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what will be the molar concentration of each ion in the electrolyte solutions once the reaction...
EXPERIMENT 3. Kinetic Study: The lodine Clock Reaction Prelaboratory Questions Name Fiza Chandning Laboratory Section 0000000000000000000000000000000000000000000000000000000000000000000000000000000...
EXPERIMENT 3. Kinetic Study: The lodine Clock Reaction Prelaboratory Questions Name Fiza Chandning Laboratory Section 0000000000000000000000000000000000000000000000000000000000000000000000000000000 1. Consider the following reaction: 2 NO(g) + 4 NO, (g) + O2(g) The initial concentration of N, O, was 0.84 mol/L, and 35 minutes after initiating the reaction, all of the N,Os has been consumed. a) Calculate the average rate of the reaction over this 35-minute time interval. b) Is it correct to assume that the rate law is Rate = k[NO]? based...
what is the equlibrium concentration of S^2 Consider the reaction for the decomposition of hydrogen disulfide:...
what is the equlibrium concentration of S^2
Consider the reaction for the decomposition of hydrogen disulfide: 2H2S(g) = 2H2(g) + S2(g), K. = 1.67 x 10-7 at 800°C The reaction is carried out at the same temperature with the following initial concentrations: H2S] = 2.50 x 10-4M [H2] = 0.00 M [S2] = 0.00 M
For questions 1-10 you will consider the following chemical reaction - the catalyzed decomposition of amino...
For questions 1-10 you will consider the following chemical reaction - the catalyzed decomposition of amino acid (B) - for which you know the overall chemical reaction, but the mechanism is unknown. Overall chemical reaction: 2B(aq) → B'(aq) + H20(1) You also have access to the following experimentally obtained kinetics data for the reaction at 290 K and 300K. Concentration (M) of B vs. Time (day) Time @ 290K @300K 0 0.90 0.75 1 0.80 0.60 2 0.70 0.45 3...
Dr. Raphael Shell created a concentration vs time graph for the following chemical reaction
Dr. Raphael Shell created a concentration vs time graph for the following chemical reaction: 2 AB2 〓 4 B + 2 A. He observed that it took one hour to complete the first half-life, 30 min to complete its second half-life and 15 minutes to complete the third half-life. Also, doubling or tripling the concentration of the reactant shows no effect on the rate of reaction.a) Determine the (general or incomplete) RATE LAW for this reaction based on the information provided above. b) Using...
In a study of the decomposition of nitrosyl bromide at 10 °C NOBr—+NO+ Br2 the concentration...
In a study of the decomposition of nitrosyl bromide at 10 °C NOBr—+NO+ Br2 the concentration of NOBr was followed as a function of time. It was found that a graph of 1/[NOBr] versus time in seconds gave a straight line with a slope of 1.27 m?s and a y-intercept of 3.98 M? Based on this plot, the reaction is order in NOBr and the rate constant for the reaction is M?? In a study of the decomposition of hydrogen...
2. Answer the following questions by connecting the half-life of each first-order reaction to the rate...
2. Answer the following questions by connecting the half-life of each first-order reaction to the rate constant. a. The rate constant of a first-order reaction is 2.43 × 10–2 min–1. What is the half-life of the reaction? (2 points) b. A first-order reaction has a rate constant of 0.547 min-1. How long will it take a reactant concentration 0.14 M to decrease to 0.07 M? (2 points) c. The half-life of a first-order reaction is 5.47 min. What is the...
Shown below is a concentration vs. time plot for the reaction 2A ⇌ B. What is...
Shown below is a concentration
vs. time plot for the reaction 2A ⇌ B. What is the value for the
equilibrium constant for this reaction?
0.100 0.080 0.060 B 0.040 Concentration (M) A 0.020 0.000 0.00 1.00 2.00 3.00 4.00 5.00 Time (min)
Lab 1l: Kinetics In the Kinetics Lab, the reaction of iodide with persulfate was studied, and it ...
Lab 1l: Kinetics In the Kinetics Lab, the reaction of iodide with persulfate was studied, and it was determined that the rate law was first order in each reactant. 21(a)s20 (22 S042(ag) rateS2091 (a) If [I-] = 0.0550 M, [S2O82-]-0.0350 M, and kー0.00400 M-1 s-1, what is the reaction rate? M/s (b) If [I-]-0.0500 M, [S2082-]-0.0350 M, and the reaction rate is 5.90×10-6 M/s, what is the rate constant? M-1s-1 (c) The reaction rate was determined indirectly in this lab...
You will need to generate a set of graphs to answer this question. Concentration vs time...
You will need to generate a set of graphs to answer this question. Concentration vs time data for the following decomposition reaction was collected at 300 K. The data is shown in the table below. What is the rate constant for the reaction at this temperature (in units of min-1)? H2O2(aq) → H2O(l) + 1/2 O2(g) time (min) [H2O2](mol/L) 0 0.00191 500 0.00082 1000 0.00035 1500 0.00015 2000 0.00006
(e) In the reaction: H202(a) +3 (a)+ 2 H(a)Is (a)+ 2 H2O( (aq) (aq)13 3 (aq) the concentration of I- decreases from 0.1...
(e) In the reaction: H202(a) +3 (a)+ 2 H(a)Is (a)+ 2 H2O( (aq) (aq)13 3 (aq) the concentration of I- decreases from 0.173 to 0.146 mol dm-3 in 1 min. What is the rate of the reaction over this time interval? [2 marks (f) The activation energy for the formation of ethane from cyclobutane is 260 kJ mol1. If the rate constant at 300°C is 7.9 x 10 9 s-1, what is the pre-exponential factor A for this reaction? 12...
EXPERIMENT 3. Kinetic Study: The lodine Clock Reaction Prelaboratory Questions Name Fiza Chandning Laboratory Section 0000000000000000000000000000000000000000000000000000000000000000000000000000000 1. Consider the following reaction: 2 NO(g) + 4 NO, (g) + O2(g) The initial concentration of N, O, was 0.84 mol/L, and 35 minutes after initiating the reaction, all of the N,Os has been consumed. a) Calculate the average rate of the reaction over this 35-minute time interval. b) Is it correct to assume that the rate law is Rate = k[NO]? based...
what is the equlibrium concentration of S^2
Consider the reaction for the decomposition of hydrogen disulfide: 2H2S(g) = 2H2(g) + S2(g), K. = 1.67 x 10-7 at 800°C The reaction is carried out at the same temperature with the following initial concentrations: H2S] = 2.50 x 10-4M [H2] = 0.00 M [S2] = 0.00 M
For questions 1-10 you will consider the following chemical reaction - the catalyzed decomposition of amino acid (B) - for which you know the overall chemical reaction, but the mechanism is unknown. Overall chemical reaction: 2B(aq) → B'(aq) + H20(1) You also have access to the following experimentally obtained kinetics data for the reaction at 290 K and 300K. Concentration (M) of B vs. Time (day) Time @ 290K @300K 0 0.90 0.75 1 0.80 0.60 2 0.70 0.45 3...
In a study of the decomposition of nitrosyl bromide at 10 °C NOBr—+NO+ Br2 the concentration of NOBr was followed as a function of time. It was found that a graph of 1/[NOBr] versus time in seconds gave a straight line with a slope of 1.27 m?s and a y-intercept of 3.98 M? Based on this plot, the reaction is order in NOBr and the rate constant for the reaction is M?? In a study of the decomposition of hydrogen...
Shown below is a concentration
vs. time plot for the reaction 2A ⇌ B. What is the value for the
equilibrium constant for this reaction?
0.100 0.080 0.060 B 0.040 Concentration (M) A 0.020 0.000 0.00 1.00 2.00 3.00 4.00 5.00 Time (min)
Lab 1l: Kinetics In the Kinetics Lab, the reaction of iodide with persulfate was studied, and it was determined that the rate law was first order in each reactant. 21(a)s20 (22 S042(ag) rateS2091 (a) If [I-] = 0.0550 M, [S2O82-]-0.0350 M, and kー0.00400 M-1 s-1, what is the reaction rate? M/s (b) If [I-]-0.0500 M, [S2082-]-0.0350 M, and the reaction rate is 5.90×10-6 M/s, what is the rate constant? M-1s-1 (c) The reaction rate was determined indirectly in this lab...
(e) In the reaction: H202(a) +3 (a)+ 2 H(a)Is (a)+ 2 H2O( (aq) (aq)13 3 (aq) the concentration of I- decreases from 0.173 to 0.146 mol dm-3 in 1 min. What is the rate of the reaction over this time interval? [2 marks (f) The activation energy for the formation of ethane from cyclobutane is 260 kJ mol1. If the rate constant at 300°C is 7.9 x 10 9 s-1, what is the pre-exponential factor A for this reaction? 12...
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