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Exam 14: Chemical Kinetics

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Question 41

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At elevated temperatures, dinitrogen pentoxide decomposes to nitrogen dioxide and oxygen: 2N₂O₅(g) → 4NO₂ (g) + O₂ (g) When the rate of formation of NO₂ is 5.5 × 10^{- 4} M/s, the rate of decomposition of ^N2^O5 is M/s)

A) 10.1 × 10^{- 4}
B) 5.5 × 10^{- 4}
C) 2.8 × 10^{- 4}
D) 2.2 × 10^{- 3}
E) 1.4 × 10^{- 4}

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Question 42

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The concentration of S₂O₈^2- remaining at 400 s is _ M.

A) +0.057
B) - 0.007
C) +0.015
D) +0.035
E) +0.045

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Question 43

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The graph shown below depicts the relationship between concentration and time for the following chemical reaction. The slope of this line is equal to .

The rate constant for a second- order reaction is 0.13 M^{- 1}s^{- 1}. If the initial concentration of reactant is 0.26 mol/L, it takes s for the concentration to decrease to 0.13 mol/L.

The average rate of disappearance of I^- between 400 s and 800 s is M/s.

The rate of disappearance of HBr in the gas phase reaction 2HBr (g) → H₂ (g) + Br₂ (g) Is 0.190 M s^{- 1} at 150°C. The rate of reaction is M s^{- 1}.

At elevated temperatures, methylisonitrile (CH₃NC) isomerizes to acetonitrile (CH₃CN) : CH₃NC (g) → CH₃CN (g) At the start of an experiment, there are 0.200 mol of reactant and 0 mol of product in the reaction vessel. After 25 min, 0.108 mol of reactant (CH₃NC) remain. There are _ _ mol of product (CH₃CN) in the reaction vessel.

The kinetics of the reaction below were studied and it was determined that the reaction rate did not change when the concentration of B was tripled. The reaction is order in B. A + B → P

The data in the table below were obtained for the reaction: 2 ClO₂ (aq) + 2 OH^- (aq) →ClO₃^- (aq) + ClO₂^- (aq) + H₂O (1) -What is the magnitude of the rate constant for the reaction?

The enzyme nitrogenase converts _ _ into _.

Heterogeneous catalysts have different phases from reactants.

Of the units below, are appropriate for a first- order reaction rate constant.

The concentration of reactants or products at any time during the reaction can be calculated from the integrated rate law.

A catalyst can increase the rate of a reaction .

Consider the following reaction: A - 2C The average rate of appearance of C is given by O[C]/Ot. Comparing the rate of appearance of C and the rate of disappearance of A, we get O[C]/Ot = × (O[A]/Ot) .

Reaction rate data obey an equation devised by _ .

In general, as temperature goes up, reaction rate .

The reaction 2NO₂ → 2NO + O₂ Follows second- order kinetics. At 300°C, [NO₂] drops from 0.0100- to 0.00650- M in 100 s. The rate constant for the reaction is _ M^{- 1}s^{- 1}.

The data in the table below were obtained for the reaction: A + B → P -The magnitude of the rate constant is .

Which one of the following graphs shows the correct relationship between concentration and time for a reaction that is second order in [A]?