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ki Q3: The decomposition mechanism of 2 N2O(g) → 4NO2(g) + O2(g) is believed to follow...
Consider the rate of decomposition: 2 N2O5(g) → 4NO2(g) + O2(g). The rate of reaction will...
Consider the rate of decomposition: 2 N2O5(g) → 4NO2(g) + O2(g). The rate of reaction will be dependent on: A. [N2O5] B. [NO2] C. [O2] D. [NO2] and [O2]
Consider the following reaction on acetone (CH3COCH3), the mechanism is believed to involve four elementary steps:...
Consider the following reaction on acetone (CH3COCH3), the mechanism is believed to involve four elementary steps: CH3COCH; 4+ CH3 + CH3CO CH3 + CH3COCH; CH4 + CH3COCH, CH;COCH2 _ky → CH3 + CH2CO CH3 + CH3COCH, ko > CH3COCZH (a) Write down an expression for the rate of disappearance of CH3COCHz. (3 marks) Assume kz >> k[CH3), apply the steady-state approximation and work out an expression for (CH3) in term of kį, kz, kz and ke. Show all of your...
The nitrogen-monoxide-catalyzed decomposition of dinitrogen monoxide is thought to proceed by a two-step mechanism: NO(g) +...
The nitrogen-monoxide-catalyzed decomposition of dinitrogen monoxide is thought to proceed by a two-step mechanism: NO(g) + N2O(g) --> N2(g) + NO2(g) (slow) 2 NO2(g) --> 2 NO(g) + O2(g) (a) If the first step of this mechanism is rate-determining (slow), choose the correct rate law for the overall process. Rate = k [N2O]2 Rate = k [NO] [NO2] Rate = k [N2O]2 [N2O] Rate = k [NO2] [N2O] Rate = k [N2O] [N2O] Rate = k [NO] [N2O] (b) Choose...
The reaction mechanism for the decomposition of N2O5 is given by the following set of equations:...
The reaction mechanism for the decomposition of N2O5 is given by the following set of equations: N2O5 -> NO2 + NO3 k1 NO2 + NO3 -> N2O5 k2 NO3 -> NO + O2 k3 NO3 + NO -> 2NO2 k4 a) Write the rate expression for the formation of O2. b) Obtain expressions for the steady state concentrations of NO and NO3. c) Using the expressions from (b), write the rate law for the formation of O2.
Step 1: NO(g) + O2(g) ---> NO2(g) + O(g) rate= k1 Step 2: NO(g) + )...
Step 1: NO(g) + O2(g) ---> NO2(g) + O(g) rate= k1 Step 2: NO(g) + ) --> NO2 (g) rate = k2 suppose that k1<<k2, That is the first step is much slower than the second. Write the balanced chem equation for the overall chemical rxn Write the experimentally observable rate law for the overall reaction. (no reaction concentrations) rate=k() Express the rate constant k for the overall reaction in terms of k1, k2 and (if necessary) the rate constant...
9,10,11 9. Consider the decomposition reaction of N2Os. 2 N203(g) → 4NO2(g) + O2(g) follows the...
9,10,11
9. Consider the decomposition reaction of N2Os. 2 N203(g) → 4NO2(g) + O2(g) follows the first order kinetics with rate constant of 4.8 x 10's. (a) if the initial 165 x 10-2M what is the concentration at 825 s? (b) How long it will take for concentration is 1.65 x 10-2M what is the concentrat the concentration of N2Os to decrease to 1.00 x 10-2M? t 10. Nitrosyl chloride, NOCI, decomposes slowly to NO and Cl2, the reaction follows...
12. The following mechanism is proposed for the decomposition of ozone (O3) to O2: 03 + M 02 + 0 + M 0+03 2 02 Apply the steady-state approximation to the concentration of atomic oxygen, and derive t...
12. The following mechanism is proposed for the decomposition of ozone (O3) to O2: 03 + M 02 + 0 + M 0+03 2 02 Apply the steady-state approximation to the concentration of atomic oxygen, and derive the rate law for the decomposition of ozone (M stands for a molecule that can exchange kinetic energy with particles undergoing the chemical reaction.)
12. The following mechanism is proposed for the decomposition of ozone (O3) to O2: 03 + M 02 +...
1A. The decomposition of dinitrogen monoxide (nitrous oxide) occurs in two steps. The mechanism that has...
1A. The decomposition of dinitrogen monoxide (nitrous oxide) occurs in two steps. The mechanism that has been proposed is as follows: Step 1: N2O (g) à N2(g) + O(g) Step 2: N2O (g) + O(g) à N2(g) + O2(g) Write the chemical equation for the overall reaction and identify any reaction intermediates (spectators). What is the molecularity of each of the elementary (steps) reactions?
The thermal decomposition of NO2: 2 NO2(g) → 2 NO(g) + O2(g) takes place in two steps: (1)...
The thermal decomposition of NO2: 2 NO2(g) → 2 NO(g) + O2(g) takes place in two steps: (1) 2 NO2(g) → NO3(g) + NO(g) (slow) (2) NO3 → NO(g) + O2(g) (fast) Which of the following statements is true? a. Rate = k [NO2] b. The reaction is second order in NO2. c. The reaction is first order in O2. d. Increasing [NO2] has no effect on reaction rate. e. All the above.
Can you explain with all necessary steps and equations? thank you 6. The reaction 2 H2...
Can you explain with all necessary steps and equations? thank
you
6. The reaction 2 H2 + 2 NO N2 + 2 H20 may proceed by the following mechanism: 2 NO - N202 (k, and k.1) H2 + N202 N2O + H2O (kz) H + N20 - N2 + H2O (ku). Use the steady-state approximation to predict the rate law for the formation of the product N.
Consider the following reaction on acetone (CH3COCH3), the mechanism is believed to involve four elementary steps: CH3COCH; 4+ CH3 + CH3CO CH3 + CH3COCH; CH4 + CH3COCH, CH;COCH2 _ky → CH3 + CH2CO CH3 + CH3COCH, ko > CH3COCZH (a) Write down an expression for the rate of disappearance of CH3COCHz. (3 marks) Assume kz >> k[CH3), apply the steady-state approximation and work out an expression for (CH3) in term of kį, kz, kz and ke. Show all of your...
9,10,11
9. Consider the decomposition reaction of N2Os. 2 N203(g) → 4NO2(g) + O2(g) follows the first order kinetics with rate constant of 4.8 x 10's. (a) if the initial 165 x 10-2M what is the concentration at 825 s? (b) How long it will take for concentration is 1.65 x 10-2M what is the concentrat the concentration of N2Os to decrease to 1.00 x 10-2M? t 10. Nitrosyl chloride, NOCI, decomposes slowly to NO and Cl2, the reaction follows...
12. The following mechanism is proposed for the decomposition of ozone (O3) to O2: 03 + M 02 + 0 + M 0+03 2 02 Apply the steady-state approximation to the concentration of atomic oxygen, and derive the rate law for the decomposition of ozone (M stands for a molecule that can exchange kinetic energy with particles undergoing the chemical reaction.)
12. The following mechanism is proposed for the decomposition of ozone (O3) to O2: 03 + M 02 +...
Can you explain with all necessary steps and equations? thank
you
6. The reaction 2 H2 + 2 NO N2 + 2 H20 may proceed by the following mechanism: 2 NO - N202 (k, and k.1) H2 + N202 N2O + H2O (kz) H + N20 - N2 + H2O (ku). Use the steady-state approximation to predict the rate law for the formation of the product N.
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