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Question 6 2 pts The variation of the rate constant with temperature for the decomposition of...
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...
The reaction 2N0(g) + C12(g) --+2NOCl(g) was studied at 1o°C. The following results were obtained where Δ[C12] Rate Initial Rate (mol/L-min) INOlo (mol/L) [Clalo (mol/L 0.10 0.10 0.20 0.10 0.20 0.20 0.18 0.36 1.45 a. What is the rate law? b. What is the value of the rate constant? (2) The rate law for the reaction at some temperature is: NOBr a. If the half-life for this reaction is 2.00 s when [NOBro 0.900 M, calculate the value of k...
Calculate the activation energy for the decomposition of hydrogen iodide (HI), if at 573K the rate constant is 2.91E-6 M/s; and at 773K the rate constant is 7.65E-2 M/s. Note: answer should be 187.38 kJ/mol Calculate the activation energy for the decomposition of hydrogen iodide (HI), if at 573 °K the rate constant is 2.91 x 106 M/s; and at 773 "K the rate constant is 7.65 x 102 M/s. a. -1.41 kJ/mol b. 187.38 kJ/mol c. 10.18 kJ/mol d....
The rate constant for the decomposition of N,Os(8) at a certain temperature is 1.70x10sl. (a) If the initial concentration of N;O(8) is 0.200 mol/L, How long will it take for the concentration to fall to 0.100 mol/L? (b) What will the concentration of N:Os(8) be after 16 hours of reaction?
The rate constant for mercury fulminate decomposition is 4.0 × 10₋8 s₋1 at 298 K, and the energy of activation is 105 kJ/mol. At what temperature (K) is the rate constant 0.16 s-1? Enter your answer as an integer.
For the gas phase decomposition of 2-bromopropane, CH3CHBCH2– CH2CH=CH2 + HBr the rate constant has been determined at several temperatures. When In k in sis plotted against the reciprocal of the Kelvin temperature, the resulting linear plot has a slope of -2.55*10* K and a y-intercept of 29.9. The activation energy for the gas phase decomposition of 2-bromopropane is kJ/mol.
Another study of the decomposition of ClO determined the rate constant vs. temperature resulting in the following data: T (K) K (M-1s-1) 238 1.9 x 109 258 3.1 x 109 278 4.9 x 109 298 7.2 x 109 Use an Arrhenius plot to determine the activation energy (Ea) and the frequency factor (A). Show all work
i need 2,3,4,5,and 6. 2. (6 Pts) Write the equilibrium expression, Kp, for the reactions in problem 1. 3. (8 Pts) At 127°C, Kc = 2.6 x 10-5 for the reaction: 2 NH3(g) + N2(g) + 3 H2(g) Calculate Kp at this temperature. 4. (10 Pts) A 1.00-L flask was filled with 2.00 mol gaseous SO2 and 2.00 mol gaseous NO, and heated. After equilibrium was reached, it was found that 1.30 mol gaseous NO was present. Assume that the...
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...
Question 6 (18 marks) (a) Given that the rate constant k for the first-order decomposition of compound X is 2.65 x 10-9 s', calculate the percentage of compound X that has decomposed in the first 2250 seconds after the reaction begins. (4 marks) (b) Consider the first order reaction: W2 → 2 Y. If [W2]=0.8 M initially and 0.17 M after 160 seconds, what will [W2] be after 350 seconds? (4 marks) (c) Data for the reaction 3A + 5B...