For this reaction, the pre-exponential factor, A, in the Arrhenius equation has the value A. 8.3 x 103 L mol-1 s-1 B. 1.5 x 10-3 L mol-1 s-1 C. 9.7 kJ mol-1 D. 1.5 x 106 kJ mol-1 E. 1.5 x 109 L mol-1 s-1
Given: Cl(g)+H2(g)→HCl(g)+H(g) Temperature (K) Rate Constant (L/mol⋅s) 90 0.00357 100 0.0773 110 0.956 120 7.781 I found the Ea = 23 kJ/mol, but need help on this one: - Use an Arrhenius plot to determine the frequency factor for the reaction. A = __ s-1