Consider the following experimental rate data for a general reaction A + B --> C Derive the rate law. [A] M [B] M Rate M/s 0.1 0.1 0.23 0.2 0.05 0.46 0.2 0.1 0.92

Consider the reaction  I- + OCl- → OH-→ IO- + Cl- Determine the reaction's rate law using the given experimental data. Exp # [I-]o [OCl-]o [OH-]o Initial Rate  (M/s) 1 0.0013 0.012 0.10 0.094 2 0.0026 0.012 0.10 0.187 3 0.0013 0.006 0.10 0.047 4 0.0013 0.012 0.20 0.047

Ⓒ Macmillan Learning Enter these data into the graphing tool and determine the value and units of the rate constant, k, for this reaction. Graphing Tool Add Row 10 total rows [A] [A] vs. t In[A] In[A] vs. t t (min) 0.0 2.0 4.0 6.0 1/[A] vs. t [A] (M) 1.00 0.66 0.43 0.28 1/[A] Clear All Data

Consider the following fictitious reaction and the measured initial rates at different reaction conditions. Determine the rate law for this reaction. X (g) + y (g) XY (g) Trial 1 2 3 Initial Rate (M/h) 0.05069 [X] M [Y] M 0.1383 0.1860 0.1383 0.6783 0.18476 0.3804 0.1860 0.05079

Consider the following reaction performed at K and the given concentration and rate data: A products Experiment [A] Rate of reaction (M) (M/s) 1 0.78 0.0026988 2 1.56 0.0053976 3 3.12 0.0107952 First determine the rate law and rate constant. Based on this information; if you set up a new experiment where the [A]. (initial concentration of A) was 1.33 M, what would the concentration of A be after 144 s? [A](M) = number (rtol=0.01, atol=1e-08) ?

General Chemistry 4th Edition McQuarrie • Rock • Gallogly University Science Books presented by Macmillan Learning Initial-rate data at a certain temperature is given in the table for the reaction N,0,(g) NO(g) + NO,(g) [N,O,], (M) Initial rate (M/s) 0.100 0.480 0.200 0.9600 0.300 1.440 Determine the value and units of the rate constant. units: k =

Given below is the data for the reaction. Calculate the value of the rate constant "k" with proper units. A + B → C Set [A] (M) [B] (M) Init, rate M-sec 1 0.050 0.200 5.0 x 10-5 2. 0.100 0.200 5.0 x 10-5 0.050 0.600 4.5 x 10-4 Determine the order in "A" Determine the order in "B" Substitute the order for A and B in the rate law equation below. Rate = k [A]' [B]