The following data were obtained from a study of the decomposition of CHEM at 320 °C: t, second S 0.00 200 400 Concentration of CHEM, mole/L 1.16 0.86 0.65 Plot the data using the first- and second-order equations. A. What is the correlation coefficient (r) for each plot? A1. r for first-order? choose your answer... A2. r for second-order? choose your answer... B. What is the order for this reaction? choose your answer... C. What is the rate constant? choose your answer... D. What is the CHEM concentration (in mol/L) at 300 s? choose your answer... V V

The first-order degradation of a drug was monitored under three different conditions (I, ii, and iii), which resulted in half-lives (in no particular order) of 4 hours, 8 hours, and 10 hours: а. i. at 37 °C. ii. at 37 °C, in the presence of a catalyst. iii. at 21 °C. Identify which half life goes with which set of conditions. For condition i., draw and label a graph of Concentration (mmol/L) vs Time (hr). Start with an initial concentration of 10 mmol/L and show the decay over 40 hours. You may use the grid below or draw your graph by hand. 10 9.5 8.5 7.5 2 6.5 E 5.5 4.5 4 3.5 2.5 1.5 0.5 4 8 10 12 14 16 18 20 22 24 26 28 30 32 34 36 38 40 Time (hours) -1 Another reaction is found to have an activation energy of 80.3 kJmol. The reaction is very slow at 25°c. Which will be the more effective way of speeding up the reaction, b. -1 i. adding a catalyst which lowers the activation energy to 30.0 kJ mol or ii. raising the temperature from 25°C to 50°C ? Show all calculations and explain…

For a gas-phase reaction 2NO(g) +H2(g) N2O(g) +H2O(g), the rate law can be expressed dp (N₂O) as dt kpop₂ The data in table have been obtained Run p°(NO)/kPa p°(H₂)/kPa Half-time/s T/K 1 80.0 1.33 19.2 1093 2 80.0 2.66 19.2 1093 3 1.33 80.0 830 1093 4 2.66 80.0 415 1093 5 80.0 1.33 10 1113 (The runs are at constant temperature and volume) (a) Determine the order of the reaction (a and b) with explanation. (b) Estimate k at 1093 K.

... cvg.cengagenow.com The gas phase decomposition of sulfuryl chloride at 600 K SO₂Cl₂(g) SO₂(g) + Cl₂(g) is first order in SO₂Cl₂. 0.000657 M after 503.0 min had passed. + OWLV2 | Online teaching and learning resource from Cengage Learning During one experiment it was found that when the initial concentration of SO₂Cl₂ was 0.00494 M, the concentration of SO₂Cl₂ dropped to Based on this experiment, the rate constant for the reaction is min-¹. 99% 00 00

0.554 Absorbance (Initial Absorbance) reading s 10 secondr Absorbance →6.148 20 seconds - 30 seconds → 0094 40 seconds 0,073 S0 Seconds > 0,058 60 seconde -

A certain first-order reaction is 62% complete in 55 s. What are the values of the rate constant and the half-life for this process? a. k = -1 S b. t₁/2 = Submit Answer S Try Another Version 1 item attempt remaining

4.2 * 10 - 4s - 1 . What is the half- life 4. The rate constantk for a first-order reaction is equal to for the reaction?