Consider the first order reaction: A → products studied at 277 K. If the rate constant, k, is found to be 0.571 1/s, and the Arrhenius factor, A, is 1.649, what is the activation energy for the reaction?
Consider the first order reaction: A → products studied at 277 K. If the rate constant, k, is found to be 0.571 1/s, and...
The rate constant for a first-order reaction is 1.8 × 10–2 s–1 at 664 K and 5.0 × 10–2 s–1 at 892 K. What is the activation energy? (R = 8.3145 J/mol · K)
The reaction A + 2B → Products was studied and found to have the rate law: Rate = k[A][B]2. By what factor will the rate increase if the concentration of B is tripled while the concentration of A is held constant?
The rate constant for this second-order reaction is 0.430 M-'.s at 300 °C. A- products How long, in seconds, would it take for the concentration of A to decrease from 0.670 M to 0.310 M? 1 = 6.355 Incorrect Calculate the rate constant, k, for a reaction at 56,0 °C that has an activation energy of 88.6 kJ/mol and a frequency factor of 6.85 x 10's-1 k= 2.2188 SI Incorrect
T'(K) k(s-1 400 0.000659 The rate of a certain reaction was studied at various temperatures. The table shows temperature (T) and rate constant (k) data collected during the experiments. Plot the data to answer the questions. 420 0.00327 440 0.0181 What is the value of the activation energy, Eq, for this reaction? 460 0.0589 480 0.213 500 0.615 520 1.66 1 Ea = kJ · mol-1 540 3.99 560 9.64 OG TOOLS What is x102 Itial factor (sometimes called the...
For a first order reactiomA-----> B, rate constant k for the reaction follows the equation: ln k= (5000/T) + 13.82 find the frequency factor A and the activation energy Ea
The rate of the elementary reaction C2H2 + O2C2H + HO2 has been studied as a function of temperature between 300 and 2500 K. The following data were obtained for the rate constant k: Temperature (K) k (L mol-1 s-1) 300 6.25×10-45 740 1.19×10-12 1180 1.91×10-4 1620 1.07 (a) Calculate the activation energy of this reaction. kJ mol-1 (b) Calculate the factor A in the Arrhenius equation for the temperature dependence of the rate constant. L mol-1 s-1
1) The rate constant for the reaction 2 N,Os(9) = 4 NO (9) + O2(9) is reported in units of sl. What is the overall order of the reaction? 2) The rate law for a reaction was reported as rate=k[A] [B][C] with molar concentrations in moles per cubic decimetre and time in seconds. What are the units of k? 3) The rate constant for the pseudo first-order acid- catalysed hydrolysis of glucose is 4.07' 10-s. Calculate the half-life for the...
Variation of the rate constant with temperature for the first-order reaction 2N2(g) + O(g) → 2N2O4(g) is given in the following table. Determine the activation energy and pre-exponential factor for the reaction. What would be the rate constant at 350 K? Temperature / K Rate Constant / s-1 273 7.87 x 103 298 3.46 x 105 318 4.98 x 106 338 4.87 x 107 What is the activation energy in kJ/mol? Do not enter the units with your answer. What...
Consider the reaction 2HI(g)→H2(g)+I2(g). At 585 K, the rate constant is 9.64×10−5Lmol s. At 690. K, the rate constant is 2.83×10−3Lmol s. Use the Arrhenius equation to calculate the activation energy for the reaction. Ea=−R[lnk2−lnk1(1T2)−(1T1)] Provide your answer below:
A first order reaction has a rate constant of 0.14 at 24 oC. Given that the Arrhenius constant for the reaction is 4.34 x 1010 sec -1, calculate the value of the activation energy in KILOJOULES (enter answer to 1 decimal place)