The rate of the reaction in terms of the "appearance of product" includes the change in the concentration of the product, the time interval, and the coefficient of the product. Consider the following reaction: 2A+3B→3C+2D The concentrations of product C at three different time intervals are given. Use the following data to determine the rate of reaction in terms of the appearance of product C between time = 0 s and time = 20 s . Time (s) 0 20 40 [C](M) 0.000 0.0720 0.1440 Express your answer in molar concentration per second to three significant figures.

Express the average reaction rate for each time interval in moles of O2 produced per liter per minute. 0-100 s 500-600 s 1100-1200 s

Initial rates were measured for the following reaction and are listed in the table. A + 2B ⎯→ products   Expt. Initial Concentrations Initial Rate (mol/L·s) [A] [B] 1 0.115 0.135 2.70 × 10−3  2 0.115 0.270 2.16 × 10−2  3 0.345 0.135 8.10 × 10−3    Determine the rate law for the reaction including the value of the rate constant with the     correct units.

The following data were collected for the reaction: 2A > 4B + C Time Concentration of A Concentration of B (minutes) (moles/L) (moles/L) 1.000 0.000 10 0.800 0.400 20 0.667 0.677 30 0.571 0.858 40 0.500 1.000 50 0.444 1.112 1. Make a graph of the concentrations of A and B versus time. Estimate the rate of disappearance of A and the rate of formation of B at t= 25 min and at t= 40 min. Compare the rates of disappearance of A and formation of B. What would you expect the rate of formation of C to be at t= 25 min and t=40 min? 2. Determine graphically whether the reaction in #1 above is a first order or a second order reaction. Calculate the rate constant for the reaction.