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Derive an expression for a "1/4-life" for a first-order reaction.


A) Derive an expression for a 1/4-life for a first-order reaction. A) B) C) D) E)
B) Derive an expression for a 1/4-life for a first-order reaction. A) B) C) D) E)
C) Derive an expression for a 1/4-life for a first-order reaction. A) B) C) D) E)
D) Derive an expression for a 1/4-life for a first-order reaction. A) B) C) D) E)
E) Derive an expression for a 1/4-life for a first-order reaction. A) B) C) D) E)

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E

Given the following balanced equation, determine the rate of reaction with respect to [SO3]. 2SO2(g) + O2(g) → 2SO3(g)


A) Rate = - Given the following balanced equation, determine the rate of reaction with respect to [SO<sub>3</sub>]. 2SO<sub>2</sub>(g) + O<sub>2</sub>(g) → 2SO<sub>3</sub>(g) A) Rate = - B) Rate = + C) Rate = - D) Rate = + E) It is not possible to determine the answer without more information. Given the following balanced equation, determine the rate of reaction with respect to [SO<sub>3</sub>]. 2SO<sub>2</sub>(g) + O<sub>2</sub>(g) → 2SO<sub>3</sub>(g) A) Rate = - B) Rate = + C) Rate = - D) Rate = + E) It is not possible to determine the answer without more information.
B) Rate = + Given the following balanced equation, determine the rate of reaction with respect to [SO<sub>3</sub>]. 2SO<sub>2</sub>(g) + O<sub>2</sub>(g) → 2SO<sub>3</sub>(g) A) Rate = - B) Rate = + C) Rate = - D) Rate = + E) It is not possible to determine the answer without more information. Given the following balanced equation, determine the rate of reaction with respect to [SO<sub>3</sub>]. 2SO<sub>2</sub>(g) + O<sub>2</sub>(g) → 2SO<sub>3</sub>(g) A) Rate = - B) Rate = + C) Rate = - D) Rate = + E) It is not possible to determine the answer without more information.
C) Rate = - Given the following balanced equation, determine the rate of reaction with respect to [SO<sub>3</sub>]. 2SO<sub>2</sub>(g) + O<sub>2</sub>(g) → 2SO<sub>3</sub>(g) A) Rate = - B) Rate = + C) Rate = - D) Rate = + E) It is not possible to determine the answer without more information.
D) Rate = + Given the following balanced equation, determine the rate of reaction with respect to [SO<sub>3</sub>]. 2SO<sub>2</sub>(g) + O<sub>2</sub>(g) → 2SO<sub>3</sub>(g) A) Rate = - B) Rate = + C) Rate = - D) Rate = + E) It is not possible to determine the answer without more information.
E) It is not possible to determine the answer without more information.

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B

Which of the following statements is FALSE?


A) The rate of a chemical reaction is a measure of how fast a reaction occurs.
B) The half-life of a first-order reaction is independent of the initial concentration of reactant.
C) The rate of a zero-order reaction is dependent on the concentration of the reactant.
D) The rate law shows the relationship between the rate and the concentrations of each reactant.
E) The rate order with respect to each reactant must be determined experimentally.

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Determine the rate law and the value of k for the following reaction using the data provided: 2N2O5(g) → 4NO2(g) + O2(g) [N2O5]i (M) Initial Rate (M-1 s-1) 0) 093 4.84 × 10-4 0) 186 9.67 × 10-4 0) 279 1.45 × 10-3


A) Rate = 5.6 × 10-2 M-1 s-1[N2O5]2
B) Rate = 6.0 × 10-1 M-2 s-1[N2O5]3
C) Rate = 1.6 × 10-3 M1/2 s-1[N2O5]1/2
D) Rate = 1.7 × 10-2 M-1/2 s-1[N2O5]3/2
E) Rate = 5.2 × 10⁻3 s-1[N2O5]

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The first-order reaction, SO2Cl2 → SO2 + Cl2, has a rate constant equal to 2.20 × 10-5 s-1 at 593 K. What percentage of the initial amount of SO2Cl2 will remain after 6.00 hours?


A) 1.00%
B) 37.8%
C) 40.2%
D) 62.2%

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Given the following rate law, how does the rate of reaction change if the concentration of X is doubled? Rate = k [X]2[Y]3


A) The rate of reaction will increase by a factor of 9.
B) The rate of reaction will increase by a factor of 2.
C) The rate of reaction will increase by a factor of 8.
D) The rate of reaction will increase by a factor of 4.
E) The rate of reaction will remain unchanged.

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The combustion of ethylene proceeds by the reaction The combustion of ethylene proceeds by the reaction (g) + 3 (g) → 2C (g) + O(g) When the rate of disappearance of is 0.74 mol L<sup>-1</sup> , the rate of disappearance of is ________ A) 1.5 B) 0.49 C) 1.1 D) 2.2 E) 0.25 The combustion of ethylene proceeds by the reaction (g) + 3 (g) → 2C (g) + O(g) When the rate of disappearance of is 0.74 mol L<sup>-1</sup> , the rate of disappearance of is ________ A) 1.5 B) 0.49 C) 1.1 D) 2.2 E) 0.25 (g) + 3 The combustion of ethylene proceeds by the reaction (g) + 3 (g) → 2C (g) + O(g) When the rate of disappearance of is 0.74 mol L<sup>-1</sup> , the rate of disappearance of is ________ A) 1.5 B) 0.49 C) 1.1 D) 2.2 E) 0.25 (g) → 2C The combustion of ethylene proceeds by the reaction (g) + 3 (g) → 2C (g) + O(g) When the rate of disappearance of is 0.74 mol L<sup>-1</sup> , the rate of disappearance of is ________ A) 1.5 B) 0.49 C) 1.1 D) 2.2 E) 0.25 (g) + The combustion of ethylene proceeds by the reaction (g) + 3 (g) → 2C (g) + O(g) When the rate of disappearance of is 0.74 mol L<sup>-1</sup> , the rate of disappearance of is ________ A) 1.5 B) 0.49 C) 1.1 D) 2.2 E) 0.25 O(g) When the rate of disappearance of The combustion of ethylene proceeds by the reaction (g) + 3 (g) → 2C (g) + O(g) When the rate of disappearance of is 0.74 mol L<sup>-1</sup> , the rate of disappearance of is ________ A) 1.5 B) 0.49 C) 1.1 D) 2.2 E) 0.25 is 0.74 mol L-1 The combustion of ethylene proceeds by the reaction (g) + 3 (g) → 2C (g) + O(g) When the rate of disappearance of is 0.74 mol L<sup>-1</sup> , the rate of disappearance of is ________ A) 1.5 B) 0.49 C) 1.1 D) 2.2 E) 0.25 , the rate of disappearance of The combustion of ethylene proceeds by the reaction (g) + 3 (g) → 2C (g) + O(g) When the rate of disappearance of is 0.74 mol L<sup>-1</sup> , the rate of disappearance of is ________ A) 1.5 B) 0.49 C) 1.1 D) 2.2 E) 0.25 The combustion of ethylene proceeds by the reaction (g) + 3 (g) → 2C (g) + O(g) When the rate of disappearance of is 0.74 mol L<sup>-1</sup> , the rate of disappearance of is ________ A) 1.5 B) 0.49 C) 1.1 D) 2.2 E) 0.25 is ________ The combustion of ethylene proceeds by the reaction (g) + 3 (g) → 2C (g) + O(g) When the rate of disappearance of is 0.74 mol L<sup>-1</sup> , the rate of disappearance of is ________ A) 1.5 B) 0.49 C) 1.1 D) 2.2 E) 0.25


A) 1.5
B) 0.49
C) 1.1
D) 2.2
E) 0.25

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Explain what the exponential factor in the Arrhenius equation represents.

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The exponential factor depends on both t...

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How many half-lives are required for the concentration of reactant to decrease to 1.56% of its original value?


A) 6
B) 5
C) 7
D) 6.5
E) 7.5

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What are the two key components of the frequency factor?


A) Orientation factor and collision frequency
B) Activation energy and collision frequency
C) Orientation factor and ideal gas constant
D) Activation energy and temperature

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A

Define half-life.

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A half-life of a reaction is t...

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Nitrogen dioxide decomposes at 300 °C via a second-order process to produce nitrogen monoxide and oxygen according to the following chemical equation: 2NO2(g) → 2NO(g) + O2(g) . A sample of NO2(g) is initially placed in a 2.50 L reaction vessel at 300 °C. If the half-life and the rate constant at 300 °C are 11 seconds and 0.54 L mol-1 s-1, respectively, how many moles of NO2 were in the original sample?


A) 0. 17 mol
B) 0. 42 mol
C) 5.9 mol
D) 15 mol

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Derive an expression for a "1/3-life" for a first-order reaction.


A) Derive an expression for a 1/3-life for a first-order reaction. A) B) C) D) E)
B) Derive an expression for a 1/3-life for a first-order reaction. A) B) C) D) E)
C) Derive an expression for a 1/3-life for a first-order reaction. A) B) C) D) E)
D) Derive an expression for a 1/3-life for a first-order reaction. A) B) C) D) E)
E) Derive an expression for a 1/3-life for a first-order reaction. A) B) C) D) E)

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The aquation of tris (1,10-phenanthroline) iron(II) in acid solution takes place according to the equation: Fe(phen) 32+ + 3H3O+ + 3H2O → Fe(H2O) 62+ + 3phenH+. If the activation energy, Ea, is 126 kJ mol-1 and the rate constant at 30 °C is 9.8 × 10-3 min-1, what is the rate constant at 35°C?


A) 4.4 × 10-3 min-1
B) 2.2 × 10-2 min-1
C) 4.5 × 101 min-1
D) 2.3 × 102 min-1

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Match the following. -Ea


A) reaction order
B) frequency factor
C) activation energy
D) rate constant
E) half-life

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For a reaction that follows the general rate law Rate = k[A]1/2[B]2, what will happen to the rate of reaction if the concentration of A and B are is increased by a factor of 4?


A) The rate will decrease by a factor of 1/32.0.
B) The rate will decrease by a factor of 1/32.00.
C) The rate will increase by a factor of 32.
D) The rate will increase by a factor of 16.0.

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What data should be plotted to show that experimental concentration data fit a zeroth-order reaction?


A) ln[reactant] vs. time
B) What data should be plotted to show that experimental concentration data fit a zeroth-order reaction? A) ln[reactant] vs. time B) vs. time C) ln(k) vs. D) ln(k) vs. E<sub>a</sub> E) [reactant] vs. time vs. time
C) ln(k) vs. What data should be plotted to show that experimental concentration data fit a zeroth-order reaction? A) ln[reactant] vs. time B) vs. time C) ln(k) vs. D) ln(k) vs. E<sub>a</sub> E) [reactant] vs. time
D) ln(k) vs. Ea
E) [reactant] vs. time

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Which of the following represents the integrated rate law for a first-order reaction?


A) Which of the following represents the integrated rate law for a first-order reaction? A) = -kt B) - = kt C) [A]<sub>t</sub> - [A]<sub>0</sub> = -kt D) k = Ae<sup>(-</sup><sup>E</sup><sub>a</sub>/RT) E) = + lnA = -kt
B) Which of the following represents the integrated rate law for a first-order reaction? A) = -kt B) - = kt C) [A]<sub>t</sub> - [A]<sub>0</sub> = -kt D) k = Ae<sup>(-</sup><sup>E</sup><sub>a</sub>/RT) E) = + lnA - Which of the following represents the integrated rate law for a first-order reaction? A) = -kt B) - = kt C) [A]<sub>t</sub> - [A]<sub>0</sub> = -kt D) k = Ae<sup>(-</sup><sup>E</sup><sub>a</sub>/RT) E) = + lnA = kt
C) [A]t - [A]0 = -kt
D) k = Ae(-Ea/RT)
E) Which of the following represents the integrated rate law for a first-order reaction? A) = -kt B) - = kt C) [A]<sub>t</sub> - [A]<sub>0</sub> = -kt D) k = Ae<sup>(-</sup><sup>E</sup><sub>a</sub>/RT) E) = + lnA = Which of the following represents the integrated rate law for a first-order reaction? A) = -kt B) - = kt C) [A]<sub>t</sub> - [A]<sub>0</sub> = -kt D) k = Ae<sup>(-</sup><sup>E</sup><sub>a</sub>/RT) E) = + lnA Which of the following represents the integrated rate law for a first-order reaction? A) = -kt B) - = kt C) [A]<sub>t</sub> - [A]<sub>0</sub> = -kt D) k = Ae<sup>(-</sup><sup>E</sup><sub>a</sub>/RT) E) = + lnA + lnA

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Given the following proposed mechanism, predict the rate law for the overall reaction. A2 + 2B → 2AB (overall reaction) Mechanism A2 ⇌ 2A fast A + B → AB slow


A) Rate = k[A][B]
B) Rate = k[A2][B]
C) Rate = k[A2][B]1/2
D) Rate = k[A2]
E) Rate = k[A2]1/2[B]

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Determine the rate law and the value of k for the following reaction using the data provided: NO2(g) + O3(g) → NO3(g) + O2(g) [NO2]i (M) [O3]i (M) Initial Rate (M-1 s-1) 0) 10 0.33 1.42 0) 10 0.66 2.84 0) 25 0.66 7.10


A) Rate = 1360 M-2.5 s-1[NO2]2.5[O3]
B) Rate = 227 M-2.5 s-1[NO2][O3]2.5
C) Rate = 43 M-1 s-1[NO2][O3]
D) Rate = 430 M-2 s-1[NO2]2[O3]
E) Rate = 130 M-2 s-1[NO2][O3]2

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