1. The rate constant for a particular reaction is 1.15 × 105s-1 at 23.7 °C and is 6.88 × 105s-1 at 63.2 °C. Calculate the energy of activation, EA for the reaction in kJ/mol.
R = 8.314472 J⋅mol-1⋅K-1. Report your answer to THREE significant figures.
2. What is the correct expression for the equilibrium constant for the following reaction?
2 A + 3 B ⇌ 5 C + 3 D
Kc = [C][D] / [A][B] |
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Kc = [C]5[D]3 / [A]2[B]3 |
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Kc = [C]2[D]6 / [A]2[B] |
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Kc = [C]10[D]6 / [A]4[B]6 |
1. The rate constant for a particular reaction is 1.15 × 105s-1 at 23.7 °C and...
The energy of activation for a particular reaction is 11.1 kJ/mol. At 18.9 °C the rate constant of the reaction is 1.67 × 102s.-1 Calculate the temperature (in °C) when the rate constant, k = 4.99 × 103s.-1 R = 8.314472 J⋅mol-1⋅K-1. Report your answer to THREE significant figures.
A particular reaction has an activation energy, Ea, of 130 kJ/mol. If the rate constant for the reaction is 0.00684 s −1 at 663 °C, at what temperature(in°C) would the rate constant be 0.376 s −1? *Please report 3 significant figures. Numbers only, no unit. No scientific notation.
part 1 Calculate the equilibrium constant at 184 °C for a reaction that has a standard enthalpy of reaction, ΔH° = 30.2 kJ/mol and an equilibrium constant, K = 0.0603 at 10.6 °C. R = 8.314472 J⋅mol−1⋅K−1. Report your answer to THREE significant figures. part 2 The standard enthalpy of reaction (i.e. ΔH°) for a particular reaction is −31.7 kJ/mol. At 24.9 °C the equilibrium constant for the reaction is 3.96 × 10−2. Calculate the temperature (in °C) at which...
QUESTION 18 A particular reaction has an activation energy, Ea, of 108 kJ/mol. If the rate constant for the reaction is 0.00573 s −1 at 498 °C, at what temperature(in°C) would the rate constant be 0.283 s −1? *Please report 3 significant figures. Numbers only, no unit. No scientific notation.
Calculate the equilibrium constant at 177 °C for a reaction that has a standard enthalpy of reaction, ΔH° = 21.3 kJ/mol and an equilibrium constant, K = 0.0612 at 40.5 °C. R = 8.314472 J⋅mol−1⋅K−1. Report your answer to THREE significant figures.
Answer the following questions based on the reaction below. At 463 K, the rate constant for this reaction is 1.35×10-4 /s and at 655 K the rate constant is 1.52×101 /s. cyclopentane → ethene + cyclopropane 1. Determine the activation energy (EA) (in kJ/mol) for this reaction. Report your answer to three significant figures in scientific notation. Tries 0/3 2. Determine the pre-exponential factor, A (in /s) for this reaction. Report your answer to three significant figures in scientific notation (Please...
A reaction has a rate constant of 1.21×10−4 s−1 at 25 ∘C and 0.226 s−1 at 77 ∘C . Part A Determine the activation barrier for the reaction. Express your answer in units of kilojoules per mole and with 3 significant figures. Ea E a = nothing kJ/mol Request Answer Part B What is the value of the rate constant at 18 ∘C ? Express your answer in units of inverse seconds (s−1) and with 3 significant figures. k k...
A particular reaction has an activation energy, Ea, of 108 kJ/mol. If the rate constant for the reaction is 0.00573 s −1 at 498 °C, at what temperature(in°C) would the rate constant be 0.283 s −1?
The activation energy, Ea, for a particular reaction is 19.4 kJ/mol. If the rate constant at 80 °C is 0.820 M⁻¹s⁻¹, then what is the value of the rate constant at 209 °C? (R = 8.314 J/mol • K)
The activation energy, Ea, for a particular reaction is 19.4 kJ/mol. If the rate constant at 80 °C is 0.820 M⁻¹s⁻¹, then what is the value of the rate constant at 121 °C? (R = 8.314 J/mol • K)