![For the reaction N205 - NO3 + NO2 the observed rate law is rate = k[N205]. If-dN205/dt = 0.20 M / min when [N205] = 0.12 M, w](http://img.homeworklib.com/questions/0374dbc0-f724-11ea-9390-291f6a1227f2.png?x-oss-process=image/resize,w_560)
![What is the correct rate law for the following reaction? CH3Cl(g) + 3Cl2(g) → CCl4(g) + 3HCl(g) rate = k[CH3CI] O a. rate = k](http://img.homeworklib.com/questions/064724f0-f724-11ea-9bc7-dfcc7c28e0a7.png?x-oss-process=image/resize,w_560)
![A given reaction has rate law rate = k[A]2[B]1/2. If the instantaneous rate of reaction is 0.034 m/s when [A] = [B] = 0.40 M,](http://img.homeworklib.com/questions/0a158350-f724-11ea-902b-5752f494dff1.png?x-oss-process=image/resize,w_560)
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The circles below represent the conversion of molecule A (closed circles) to B (open circles). •...
N205 - NO3 + NO2 the observed rate law is rate = k[N205). If-dN205/dt = 0.20...
N205 - NO3 + NO2 the observed rate law is rate = k[N205). If-dN205/dt = 0.20 M/min when [N205) = 0.12 M, what is the value of the rate constant? O a. 0.32 min1 O 6.0.60 min-1 OC. 0.024 min-1 O d. none of these Oe. 1.7 min-1
What happens to the rate of the forward reaction as time passes in the equilibrium region...
What happens to the rate of the forward reaction as time passes in the equilibrium region of the graph below? Concentration Time Ob. the rate decreases a cannot be determined from the graph Ос. the rate both increases and decreases the rate remains constant O d. the rate increases Concentration of reactant A was measured as a function of time, and the data were plotted as shown below. Which of the following statements is true? 850 Chart Area 800 1/[A]...
2. (13 pts) Determine the rate constant and reaction orders for the following reaction using the...
2. (13 pts) Determine the rate constant and reaction orders for the following reaction using the data provided: 2 NO (g) + 02 (g) > 2 NO2 (g) Rate (M/s 0.028 0.057 0.114 0.227 Experiment NO 0.020 0.020 0.020 0.040 0.010 0.010 0.020 0.040 0.020 0.020 3 4 a.) For the rate law, determine all reaction orders Rate -k [NO]m[O2]' Reaction order m (CIRCLE ONE) 1½ Reaction order n (CIRCLE ONE) 1½
please help with these two questions The following data were obtained for the formation of nitrosyl...
please help with these two questions
The following data were obtained for the formation of nitrosyl bromide from nitrogen monoxide and bromine. Initial (NO) Initial (Bra) Initial rate of reaction Trial 1 0.025 M 0.040 M 1.2 m/s Trial 20.025 M 0.080 M 2.4 M/S Trial 3 0.025 M 0.120 M 3.6 M/s Trial 4 0.050 M 0.040 M 4.8 M/s Trial 5 0.075 M 0.040 M 10.8 Mis The rate law for this reaction would be: zero-order in NO...
can you do the 6-12 number 8 is multiple choice 6. The initial rates listed in...
can
you do the 6-12 number 8 is multiple choice
6. The initial rates listed in the table below were determined for the reaction CO(g) + NO2(g) + CO2(g) + NO(g) at varied concentration of the reactants, CO and NO2. Determine the rate law of this reaction. Experiment Initial [CO] (mol/L) Initial [NO] (mol/L) Initial rate (mol/Ls) 5.0x10+ 3.5x10 3.4x10-8 5.0x10+ 7.0x10- 6.8x10-8 1.5x10 3.5x10 1.02x10-7 7. The half-life of the reaction C&H:(8) ► 2CH.g) at constant temperature is independent...
The following data were obtained for the formation of nitrosyl bromide from nitrogen monoxide and bromine....
The following data were obtained for the formation of nitrosyl bromide from nitrogen monoxide and bromine. Initial (NO) Initial (Br2) Initial rate of reaction Trial 1 0.025 M 0.040 M 1.2 m/s Trial 2 0.025 M 0.080 M 2.4 M/s Trial 3 0.025 M 0.120 M 3.6 Mis Trial 40.050 M 0.040 M 4.8 M/s Trial 5 0.075 M 0.040 M 10.8 m/s The rate law for this reaction would be: zero-order in NO half-order in NO first-order in NO...
If molecular oxygen is reacting at a rate of 0.024 M/s in the following reaction; 4...
If molecular oxygen is reacting at a rate of 0.024 M/s in the following reaction; 4 NO2(g) + O2(g) → 2 N205(8) at what rate is N2O5 being formed? O 0.048 M/s 0.096 M/S 0.024 M/s 0.012 M/s The rate law for the reaction 2 NO, +O3 -- N2O5 + O, is rate - k[NO][03]. Which one of the following mechanisms is consistent with this rate law? NO2 + NO2-N202 + O2 (slow) N2O2 +O3-N20s (fast) NO2+O3 -NO3 + O2...
QUESTION 6 From the following data, the reaction order for Ais___and the reaction order for Bis...
QUESTION 6 From the following data, the reaction order for Ais___and the reaction order for Bis A Second order for A: first order for B B. zero order for Azero order for B C. zero order for Afirst order for B D. first order for As first order for B E. None of the answers are correct. QUESTION 7 You are trying to determine the reaction rate for a reaction with several intermediate steps. The rate for the overall reaction...
30) The decomposition of dinitrogen pentoxide is described by the following chemical equation 2 N205(g) -...
30) The decomposition of dinitrogen pentoxide is described by the following chemical equation 2 N205(g) - 4 NO2(g) + O2(g) If the rate of disappearance of N2O5 is equal to 1.80 mol/min at a particular moment, what is the rate of appearance of NO2 at that moment? 31) The decomposition of dinitrogen pentoxide is described by the following chemical equation 2 N205(g) - 4 NO2(g) + O2(g) If the rate of appearance of NO2 is equal to 0.560 mol/min at...
Please answer as many questions as you can Thanks 1. For the reaction, N2(g) 3H2(g)2NH3(g). if...
Please answer as many questions as you can
Thanks
1. For the reaction, N2(g) 3H2(g)2NH3(g). if the rate of formation of ammonia is 0.04 mol/L min, find the rate of disappearance of H2 and N2 during that same time period. 2. For the following reaction, 5Br BrO3 6H3Br2 3H20, the rate of consumption of bromide ion at some time was found to be 0.20 mo/L s. What is the rate of formation of water over the same time period? 3....
N205 - NO3 + NO2 the observed rate law is rate = k[N205). If-dN205/dt = 0.20 M/min when [N205) = 0.12 M, what is the value of the rate constant? O a. 0.32 min1 O 6.0.60 min-1 OC. 0.024 min-1 O d. none of these Oe. 1.7 min-1
What happens to the rate of the forward reaction as time passes in the equilibrium region of the graph below? Concentration Time Ob. the rate decreases a cannot be determined from the graph Ос. the rate both increases and decreases the rate remains constant O d. the rate increases Concentration of reactant A was measured as a function of time, and the data were plotted as shown below. Which of the following statements is true? 850 Chart Area 800 1/[A]...
2. (13 pts) Determine the rate constant and reaction orders for the following reaction using the data provided: 2 NO (g) + 02 (g) > 2 NO2 (g) Rate (M/s 0.028 0.057 0.114 0.227 Experiment NO 0.020 0.020 0.020 0.040 0.010 0.010 0.020 0.040 0.020 0.020 3 4 a.) For the rate law, determine all reaction orders Rate -k [NO]m[O2]' Reaction order m (CIRCLE ONE) 1½ Reaction order n (CIRCLE ONE) 1½
please help with these two questions
The following data were obtained for the formation of nitrosyl bromide from nitrogen monoxide and bromine. Initial (NO) Initial (Bra) Initial rate of reaction Trial 1 0.025 M 0.040 M 1.2 m/s Trial 20.025 M 0.080 M 2.4 M/S Trial 3 0.025 M 0.120 M 3.6 M/s Trial 4 0.050 M 0.040 M 4.8 M/s Trial 5 0.075 M 0.040 M 10.8 Mis The rate law for this reaction would be: zero-order in NO...
can
you do the 6-12 number 8 is multiple choice
6. The initial rates listed in the table below were determined for the reaction CO(g) + NO2(g) + CO2(g) + NO(g) at varied concentration of the reactants, CO and NO2. Determine the rate law of this reaction. Experiment Initial [CO] (mol/L) Initial [NO] (mol/L) Initial rate (mol/Ls) 5.0x10+ 3.5x10 3.4x10-8 5.0x10+ 7.0x10- 6.8x10-8 1.5x10 3.5x10 1.02x10-7 7. The half-life of the reaction C&H:(8) ► 2CH.g) at constant temperature is independent...
The following data were obtained for the formation of nitrosyl bromide from nitrogen monoxide and bromine. Initial (NO) Initial (Br2) Initial rate of reaction Trial 1 0.025 M 0.040 M 1.2 m/s Trial 2 0.025 M 0.080 M 2.4 M/s Trial 3 0.025 M 0.120 M 3.6 Mis Trial 40.050 M 0.040 M 4.8 M/s Trial 5 0.075 M 0.040 M 10.8 m/s The rate law for this reaction would be: zero-order in NO half-order in NO first-order in NO...
If molecular oxygen is reacting at a rate of 0.024 M/s in the following reaction; 4 NO2(g) + O2(g) → 2 N205(8) at what rate is N2O5 being formed? O 0.048 M/s 0.096 M/S 0.024 M/s 0.012 M/s The rate law for the reaction 2 NO, +O3 -- N2O5 + O, is rate - k[NO][03]. Which one of the following mechanisms is consistent with this rate law? NO2 + NO2-N202 + O2 (slow) N2O2 +O3-N20s (fast) NO2+O3 -NO3 + O2...
QUESTION 6 From the following data, the reaction order for Ais___and the reaction order for Bis A Second order for A: first order for B B. zero order for Azero order for B C. zero order for Afirst order for B D. first order for As first order for B E. None of the answers are correct. QUESTION 7 You are trying to determine the reaction rate for a reaction with several intermediate steps. The rate for the overall reaction...
30) The decomposition of dinitrogen pentoxide is described by the following chemical equation 2 N205(g) - 4 NO2(g) + O2(g) If the rate of disappearance of N2O5 is equal to 1.80 mol/min at a particular moment, what is the rate of appearance of NO2 at that moment? 31) The decomposition of dinitrogen pentoxide is described by the following chemical equation 2 N205(g) - 4 NO2(g) + O2(g) If the rate of appearance of NO2 is equal to 0.560 mol/min at...
Please answer as many questions as you can
Thanks
1. For the reaction, N2(g) 3H2(g)2NH3(g). if the rate of formation of ammonia is 0.04 mol/L min, find the rate of disappearance of H2 and N2 during that same time period. 2. For the following reaction, 5Br BrO3 6H3Br2 3H20, the rate of consumption of bromide ion at some time was found to be 0.20 mo/L s. What is the rate of formation of water over the same time period? 3....
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