![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](http://img.homeworklib.com/questions/bf010700-4c28-11eb-89e5-f9bb232fac2a.png?x-oss-process=image/resize,w_560)
Homework Answers
a)
see experiment 2 and 4:
[NO] doubles
[O2] is constant
rate becomes 4 times
so, order of NO is 2
Answer: m = 2
b)
see experiment 1 and 2:
[NO] is constant
[O2] doubles
rate doubles
so, order of O2 is 1
Answer: n = 1
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2. (13 pts) Determine the rate constant and reaction orders for the following reaction using the...
The rate of reaction of nitrogen monoxide with oxygen was measured at 25 degree C starting...
The rate of reaction of nitrogen monoxide with oxygen was measured at 25 degree C starting with various initial concentrations of NO and O2. 2 NO(g) + O2(g) --> 2 NO2(g) The data collected is summarized in the following table: Trail n Initial concentration mol / L Initial reaction rate mol/l.s 1 0.020 0.010 0.028 2 0.020 0.020 0.057 3 0.040 0.020 0.227 a. Use the method of initial rates to find the reaction orders with respect to NO and...
From the data, determine the rate constant (k) for the reaction. Express your answer using two...
From the data, determine the
rate constant (k) for the reaction. Express your answer using two
significant figures.
<Chapter 14 Homework For Practice 14.2 - Enhanced - with Feedback 10 of 48 Review I Constants Periodic Table Consider the following reaction: CHCl (g)Cl(g) -CCl (g) +HCl(g) Submit Previous Answers The initial rate of the reaction is measured at several different concentrations of the reactants with the Correct following results Fractional-order reactions are not comman but are occasionally observed. The first...
Part A From the data, determine the rate law for the reaction. You may want to...
Part A From the data, determine the rate law for the reaction. You may want to reference (Pages 629 - 634) Section 14.3 while completing this problem. Consider the following reaction: CHCl(9) + Cl2(g) → CCL (9) + HC1() The Initial rate of the reaction is measured at several different concentrations of the reactants with the following results: [CHCI](M) [CI] (M) initial Rate (M/s) 0.010 0.010 0.0034 0.020 0.010 0.0068 rate=K[CHC13]/2Cl2}\/2 O rate-k[CHCI)(CI)" Oratenk(CHCI)(C1) O rate=k[CHC13) C1,]1/2 0.020 0.040 0.020...
Nitrogen monoxide (NO) reacts with oxygen (O2) to form nitrogen dioxide (NO2): NO(g) + O2(g) →...
Nitrogen monoxide (NO) reacts with oxygen (O2) to form nitrogen dioxide (NO2): NO(g) + O2(g) → NO2(g) Initial rates for the reaction of nitrogen monoxide (NO) and oxygen (02) were measured at 25°C starting with various concentrations of NO and O2. The following data were collected: Exp. [NO]. (A) [02]. (A) d[NO]/dt (M/s) 0.020 0.010 -0.056 0.020 0.020 -0.112 3 0 .020 0.040 -0.224 0.040 0.020 -0.448 5 0.010 0.020 -0.028 4 What is the numerical value of the rate...
GIVEN THE FOLLOWING DATA FOR THIS REACTION: NH4+(aq) + NO2-(aq) ---> N2(g) + 2H2O(l) EXPT NH4+...
GIVEN THE FOLLOWING DATA FOR THIS REACTION: NH4+(aq) + NO2-(aq) ---> N2(g) + 2H2O(l) EXPT NH4+ NO2- RATE 1 0.010 M 0.020 M 0.020 M/s 2 0.015 M 0.020 M 0.030 M/s 3 0.010 M 0.010 M 0.005 M/s a. Calculate the order of reaction with respect to NH4+ b. Calculate the order of reaction with respect to NO2- c. Calculate the rate constant k d. Determine the overall order of reaction e. Determine the rate law
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...
Consider the reaction: 2 NO(g) + O2 (g)--> 2 NO2 (g) The following data were obtained...
Consider the reaction: 2 NO(g) + O2 (g)--> 2 NO2 (g)
The following data were obtained from three experiments using
the method of initial rates:
3. Consider the reaction: 2 NO(g) + O2(g) → 2 NO2(g) The following data were obtained from three experiments using the method of initial rates: Initial [NO] Initial rate NO Initial [02] mol mol L-1 mol L-1 L-15-1 0.010 0.010 Experiment 1 Experiment 2 Experiment 3 0.020 0.010 2.5 x 10-5 1.0 x 10-4 5.0...
4 of 15 Determine the overall reaction order for the reaction, A C+D using the table...
4 of 15 Determine the overall reaction order for the reaction, A C+D using the table of data below: Experiment Initial [A]/M Initial [B]/M Initial rate/M s. 1 1 2 0.010 0.020 0.040 0.075 0.050 0.025 0.0017 0.0015 0.0016 O O WN - o O O 5 of 15 Which of the following would have the greatest effect on the value of the rate law constant in the rate law equation, rate=k[A]? O increasing the concentration of the reactant O...
SECTION B (Open ended) 1. Given the following data for this reaction: NH" (B) + NO2 aa = N2 + 2H2O) EXPT INHE...
SECTION B (Open ended) 1. Given the following data for this reaction: NH" (B) + NO2 aa = N2 + 2H2O) EXPT INHE'] [NO:') RATE 0.010 M 0.015 M 0.010 M 0.020 M 0.020 M 0.010 M 0.020 M/s 0.030 M/s 0.005 M/s (a) Calculate the order of reaction with respect to NH. (4 points) (b) Calculate the order of reaction with respect to NO3' (4 points) (c) Calculate the rate constant k (4 points) (d) Determine the overall order...
12 of 15 Use the table below to calculate the initial reaction rate of the following...
12 of 15 Use the table below to calculate the initial reaction rate of the following reaction: 2AB+C [A]/M t/s 0.100 0.045 O 0.006 M/S -0.006 M/S -0.012 M/s 0.012 M/s 13 of 15 Use the table below to determine the rate law for the reaction A-2B: Initial rate/Ms Experiment Initial [A]/M 1 0.010 0.020 0.040 0.0010 0.0040 0.0160 2 3 1 rate=k O rate=k[A] O rate=k[A]2 O rate=k[A][B]2
The rate of reaction of nitrogen monoxide with oxygen was measured at 25 degree C starting with various initial concentrations of NO and O2. 2 NO(g) + O2(g) --> 2 NO2(g) The data collected is summarized in the following table: Trail n Initial concentration mol / L Initial reaction rate mol/l.s 1 0.020 0.010 0.028 2 0.020 0.020 0.057 3 0.040 0.020 0.227 a. Use the method of initial rates to find the reaction orders with respect to NO and...
From the data, determine the
rate constant (k) for the reaction. Express your answer using two
significant figures.
<Chapter 14 Homework For Practice 14.2 - Enhanced - with Feedback 10 of 48 Review I Constants Periodic Table Consider the following reaction: CHCl (g)Cl(g) -CCl (g) +HCl(g) Submit Previous Answers The initial rate of the reaction is measured at several different concentrations of the reactants with the Correct following results Fractional-order reactions are not comman but are occasionally observed. The first...
Part A From the data, determine the rate law for the reaction. You may want to reference (Pages 629 - 634) Section 14.3 while completing this problem. Consider the following reaction: CHCl(9) + Cl2(g) → CCL (9) + HC1() The Initial rate of the reaction is measured at several different concentrations of the reactants with the following results: [CHCI](M) [CI] (M) initial Rate (M/s) 0.010 0.010 0.0034 0.020 0.010 0.0068 rate=K[CHC13]/2Cl2}\/2 O rate-k[CHCI)(CI)" Oratenk(CHCI)(C1) O rate=k[CHC13) C1,]1/2 0.020 0.040 0.020...
Nitrogen monoxide (NO) reacts with oxygen (O2) to form nitrogen dioxide (NO2): NO(g) + O2(g) → NO2(g) Initial rates for the reaction of nitrogen monoxide (NO) and oxygen (02) were measured at 25°C starting with various concentrations of NO and O2. The following data were collected: Exp. [NO]. (A) [02]. (A) d[NO]/dt (M/s) 0.020 0.010 -0.056 0.020 0.020 -0.112 3 0 .020 0.040 -0.224 0.040 0.020 -0.448 5 0.010 0.020 -0.028 4 What is the numerical value of the rate...
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...
Consider the reaction: 2 NO(g) + O2 (g)--> 2 NO2 (g)
The following data were obtained from three experiments using
the method of initial rates:
3. Consider the reaction: 2 NO(g) + O2(g) → 2 NO2(g) The following data were obtained from three experiments using the method of initial rates: Initial [NO] Initial rate NO Initial [02] mol mol L-1 mol L-1 L-15-1 0.010 0.010 Experiment 1 Experiment 2 Experiment 3 0.020 0.010 2.5 x 10-5 1.0 x 10-4 5.0...
4 of 15 Determine the overall reaction order for the reaction, A C+D using the table of data below: Experiment Initial [A]/M Initial [B]/M Initial rate/M s. 1 1 2 0.010 0.020 0.040 0.075 0.050 0.025 0.0017 0.0015 0.0016 O O WN - o O O 5 of 15 Which of the following would have the greatest effect on the value of the rate law constant in the rate law equation, rate=k[A]? O increasing the concentration of the reactant O...
SECTION B (Open ended) 1. Given the following data for this reaction: NH" (B) + NO2 aa = N2 + 2H2O) EXPT INHE'] [NO:') RATE 0.010 M 0.015 M 0.010 M 0.020 M 0.020 M 0.010 M 0.020 M/s 0.030 M/s 0.005 M/s (a) Calculate the order of reaction with respect to NH. (4 points) (b) Calculate the order of reaction with respect to NO3' (4 points) (c) Calculate the rate constant k (4 points) (d) Determine the overall order...
12 of 15 Use the table below to calculate the initial reaction rate of the following reaction: 2AB+C [A]/M t/s 0.100 0.045 O 0.006 M/S -0.006 M/S -0.012 M/s 0.012 M/s 13 of 15 Use the table below to determine the rate law for the reaction A-2B: Initial rate/Ms Experiment Initial [A]/M 1 0.010 0.020 0.040 0.0010 0.0040 0.0160 2 3 1 rate=k O rate=k[A] O rate=k[A]2 O rate=k[A][B]2
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