A chemical reaction involves the reactants A and B, and the product C. A+B C Trial [A] (l) [B](mol) A[A] mol L At Ls 1 0.030 0.030 0.0004851 2 0.030 0.060 0.0004851 3 0.060 0.030 0.0019404 Use the experimental data above and the method of initial rates to determine the complete rate law for the reaction. Type in the entire rate law expression, including the value of k. • Enter the order of the reactants A and B as the exponents on [A] and [B] respectively. • Report your value of k as a decimal with two significant figures. Provide your answer below: rate = ☐[A] [B]

Two mechanisms are proposed for the reaction 2NO(g)+O2(g)2NO2(g)Mechanism 1: NO+O2NO3(fast) NO3+NO2NO2(slow) Mechanism 2: NO+ON2O2(fast) N2O2+O22NO2(slow) Show that each of these mechanisms is consistent with the observed rate law: rate=k[ NO2 ]2[ O2 ].

11.102 Suppose that you are studying a reaction and need to determine its rate law. Explain what you would need to measure in order to accomplish this in a single experiment, and how you could use graphical methods to get from the experimental data to a complete rate law.

The initial rate for a reaction is equal to the slope of the tangent line at t 0 in a plot of [A] versus time. From calculus, initial rate = d[A]dt . Therefore. the differential rate law for a reaction is Rate = d[A]dt=k[A]n. Assuming you have some calculus in your background, derive the zero-, first-, and second-order integrated rate laws using the differential rate law.

Candle wax is a mixture of hydrocarbons. In the reaction of oxygen with candle w ax in Figure 11.2, the rate of consumption of oxygen decreased with time after the flask was covered, and eventually' the flame went out. From the perspective of the kinetic-molecular theory, describe what is happening in the flask. FIGURE 11.2 When a candle burns in a closed container, the flame will diminish and eventually go out. As the amount of oxygen present decreases, the rate of combustion will also decrease. Eventually, the rate of combustion is no longer sufficient to sustain the flame even though there is still some oxygen present in the vessel.

For the reaction A + B C, explain at least two ways in which the rate law could be zero order in chemical A.

Can a reaction mechanism ever be proven correct? Can it be proven incorrect?

A study of the rate of dimerization of C4H6 gave the data shown in the table: 2C4H6C8H12 (a) Determine the average rate of dimerization between 0 s and 1600 s, and between 1600 s and 3200 s. (b) Estimate the instantaneous rate of dimerization at 3200 s from a graph of time versus [C4H6]. What are the units of this rate? (c) Determine the average rate of formation of C8H12 at 1600 s and the instantaneous rate of formation at 3200 s from the rates found in parts (a) and (b).

. Account for the increase in reaction rate brought about by a catalyst.

. find the rate law predicted for a particular reaction mechanism.