Determine the order of the reaction with respect to NOBr (g).
| Time (s) | [NOBr] (M) | ln [NOBr] | 1 / [NOBr] (M-1) |
| 0 | 0.01 | -4.60 | 100.000 |
| 2 | 0.0071 | -4.95 | 140.845 |
| 4 | 0.0055 | -5.20 | 181.818 |
| 6 | 0.0045 | -5.40 | 222.222 |
| 8 | 0.0038 | -5.57 | 263.158 |
| 10 | 0.0033 | -5.71 | 303.030 |
Determine the order of the reaction with respect to NOBr (g). Time (s) [NOBr] (M) ln...
Given the data below for the decomposition of NOBr (g) to NO (g) and Br2 (g), determine the order of the reaction with respect to NOBr (g). To do this, create a graph of the data for each of the orders of reaction and report the R2 value for each linear fit. The graph with the R2 value closest to 1 is the most linear graph and the equation graphed corresponds to the order of the reaction. *I do not...
The decomposition of NOBr is studied manometrically because the number of moles of gas changes; it cannot be studied colorimetrically because both NOBr and Br2are reddish-brown. 2NOBr(g) ? 2NO(g) + Br2(g) Use the data below to make the following determinations: (a) the average rate of decomposition of NOBr over the entire experiment. (b) the average rate of decomposition of NOBr between 2.00 and 4.00 seconds. Time (s) [NOBr] (mol/L) 0.00 0.0100 2.00 0.0071 4.00 0.0055 6.00 0.0045 8.00 0.0038 10.00...
Determine the order of the reactant. aA bB Time [A] (s) 0 0.0100 4 0.0071 0.0055 8 12 0.0045 16 0.0038
Determine the first half-life of the reaction. Determine the second and third half-lives. aA - bВ Time [A] (S) 0 0.0100 0.0071 8 0.0055 112 0.0045 16 0.0038
8. Nitrosyl bromide (NOBr) decomposes to nitrogen oxide and bromine. Use the following data to determine the order of the decomposition reaction. time 6 12 18 24 INOBr] 0.0286 0.0253 0.0229 0.0208 0.0190 Ln NOB] -3.554 1 -3.677 -3.777 -3.873 -3.963 1/[NOBr] 35.0 39.5 43.7 48.1 52.6
The rate constant for the second-order reaction: 2NOBr(g) → 2NO(g) + Br2(g) is 0.80/(M · s) at 10°C. Starting with a concentration of 0.86 M, calculate the concentration of NOBr after 89 s. M
The rate constant for the second-order reaction: 2NOBr(g) → 2NO(g) + Br2(g) is 0.80/(M · s) at 10°C. Starting with a concentration of 0.86 M, calculate the concentration of NOBr after 59 s.
28. For the reaction 2 SO2(g) + O2(g) → 2 S03(), a. Determine the expression for the rate of the reaction with respect to each of the reactants and products. b. When SO3 is increasing at a rate of 0.0071 M/s, how fast is 02 decreasing? How fast is SO2 A decreasing?
Consider this initial-rate data at a certain temperature for the reaction described by [SO, Cl, 1, (M) Initial rate (M/s) SO,Cl2(g) → SO2(g) + Cl2(g) 1.80 x 10-6 Determine the order with respect to SOC12. 0.100 0.200 0.300 3.60 x 10-6 5.40 x 10-6 order: Determine the value and units of the rate constant. units: Initial rate data at a certain temperature is given in the table for the following reaction. 2 NOBr(g) —> 2 NO(g) + Br2(g) [NOBr), (M)...
2NO (g) +Cl2 (g) → NOCl (g) Experiment concentration of NO (M) concentration of Cl2(M) Rate (M/s) 1 0.05 0.01 3.40 x 10-4 2 0.025 0.01 8.50 x 10-5 3 0.025 0.04 3.40 x 10-4 What is the reaction order with respect to NO ? the reaction order with respect to reaction order to Cl2 ? overall reaction order ? what is the rate constant ?