![9. For the following reaction, 2 H2(g) + 2 NO (g) → N2(g) + 2 H20 (g) the rate law is: rate = k[H2][NO]?. At a given temperat](http://img.homeworklib.com/questions/301a2b30-97df-11ea-88af-bbe4183e9f9f.png?x-oss-process=image/resize,w_560)
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![9 Rate lacu Ri = K[Hz] [NO] 0 - Now concentration of hy is quadrupled and the concentration of No Po doubled. 1. So, New Rate](http://img.homeworklib.com/questions/98984f20-a04a-11ea-96e2-074d2d915c72.png?x-oss-process=image/resize,w_560)
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9. For the following reaction, 2 H2(g) + 2 NO...
The reaction 2 NO(g) + 2 H2(g) N2(g) + 2 H2O(g) was studied at a certain...
The reaction 2 NO(g) + 2 H2(g)
N2(g) + 2 H2O(g) was studied at a certain
temperature with the following results:
Experiment
[NO(g)] (M)
[H2(g)] (M)
Rate (M/s)
1
0.0867
0.0867
71.7
2
0.0867
0.173
143
3
0.173
0.0867
285
4
0.173
0.173
570.
(a) What is the rate law for this reaction?
Rate = k [NO(g)] [H2(g)]
Rate = k [NO(g)]2
[H2(g)]
Rate = k [NO(g)] [H2(g)]2
Rate = k [NO(g)]2 [H2(g)]2
Rate = k [NO(g)] [H2(g)]3
Rate =...
2. Consider the reaction below between nitric oxide and hydrogen gas: 2 NO(g) + 2 H2(g)...
2. Consider the reaction below between nitric oxide and hydrogen gas: 2 NO(g) + 2 H2(g) - N2 + 2 H2009) Upon being studied experimentally, it has been determined that the rate law expression for this reaction is first order in Hz and second order in NO(g). With this information in mind, answer the following: [Tip: You can assume that the steady-state approximation is valid for any intermediate here.) a. As written, is the reaction above a valid mechanism? In...
1. For the following reaction N2 (g) + 3 H2(g) — 2 NH3(g) AH° = -92.4...
1. For the following reaction N2 (g) + 3 H2(g) — 2 NH3(g) AH° = -92.4 kJ K = 1.245 x 10-5 at 427°C for each change listed, predict the equilibrium shift and the effect on the indicated quantity. Direction of Shift Gt; or no change) Effect on Quantity Change Effect (increase, decrease, or no change) amount of NH3(g) amount of N2(g) (a) decrease in volume (b) Decrease temperature (c) addition of H2(g) (d) addition of NH3(g) (e) removal of...
Question 7 A catalyst ) 2 NH3 ( g N2 (9) + 3 H2 ( g...
Question 7 A catalyst ) 2 NH3 ( g N2 (9) + 3 H2 ( g The catalyzed decomposition of NH3 (g) at high temperature is represented by the equation above. The rate of disappearance of NH3 (g) was measured over time for two different initial concentrations of NH3 (g) at a constant temperature. The data are plotted in the graph below. Time (s) On the basis of the data in the graph, which of the following best represents the...
only do part (c) **please explain how to solve M^-2 The Haber process is used to...
only do part (c) **please explain how to solve M^-2
The Haber process is used to make ammonia, N2(g) + 3H2(g) = 2NH3(g) a) Write down the condition for equilibrium for this reaction in terms of the concentrations of reactants and products. At 298 K, this reaction has AH° = -46 kJ mol"', and AS° = -100 J K-mol?. Assume that AH° and ASº are independent of temperature. At what temperature does AGº vanish, i.e. AG° = 0? (c) Under...
1) 2) 3) Please explain step by step so I can understand how answer was obtained...
1)
2)
3)
Please explain step by step so I can understand how answer was
obtained
Given the following rate law, how does the rate of reaction change if the concentration of Z is tripled? Rate = k [X] [Y]2[z] The rate of reaction will increase by a factor of 06 OOOO At a certain temperature the equilibrium constant, Kc, equals 0.11 for the reaction: 2 ICI(g) = 12(g) + Cl2(g). What is the equilibrium concentration of Cl2 if 4.27...
1. Consider the reaction: 2 NO (g) + 2 H2 (g) → N2 (g) + 2...
1. Consider the reaction: 2 NO (g) + 2 H2 (g) → N2 (g) + 2 H2O (g). If the rate of change in NO is -0.68 M s^-1 then write the rate of change for the other reactants and products. What is the rate of the reaction? 2. Consider the reaction: CH3COOC2H5 (aq) + OH- (aq) → CH3CO2- (aq) + CH3CH2OH (aq) The reaction is known to be first order in CH3COOC2H5 and first order in OH-. The second-...
1. Consider the reaction below. N2(g) + 3 H2(g) ⇋ 2 NH3(g) Which of the following...
1. Consider the reaction below. N2(g) + 3 H2(g) ⇋ 2 NH3(g) Which of the following changes would cause less NH3 to be produced? decreasing the volume adding N2 increasing the volume adding H2 2. Consider the following reaction. N2(g) + 3 H2(g) ⇋ 2 NH3(g) The forward reaction is exothermic. Which of the following changes would cause less NH3 to be produced? decreasing the temperature adding H2 increasing the temperature adding N2 3. What is the effect of a...
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.
14. The reaction 2 H2(g) + 2 NO(g) ® N2(g) + 2 H2O(g) is proposed to...
14. The reaction 2 H2(g) + 2 NO(g) ® N2(g) + 2 H2O(g) is proposed to have the alternate mechanism: 2 NO(g) ® N2O2(g) FAST N2O2(g) + H2(g) ® N2O(g) + H2O(g) SLOW N2O(g) + H2(g) ® N2(g) + H2O(g) FAST If the rate law is found to be Rate = k[H2][NO]2, could this support the proposed mechanism? Does the rate law indicate that the reaction is termolecular?
The reaction 2 NO(g) + 2 H2(g)
N2(g) + 2 H2O(g) was studied at a certain
temperature with the following results:
Experiment
[NO(g)] (M)
[H2(g)] (M)
Rate (M/s)
1
0.0867
0.0867
71.7
2
0.0867
0.173
143
3
0.173
0.0867
285
4
0.173
0.173
570.
(a) What is the rate law for this reaction?
Rate = k [NO(g)] [H2(g)]
Rate = k [NO(g)]2
[H2(g)]
Rate = k [NO(g)] [H2(g)]2
Rate = k [NO(g)]2 [H2(g)]2
Rate = k [NO(g)] [H2(g)]3
Rate =...
2. Consider the reaction below between nitric oxide and hydrogen gas: 2 NO(g) + 2 H2(g) - N2 + 2 H2009) Upon being studied experimentally, it has been determined that the rate law expression for this reaction is first order in Hz and second order in NO(g). With this information in mind, answer the following: [Tip: You can assume that the steady-state approximation is valid for any intermediate here.) a. As written, is the reaction above a valid mechanism? In...
1. For the following reaction N2 (g) + 3 H2(g) — 2 NH3(g) AH° = -92.4 kJ K = 1.245 x 10-5 at 427°C for each change listed, predict the equilibrium shift and the effect on the indicated quantity. Direction of Shift Gt; or no change) Effect on Quantity Change Effect (increase, decrease, or no change) amount of NH3(g) amount of N2(g) (a) decrease in volume (b) Decrease temperature (c) addition of H2(g) (d) addition of NH3(g) (e) removal of...
Question 7 A catalyst ) 2 NH3 ( g N2 (9) + 3 H2 ( g The catalyzed decomposition of NH3 (g) at high temperature is represented by the equation above. The rate of disappearance of NH3 (g) was measured over time for two different initial concentrations of NH3 (g) at a constant temperature. The data are plotted in the graph below. Time (s) On the basis of the data in the graph, which of the following best represents the...
only do part (c) **please explain how to solve M^-2
The Haber process is used to make ammonia, N2(g) + 3H2(g) = 2NH3(g) a) Write down the condition for equilibrium for this reaction in terms of the concentrations of reactants and products. At 298 K, this reaction has AH° = -46 kJ mol"', and AS° = -100 J K-mol?. Assume that AH° and ASº are independent of temperature. At what temperature does AGº vanish, i.e. AG° = 0? (c) Under...
1)
2)
3)
Please explain step by step so I can understand how answer was
obtained
Given the following rate law, how does the rate of reaction change if the concentration of Z is tripled? Rate = k [X] [Y]2[z] The rate of reaction will increase by a factor of 06 OOOO At a certain temperature the equilibrium constant, Kc, equals 0.11 for the reaction: 2 ICI(g) = 12(g) + Cl2(g). What is the equilibrium concentration of Cl2 if 4.27...
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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