What is the value of the activation energy?
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If a reaction has k= 3.0 x 10^-4 s^-1 at 25°C and an activation energy of 100.0 kJ/mol, what will the value of k be at 50°C?
Answer:
You have to use the Arrhenius equation twice: k = A e^(-E/RT) where, k = rate constant at Temperature...
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Other solutions
Answer:
On One Hand: Activation Energy Is a ConstantReaction energy profiles typically show a curve with one...
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Answer:
The activation energy/rate of a reaction are related by the equation k=Aexp(-Ea/RT), where k is rate...
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Answer:
Universally Accepted Activation Energy = 8.314e-3 x ((270 x 300) / (300 - 270)) * ln(1.4e-10 / 1.1e...
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At what temperature (K), would the rate constant increase by a factor of 6.486 to 6.486k? Use R = 8.314 J/K·mol in your calculation
Answer:
Let UNITs guide you; always USE THEM in your calculation to prevent errors Rate1 = A e^(-E/RT1) Rate...
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I have a value of activation energy at one temperature and need to estimate it at another but do not have any data at this other temperature
Answer:
What varies with temperature is not the activation energy, but the rate of reaction. Activation energy...
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if the following exothermic chemical reaction has an activation energy value measured to be 54kcal/mole and its heat of reaction value is measrued to be -42kcal/mole CO+Cl2= COCl2 ...show more
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Rate constants for the reaction NO2+CO > NO+CO2 are 1.3 1/M*s at 700K and 23.0 1/M*s at 800K. 1) What is the value of the activation energy in kJ/mol? 2) What's the rate constant at 730K?
Answer:
1) What is the value of the activation energy in kJ/mol? Use the relation: ln (k'/k) = Ea/R ( 1/T- ...
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if the following exothermic chemical reaction has an activation energy value measured to be 54kcal/Mole and its heat of reaction valur is measured to be -42kcal/Mole CO(g) + Cl2(g)= ...show more
Answer:
Let Er = Energy of reactant; Ep = Energy of product; E* = Energy of activated complex and Ea = Energy...
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Activation energy is 1. the energy released when products are formed. 2. the maximum amount of energy that can be used during a reaction. 3. the energy of the chemically active reactant. 4. the energy required to initially start a chemical reaction....
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