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Flashcards: Kinetics and Kinematics

A scientist is studying a reaction, and places the reactants in a beaker at room temperature. The reaction progresses, and she analyzes the products via NMR. Based on the NMR readout, she determines the reaction proceeds as follows:

$NH_{4}^{+}(aq) + NO_{2}^{-}(aq) \rightarrow N_{2}(g) +2H_{2}O(l)$ $\displaystyle NH_{4}^{+}(aq) + NO_{2}^{-}(aq) \rightarrow N_{2}(g) +2H_{2}O(l)$

In an attempt to better understand the reaction process, she varies the concentrations of the reactants and studies how the rate of the reaction changes. The table below shows the reaction concentrations as she makes modifications in three experimental trials.

$\begin{matrix} Trial & [NH_4^+] & [NO_2^-] &Rate \\ 1& 0.480M &0.120M &0.018\frac{M}{s} \\ 2& 0.240M & 0.120M& 0.009\frac{M}{s}\\ 3& 0.240M& 0.360M & 0.027\frac{M}{s} \end{matrix}$ $\displaystyle \begin{matrix} Trial & [NH_4^+] & [NO_2^-] &Rate \\ 1& 0.480M &0.120M &0.018\frac{M}{s} \\ 2& 0.240M & 0.120M& 0.009\frac{M}{s}\\ 3& 0.240M& 0.360M & 0.027\frac{M}{s} \end{matrix}$

Reaction rates depend on reaction concentrations, as well as the reaction constant $\displaystyle k$. The Arrhenius equation is used to calculate this constant. Which of the following factors is used in the Arrhenius equation?

I. Temperature

II. Activation energy

III. Reactant concentrations

I only

III only

I and II

II and III

I, II, and III

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Flashcards: Kinetics and Kinematics

$NH_{4}^{+}(aq) + NO_{2}^{-}(aq) \rightarrow N_{2}(g) +2H_{2}O(l)$ $\displaystyle NH_{4}^{+}(aq) + NO_{2}^{-}(aq) \rightarrow N_{2}(g) +2H_{2}O(l)$

I. Temperature

II. Activation energy

III. Reactant concentrations

I only

III only

I and II

II and III

I, II, and III

Report an Error Copyright Notice

Flashcards: Kinetics and Kinematics

I. Temperature

II. Activation energy

III. Reactant concentrations

Your answer:

I only

Your answer:

III only

Your answer:

II and III

Your answer:

I, II, and III

Correct answer:

I and II

Explanation:

If you thought all of these factors are used in the Arrhenius equation, consider that the rate constant is independent of the reactant concentrations. The concentration effect is considered in the rate law by multiplying the concentrations by the constant, but the concentrations themselves are independent of the actual Arrhenius calculation.

The calculation shows that $k=Ae^{-\frac{E_a}{RT}}$ $\displaystyle k=Ae^{-\frac{E_a}{RT}}$. In this equation, $\small E_a$ $\displaystyle \small E_a$ is the activation energy and $\small T$ $\displaystyle \small T$ is the temperature.

Flashcards: Kinetics and Kinematics

$A + 2B + C \rightarrow D$ $\displaystyle A + 2B + C \rightarrow D$

You want to find the order of each reactant by manipulating the reactant concentrations in multiple trials. The table below shows the effect of altered reactant concentrations on initial reaction rate.

$\begin{matrix} \text{Trial} & \text{Initial [A]} & \text{Initial [B]} & \text{Initial [C]} & \text{Rate}\ (\frac{M}{s})\\ 1&0.1 &0.3 &0.2 &0.002 \\ 2& 0.1& 0.9& 0.2& 0.006\\ 3& 0.2& 0.3& 0.2& 0.002\\ 4& 0.1& 0.3& 0.4 & 0.008 \end{matrix}$ $\displaystyle \begin{matrix} \text{Trial} & \text{Initial [A]} & \text{Initial [B]} & \text{Initial [C]} & \text{Rate}\ (\frac{M}{s})\\ 1&0.1 &0.3 &0.2 &0.002 \\ 2& 0.1& 0.9& 0.2& 0.006\\ 3& 0.2& 0.3& 0.2& 0.002\\ 4& 0.1& 0.3& 0.4 & 0.008 \end{matrix}$

Using the above trials, write the rate law for the reaction.

$\displaystyle Rate=k[A][B][C]$

$Rate = k[B][C]^{2}$ $\displaystyle Rate = k[B][C]^{2}$

$Rate = k[A][B]^{2}[C]$ $\displaystyle Rate = k[A][B]^{2}[C]$

$Rate = k[A][B][C]^{2}$ $\displaystyle Rate = k[A][B][C]^{2}$

$Rate = k[B]^{2}[C]^{4}$ $\displaystyle Rate = k[B]^{2}[C]^{4}$

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Flashcards: Kinetics and Kinematics

Using the above trials, write the rate law for the reaction.

Your answer:

$\displaystyle Rate=k[A][B][C]$

Your answer:

$Rate = k[A][B]^{2}[C]$ $\displaystyle Rate = k[A][B]^{2}[C]$

Your answer:

$Rate = k[A][B][C]^{2}$ $\displaystyle Rate = k[A][B][C]^{2}$

Your answer:

$Rate = k[B]^{2}[C]^{4}$ $\displaystyle Rate = k[B]^{2}[C]^{4}$

Correct answer:

$Rate = k[B][C]^{2}$ $\displaystyle Rate = k[B][C]^{2}$

Explanation:

Keep in mind that the chemical equation and its coefficients have NOTHING to do with the rate law. The order of each reactant must be determined by experiment.

To find the order of each reactant, compare the initial reaction rates of two trials in which only one of the three reactants' concentrations is altered. For example, trials 1 and 4 keep A and B equal, but C is doubled. When C is doubled, we see that the initial reaction rate is quadrupled. As a result, we determine that the order of reactant C is 2. When the reactant is altered, but the initial reaction rate is kept constant, as seen in trials 1 and 3 with respect to A, the order of that reactant is 0. Finally, when the reactant is multiplied by the same factor that the initial reaction rate is multiplied, as seen in trials 1 and 2 with respect to B, the order of the reactant is 1.

Putting the data together: A is zeroth order, B is first order, and C is second order. Our rate law can thus be written $\displaystyle Rate=k[B][C]^2$.

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Flashcards: Kinetics and Kinematics

All GRE Subject Test: Chemistry Resources

Flashcards: Kinetics and Kinematics

Flashcards: Kinetics and Kinematics

Flashcards: Kinetics and Kinematics

Flashcards: Kinetics and Kinematics

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Flashcards: Kinetics and Kinematics

All GRE Subject Test: Chemistry Resources

Flashcards: Kinetics and Kinematics

Flashcards: Kinetics and Kinematics

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Flashcards: Kinetics and Kinematics

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