Multiple Choice
Which of the following reacting molecules are able to produce products the fastest?
15. Chemical Kinetics
Factors Influencing Rates
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Calculate the activation energy for the reaction that has a rate constant of 0.124 s–1 at 125.0 °C and a rate constant of 0.345 at 200.0 °C.
A
–2.84 kJ
B
–21.4 kJ
C
+2.57 kJ
D
+2.84 kJ
E
+21.4 kJ
Verified step by step guidance1
Identify the given values: rate constant k1 = 0.124 s-1 at T1 = 125.0 °C and rate constant k2 = 0.345 s-1 at T2 = 200.0 °C.
Convert the temperatures from Celsius to Kelvin by adding 273.15 to each temperature: T1 = 125.0 + 273.15 K and T2 = 200.0 + 273.15 K.
Use the Arrhenius equation in its logarithmic form: ln(k2/k1) = (Ea/R) * (1/T1 - 1/T2), where Ea is the activation energy and R is the gas constant (8.314 J/mol·K).
Rearrange the equation to solve for the activation energy Ea: Ea = R * ln(k2/k1) / (1/T1 - 1/T2).
Substitute the known values into the equation and solve for Ea, ensuring that the units are consistent throughout the calculation.
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