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Calculate the average rate over the interval 0 to 5.0 h. Compare your result with the average rates over the intervals 1.0 to 4.0 h and 2.0 to 3.0 h, all of which have the same midpoint (2.5 h from the start).
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- The decomposition of aqueous sucrose to form the isomers glucose and fructose is a common organic reaction, which requires a strong catalyst: C12H22O11(aq) + H2O(l) → 2C6H12O6(aq). The following data were collected during the process: Time (min) [C12H22O11] (mol/L) 0 0.316 39 0.274 80 0.238 140 0.190 210 0.146 Use the following grids to plot three separate graphs of [C12H22O11], ln[C12H22O11], and 1/[C12H22O11] against time to determine the reaction order. (a)Write the rate law expression in its general form (water should not be included). (b)Determine the rate constant with units. (c)Determine the half-life. (d)If we performed a new trial with an initial concentration of sucrose of 0.400 mol/L, what concentration would remain after 4.0 h has passed?Time(s) [X3] (mole/L) 0 0.600 200 0.458 400 0.362 600 0.281 800 0.204 1000 0.175 1200 0.134 1400 0.104 1600 0.083 1800 0.063 2000 0.047 plot ln[X3] vs time plot 1/[X3] vs timeUse this data to determine the value of the rate constant. Ex # [A] (M) [B] (M) Rate (M/hr) 1 .240 .120 2.00 2 .120 .120 .500 3 .240 .0600 1.00 Question 4 options: 289 per hour 579 per hour 8.3 per hour 0.0144 per hour 69.4 per hour .00346 per hour 0.060 per hour 0.0173 per hour 17 per hour 0.12 per hour
- Please answer questions 4a, 4b, and 4c. The questions are provided in the attached image. Thank you.Determine the average rate of change of BB from ?=0 s�=0 s to ?=392 s.�=392 s. A⟶2BA⟶2B Time (s) Concentration of A (M) 0 0.7300.730 196196 0.4450.445 392392 0.160For the fictitious reaction: AB → A + B Some data was collected measuring the [AB] at certain time intervals. This data was then graphed as described below. A graph of 1/[AB] versus time (s) gives a straight line with the equation: y = 0.0052x + 0.1135 and a R2 = 0.9995. A graph of ln[AB] versus time (s) gives a straight line with the equation: y = -0.0068x + 1.725 and a R2 = 0.8925. Assume the data doesn't fit a zero order reaction. The rate law is: Rate = k[AB]2 Find: What is the value of the rate constant for the given reaction? Select one: a. k = 0.0157 Ms-1 b. k = 0.0052 M-1s-1 c. k = 0.0068 s-1 d. There is no way to determine the value of the rate constant from the given information.
- In aqueous solution, chlorine dioxide oxidizes iodide ion to iodine and chlorine dioxide is reduced to chlorite ion. 2ClO2 (aq) + 2 I- (aq) ----> 2ClO2- (aq) + I2 (aq) The concentration in molarity, of ClO2 was measured at various time points. The data was plotted and the plot of [1/[ClO2] versus time in seconds was most linear. The linear regression equation for the plot is y= 7.60x10-2 (t) + 2.353. What is the concentration of ClO2 at 2.00 minutes if the initial concentration of ClO4 ia 0.425 M? a.) 0.0872 M b.) 2.50 M c.) 11.5 M d.) 0.399 MA group of students compiled the data shown in data table 1 below. What is the exact calculated order for IO3-(aq) to 2 decimal places? Exp. # [IO3-]0 (M) [I-]0 (M) [H+]0 (M) Time (s) 1 0.005 0.05 2 x 10-5 22.12 2 0.010 0.05 2 x 10-5 86.84 3 0.005 0.10 2 x 10-5 5.35 4 0.005 0.05 4 x 10-5 2.65 Question 4 options: 2.44 -2.49 1.81 2.09 -1.72 -2.13 -2.36 1.49 2.24 -1.97 -1.53 1.65Can I get detailed explanation for this table , mentioning the apparatus and when’s the timer is started ? What happens next
- Determine the average rate of change of BB from ?=0 st=0 s to ?=272 s.t=272 s. A⟶2BA⟶2B Time (s) Concentration of A (M) 0 0.7300.730 136136 0.4450.445 272272 0.1600.160 rateB= __________M/sUse the information given here to answer both questions (4 and 5). For the fictitious reaction: AB → A + B Some data was collected measuring the [AB] at certain time intervals. This data was then graphed as described below. A graph of 1/[AB] versus time (s) gives a straight line with the equation: y = 0.0052x + 0.1135 and a R2 = 0.9995. A graph of ln[AB] versus time (s) gives a straight line with the equation: y = -0.0068x + 1.725 and a R2 = 0.8925. Assume the data doesn't fit a zero order reaction. What is the rate law for this reaction? Select one: a. Rate = k[AB]2 b. Rate = k[A][B] c. Rate = k[AB] d. Rate = k Using the data from the previous question. What is the value of the rate constant for the given reaction? Select one: a. k = 0.0052 M-1s-1 b. k = 0.0157 Ms-1 c. k = 0.0068 s-1 d. There is no way to determine the value of the rate constant from the given information.Time (min) Concentration of Phenyl Acetate (M) 0 0.55 0.25 0.42 0.50 0.31 0.75 0.23 1.00 0.17 1.25 0.12 1.50 0.082 what is the difference between concentration vs. time, 1/concentration vs. time, and ln concentration vs. time in terms of graphing?