4) The rate constants for two different reactions are given: for rxn. 1 $$k=4.852x10^8 s^{-1}$$ at 190°C and $$k=2.203x10^4 s^{-1}$$ at 103°C for rxn. 2 $$k=4.852x10^8 s^{-1}$$ at 190°C and $$k=8.886x10^6 s^{-1}$$ at 103°C a) Calculate the activation energy for the two reactions. b) Find out the temperature rises needed to double the reaction rate, at 103°C for each reaction. c) Comment on the results of part a and b.
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314 J/mol·K), and T is the temperature in Kelvin. We can use the two given rate constants and temperatures for each reaction to solve for Ea. We can rewrite the Arrhenius equation as: $$ln(k) = ln(A) - \frac{E_a}{RT}$$ Using two different temperatures and rate Show more…
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A) The activation energy of a certain reaction is 48.4 kJ/mol. At 23 °C, the rate constant is 0.0120 s^(-1). At what temperature in degrees Celsius would this reaction go twice as fast? B) The initial rate constant is 0.0120 s^(-1) at an initial temperature of 23 °C. What would the rate constant be at a temperature of 130 °C for the same reaction described in Part A? C) A certain reaction has an activation energy of 66.0 kJ/mol and a frequency factor of A1 = 3.70×10^(12) M^(-1)s^(-1). What is the rate constant, k, of this reaction at 30.0 °C? Express your answer with the appropriate units. Indicate the multiplication of units explicitly either with a multiplication dot (asterisk) or a dash. D) An unknown reaction was observed, and the following data were collected: T (K) k (M^(-1)·s^(-1)) 352 109 426 185 Determine the activation energy for this reaction. Express your answer with the appropriate units.
Madhur L.
(a) A certain first-order reaction has a rate constant of $2.75 \times 10^{-2} \mathrm{s}^{-1}$ at $20^{\circ} \mathrm{C}$ . What is the value of $k$ at $60^{\circ} \mathrm{C}$ if $E_{a}=75.5 \mathrm{kJ} / \mathrm{mol} ?(\mathbf{b})$ Another first-order reaction also has a rate constant of $2.75 \times 10^{-2} \mathrm{s}^{-1}$ at $20^{\circ} \mathrm{C} .$ What is the value of $k$ at $60^{\circ} \mathrm{C}$ if $E_{a}=125 \mathrm{kJ} / \mathrm{mol} ?(\mathbf{c})$ What assumptions do you need to make in order to calculate answers for parts (a) and (b)?
Two reactions (i) $A \rightarrow$ products, (ii) $B \rightarrow$ products, follows first order kinetics. The rate of the reaction: $(i)$ is doubled when the temperature is raised from $300 \mathrm{~K}$ to $310 \mathrm{~K}$. The half life for this reaction at $310 \mathrm{~K}$ is 30 minutes. At the same temperature $B$ decomposes twice as fast as $A$. If the energy of activation for the reaction, (ii) is half that of reaction (i), calculate the rate constant of the reaction (ii) at $300 \mathrm{~K}$.
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Topic 2 : Effect of Temperature and Catalyst on Rate of Reactions, Collosion Theory of Chemical Reactions
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