The rate constant at $325^{\circ} \mathrm{C}$ for the decomposition reaction $\mathrm{C}_4 \mathrm{H}_8 \longrightarrow 2 \mathrm{C}_2 \mathrm{H}_4$ is $6.1 \times 10^{-8} \mathrm{~s}$, and the activation energy is $261 \mathrm{~kJ}$ per mole of $\mathrm{C}_4 \mathrm{H}_8$. Determine the frequency factor for the reaction.

The annual production of $\mathrm{HNO}_{3}$ in 2013 was 60 million metric tons Most of that was prepared by the following sequence of reactions, each run in a separate reaction vessel. (a) $4 \mathrm{NH}_{3}(g)+5 \mathrm{O}_{2}(g) \longrightarrow 4 \mathrm{NO}(g)+6 \mathrm{H}_{2} \mathrm{O}(g)$ (b) $2 \mathrm{NO}(g)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{NO}_{2}(g)$ (c) $3 \mathrm{NO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow 2 \mathrm{HNO}_{3}(a q)+\mathrm{NO}(g)$ The first reaction is run by burning ammonia in air over a platinum catalyst. This reaction is fast. The reaction in equation (c) is also fast. The second reaction limits the rate at which nitric acid can be prepared from ammonia. If equation (b) is second order in NO and first order in $\mathrm{O}_{2}$, what is the rate of formation of $\mathrm{NO}_{2}$ when the oxygen concentration is 0.50 Mand the nitric oxide concentration is 0.75 M? The rate constant for the reaction is 5.8 x $10^{-6} \mathrm{L}^{2} / \mathrm{mol}^{2} / \mathrm{s}$.

Nitrogen monoxide reacts with chlorine according to the equation:

$$2 \mathrm{NO}(\mathrm{g})+\mathrm{Cl}_2(\mathrm{~g}) \longrightarrow 2 \mathrm{NOCl}(\mathrm{g})$$

The following initial rates of reaction have been observed for certain reactant concentrations:

What is the rate law that describes the rate's dependence on the concentrations of $\mathrm{NO}_2$ and $\mathrm{Cl}_2$ ? What is the rate constant? What are the orders with respect to each reactant?

Regular flights of supersonic aircraft in the stratosphere are of concern because such aircraft produce nitric oxide, NO, as a byproduct in the exhaust of their engines. Nitric oxide reacts with ozone, and it has been suggested that this could contribute to depletion of the ozone layer. The reaction $\mathrm{NO}+\mathrm{O}_{3} \longrightarrow \mathrm{NO}_{2}+\mathrm{O}_{2}$ is first order with respect to both NO and $\mathrm{O}_{3}$ with a rate constant of 2.20 $\times 10^{7}$ L/mol/s. What is the instantaneous rate of disappearance of NO when [NO] = 3.3 $\times 10^{-6}$ M and [$\mathrm{O}_{3}$] = 5.9 $\times 10^{-7}$ M?

In a kinetics experiment, a chemist places crystals of iodine in a closed reaction vessel, introduces a given quantity of hydrogen gas, and obtains data to calculate the rate of hydrogen iodide formation. In a second experiment, she uses the same amounts of iodine and hydrogen, but first warms the flask to $130 ^ { \circ } \mathrm { C } ,$ a temperature above the sublimation point of iodine. In which of these experiments does the reaction proceed at a higher rale? Explain.

Indicate whether each of the following statements about Helicobacter pylori (Hp) bacteria in the human stomach is true or false.

a. Hp is a bacterium that can live in highly acidic environments.

b. Hp bacteria use the enzyme urease to directly neutralize stomach acid.

c. Hp bacteria irritate the stomach lining by interfering with the protective mucous coating present.

d. Poor sanitation conditions correlate well with Hp infection rates.

Explain how Uncle Tom's Cabin affected the abolitionist cause. Use details from the lesson to support your answer.

The rate of a certain reaction doubles for every $10^{\circ} \mathrm{C}$ rise in temperature. (a) How much faster does the reaction proceed at $45^{\circ} \mathrm{C}$ than at $25^{\circ} \mathrm{C}$ ? (b) How much faster does the reaction proceed at $95^{\circ} \mathrm{C}$ than at $25^{\circ} \mathrm{C}$ ?

How does an increase in temperature affect rate of reaction? Explain this effect in terms of the collision theory of the reaction rate.

Describe how graphical methods can be used to determine the activation energy of a reaction from a series of data that includes the rate of reaction at varying temperatures.

Account for the relationship between the rate of a reaction and its activation energy.

What is the activation energy of a reaction, and how is this energy related to the activated complex of the reaction?

When every collision between reactants leads to a reaction, what determines the rate at which the reaction occurs?

Chemical reactions occur when reactants collide. What are two factors that may prevent a collision from producing a chemical reaction?