Dinitrogen tetroxide decomposes to form nitrogen dioxide in a second-order reaction: N2O4(g)→ 2NO2(g) At 400.0 K,the rate constant for this reaction has been measured to be 2.9 × 108 L/(mol ∙ s).Suppose 0.742 mol of N2O4(g)is placed in a sealed 34.3-L container at 400.0 K and allowed to react.What is the total pressure inside the vessel after 49.6 ns has elapsed? (R= 0.0821 (L ∙ atm)/(K ∙ mol))

A) 0.879 atm B) 0.7138 atm C) 0.541 atm D) 2.13 atm E) 1.42 atm A) 0.879 atm B) 0.7138 atm C) 0.541 atm D) 2.13 atm E) 1.42 atm A

The following mechanism has been suggested for the reaction between nitrogen monoxide and oxygen: NO(g)+ NO(g)→ N2O2(g)(fast) N2O2(g)+ O2(g)→ 2NO2(g)(slow) According to this mechanism,the experimental rate law is

A) second-order in NO and zero-order in O2. B) second-order in NO and first-order in O2. C) first-order in NO and first-order in O2. D) first-order in NO and second-order in O2. E) first-order in NO and zero-order in O2. A) second-order in NO and zero-order in O2. B) second-order in NO and first-order in O2. C) first-order in NO and first-order in O2. D) first-order in NO and second-order in O2. E) first-order in NO and zero-order in O2. B

The oxidation of ammonia produces nitrogen and water via the following reaction: 4NH3(g)+ 3O2(g)→ 2N2(g)+ 6H2O(l) Suppose the rate of formation of H2O(l)is 3.0 mol/(L ∙ s).Which of the following statements is true?

A) The rate of consumption of NH3 is 2.0 mol/(L ∙ s). B) The rate of consumption of O2 is 2.0 mol/(L ∙ s). C) The rate of formation of N2 is 1.3 mol/(L ∙ s). D) The rate of formation of N2 is 2.0 mol/(L ∙ s). E) The rate of consumption of NH3 is 0.50 mol/(L ∙ s). A) The rate of consumption of NH3 is 2.0 mol/(L ∙ s). B) The rate of consumption of O2 is 2.0 mol/(L ∙ s). C) The rate of formation of N2 is 1.3 mol/(L ∙ s). D) The rate of formation of N2 is 2.0 mol/(L ∙ s). E) The rate of consumption of NH3 is 0.50 mol/(L ∙ s).

In aqueous solution,iodine reacts with acetone as represented by the following equation: I2(aq)+ CH3COCH3(aq)→ CH3COCH2I(aq)+ H+(aq)+ I-(aq) The experimental rate law is Rate = k[H+][CH3COCH3].According to the information above,an increase in the hydrogen ion concentration has what effect on the reaction?

A) It decreases the rate of the reaction. B) It increases the rate of the reaction. C) It decreases the value of the equilibrium constant. D) It increases the value of the equilibrium constant. E) It does not affect the rate of the reaction. A) It decreases the rate of the reaction. B) It increases the rate of the reaction. C) It decreases the value of the equilibrium constant. D) It increases the value of the equilibrium constant. E) It does not affect the rate of the reaction.

A proposed mechanism for the decomposition of N2O5 is as follows: N2O5 NO2 + NO3 Slow step NO2 + NO3 NO2 + O2 + NO Fast step NO + N2O5 3NO2 Fast step What is the rate law predicted by this mechanism?

A) Rate = k1k2[N2O5][NO2][NO3] B) Rate = k2[NO2][NO3] C) Rate = k3[NO][N2O5] D) Rate = k1k2k3[N2O5]2 E) Rate = k1[N2O5] A) Rate = k1k2[N2O5][NO2][NO3] B) Rate = k2[NO2][NO3] C) Rate = k3[NO][N2O5] D) Rate = k1k2k3[N2O5]2 E) Rate = k1[N2O5]

A suggested mechanism for the decomposition of ozone is as follows: O3 O2 + O fast equilibrium O + O3 2O2 slow step What is the rate law predicted by this mechanism?

A) Rate = B) Rate = k2[O] [O3] C) Rate = D) Rate = E) Rate = A) Rate = B) Rate = k2[O] [O3] C) Rate = D) Rate = E) Rate =

Exam 13: Rates of Reaction

Dinitrogen tetroxide decomposes to form nitrogen dioxide in a second-order reaction: N₂O₄(g)→ 2NO₂(g) At 400.0 K,the rate constant for this reaction has been measured to be 2.9 × 10⁸ L/(mol ∙ s).Suppose 0.742 mol of N₂O₄(g)is placed in a sealed 34.3-L container at 400.0 K and allowed to react.What is the total pressure inside the vessel after 49.6 ns has elapsed? (R= 0.0821 (L ∙ atm)/(K ∙ mol))

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Question 1

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The following mechanism has been suggested for the reaction between nitrogen monoxide and oxygen: NO(g)+ NO(g)→ N₂O₂(g)(fast) N₂O₂(g)+ O₂(g)→ 2NO₂(g)(slow) According to this mechanism,the experimental rate law is

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Question 2

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For the reaction of the ammonium ion with nitrous acid,the net reaction is NH₄⁺(aq)+ HNO₂(aq)→ N₂(g)+ 2H₂O(l)+ H⁺(aq) If the initial concentration of nitrous acid is 1.00 M and,after 17.8 s has elapsed,the concentration of nitrous acid has fallen to 0.72 M,what is the average rate of the reaction over this time interval?

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Question 3

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In a chemical reaction at constant temperature,the addition of a catalyst

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Question 4

The oxidation of ammonia produces nitrogen and water via the following reaction: 4NH₃(g)+ 3O₂(g)→ 2N₂(g)+ 6H₂O(l) Suppose the rate of formation of H₂O(l)is 3.0 mol/(L ∙ s).Which of the following statements is true?

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Question 5

How many mechanistic steps are depicted by in this potential energy diagram for the decomposition of cyclobutane to ethylene?

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Question 6

In aqueous solution,iodine reacts with acetone as represented by the following equation: I₂(aq)+ CH₃COCH₃(aq)→ CH₃COCH₂I(aq)+ H⁺(aq)+ I^-(aq) The experimental rate law is Rate = k[H⁺][CH₃COCH₃].According to the information above,an increase in the hydrogen ion concentration has what effect on the reaction?

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Question 7

The complete mechanism for a reaction is considered to occur in two steps,one of which is slow and the other fast: A + B → C + D slow A + C → E + F fast What is the net chemical equation predicted by this mechanism?

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Question 8

For the reaction 6CH₂O(aq)+ 4NH₃(aq)→ (CH₂)₆N₄(aq)+ 6H₂O(l) The rate of the reaction may be expressed as )What is an equivalent expression for the rate of the reaction?

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Question 9

For a second-order reaction,what are the possible units of the rate constant?

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Question 10

Identify the rate equation of the termolecular elementary reaction given below. A + B + C $\rarr$ D + E

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Question 11

For the reaction between nitrogen monoxide and chlorine to produce nitrosyl chloride,2NO(g)+ Cl₂(g)→ 2NOCl(g),it is found that tripling the initial concentration of both reactants increases the initial rate by a factor of 27.If only the initial concentration of chlorine is tripled,the initial rate increases by a factor of 3.What is the order of the reaction with respect to Cl₂?

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Question 12

Consider the reaction AA + bB DD + eE C = catalyst The rate law is Rate = k[A]^q[B]^r[C]s Which of the following statements is incorrect?

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Question 13

For the hypothetical second-order reaction A → products,k = 0.379 M^-1 s^-1.If the initial concentration of A is 0.799 M,how long would it take for A to be 39.7% consumed?

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Question 14

The following data were obtained for the hypothetical reaction 2A + B → products. What is the overall order of this reaction?

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Question 15

The reaction between selenous acid and the iodide ion in acid solution is H₂SeO₃(aq)+ 6I^-(aq)+ 4H⁺(aq)→ Se(s)+ 2I₃^-(aq)+ 3H₂O(l) The data in the following table were measured at 0°C. Experiment [H₂SeO₃]₀ (M) [H⁺]₀ (M) [I^-]₀ (M) Initial Rate [mol/(L ∙ s)] 1 1)00 × 10^-4 2)00 × 10^-2 3)00 × 10^-2 5)30 × 10^-7 2 2)00 × 10^-4 2)00 × 10^-2 3)00 × 10^-2 1)06 × 10^-6 3 3)00 × 10^-4 4)00 × 10^-2 3)00 × 10^-2 6)36 × 10^-6 4 3)00 × 10^-4 8)00 × 10^-2 3)00 × 10^-2 2)54 × 10^-5 5 3)00 × 10^-4 8)00 × 10^-2 6)00 × 10^-2 2)04 × 10^-4 6 2)00 × 10^-4 2)00 × 10^-2 6)00 × 10^-2 8)48 × 10^-6 Tripling the initial concentration of I^- while holding the initial concentrations of H₂SeO₃ and H⁺ constant increases the initial rate of the reaction by a factor of

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Question 16

Which of the following statements is true concerning the reaction given below? 2H₂S(g)+ O₂(g)→ 2S(s)+ 2H₂O(g)

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Question 17

Which of the following statements is always true?

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Question 18

A proposed mechanism for the decomposition of N₂O₅ is as follows: N₂O₅ NO₂ + NO₃ Slow step NO₂ + NO₃ NO₂ + O₂ + NO Fast step NO + N₂O₅ 3NO₂ Fast step What is the rate law predicted by this mechanism?

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Question 19

A suggested mechanism for the decomposition of ozone is as follows: O₃ O₂ + O fast equilibrium O + O₃ 2O₂ slow step What is the rate law predicted by this mechanism?

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Question 20

Showing 1 - 20 of 113

The following mechanism has been suggested for the reaction between nitrogen monoxide and oxygen: NO(g)+ NO(g)→ N₂O₂(g)(fast) N₂O₂(g)+ O₂(g)→ 2NO₂(g)(slow) According to this mechanism,the experimental rate law is

In a chemical reaction at constant temperature,the addition of a catalyst

The oxidation of ammonia produces nitrogen and water via the following reaction: 4NH₃(g)+ 3O₂(g)→ 2N₂(g)+ 6H₂O(l) Suppose the rate of formation of H₂O(l)is 3.0 mol/(L ∙ s).Which of the following statements is true?

How many mechanistic steps are depicted by in this potential energy diagram for the decomposition of cyclobutane to ethylene?

The complete mechanism for a reaction is considered to occur in two steps,one of which is slow and the other fast: A + B → C + D slow A + C → E + F fast What is the net chemical equation predicted by this mechanism?

For the reaction 6CH₂O(aq)+ 4NH₃(aq)→ (CH₂)₆N₄(aq)+ 6H₂O(l) The rate of the reaction may be expressed as )What is an equivalent expression for the rate of the reaction?

For a second-order reaction,what are the possible units of the rate constant?

Identify the rate equation of the termolecular elementary reaction given below. A + B + C $\rarr$ D + E

Consider the reaction AA + bB DD + eE C = catalyst The rate law is Rate = k[A]^q[B]^r[C]s Which of the following statements is incorrect?

For the hypothetical second-order reaction A → products,k = 0.379 M^-1 s^-1.If the initial concentration of A is 0.799 M,how long would it take for A to be 39.7% consumed?

The following data were obtained for the hypothetical reaction 2A + B → products. What is the overall order of this reaction?

Which of the following statements is true concerning the reaction given below? 2H₂S(g)+ O₂(g)→ 2S(s)+ 2H₂O(g)

Which of the following statements is always true?

A proposed mechanism for the decomposition of N₂O₅ is as follows: N₂O₅ NO₂ + NO₃ Slow step NO₂ + NO₃ NO₂ + O₂ + NO Fast step NO + N₂O₅ 3NO₂ Fast step What is the rate law predicted by this mechanism?

A suggested mechanism for the decomposition of ozone is as follows: O₃ O₂ + O fast equilibrium O + O₃ 2O₂ slow step What is the rate law predicted by this mechanism?

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Exam 13: Rates of Reaction

The following mechanism has been suggested for the reaction between nitrogen monoxide and oxygen: NO(g)+ NO(g)→ N2O2(g)(fast) N2O2(g)+ O2(g)→ 2NO2(g)(slow) According to this mechanism,the experimental rate law is

In a chemical reaction at constant temperature,the addition of a catalyst

The oxidation of ammonia produces nitrogen and water via the following reaction: 4NH3(g)+ 3O2(g)→ 2N2(g)+ 6H2O(l) Suppose the rate of formation of H2O(l)is 3.0 mol/(L ∙ s).Which of the following statements is true?

How many mechanistic steps are depicted by in this potential energy diagram for the decomposition of cyclobutane to ethylene?

The complete mechanism for a reaction is considered to occur in two steps,one of which is slow and the other fast: A + B → C + D slow A + C → E + F fast What is the net chemical equation predicted by this mechanism?

For the reaction 6CH2O(aq)+ 4NH3(aq)→ (CH2)6N4(aq)+ 6H2O(l) The rate of the reaction may be expressed as )What is an equivalent expression for the rate of the reaction?

For a second-order reaction,what are the possible units of the rate constant?

Identify the rate equation of the termolecular elementary reaction given below. A + B + C →\rarr→ D + E

Consider the reaction AA + bB DD + eE C = catalyst The rate law is Rate = k[A]q[B]r[C]s Which of the following statements is incorrect?

For the hypothetical second-order reaction A → products,k = 0.379 M-1 s-1.If the initial concentration of A is 0.799 M,how long would it take for A to be 39.7% consumed?

The following data were obtained for the hypothetical reaction 2A + B → products. What is the overall order of this reaction?

Which of the following statements is true concerning the reaction given below? 2H2S(g)+ O2(g)→ 2S(s)+ 2H2O(g)

Which of the following statements is always true?

A proposed mechanism for the decomposition of N2O5 is as follows: N2O5 NO2 + NO3 Slow step NO2 + NO3 NO2 + O2 + NO Fast step NO + N2O5 3NO2 Fast step What is the rate law predicted by this mechanism?

A suggested mechanism for the decomposition of ozone is as follows: O3 O2 + O fast equilibrium O + O3 2O2 slow step What is the rate law predicted by this mechanism?

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Calculations With Chemical Formulas and Equations

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The Gaseous State

Thermochemistry

Quantum Theory of the Atom

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Molecular Geometry and Chemical Bonding Theory

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Solutions

Chemical Equilibrium

Acids and Bases

Acid-Base Equilibria

Solubility and Complex-Ion Equilibria

Thermodynamics and Equilibrium

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Chemistry of the Main-Group Metals

The Transition Elements and Coordination Compounds

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The following mechanism has been suggested for the reaction between nitrogen monoxide and oxygen: NO(g)+ NO(g)→ N₂O₂(g)(fast) N₂O₂(g)+ O₂(g)→ 2NO₂(g)(slow) According to this mechanism,the experimental rate law is

The oxidation of ammonia produces nitrogen and water via the following reaction: 4NH₃(g)+ 3O₂(g)→ 2N₂(g)+ 6H₂O(l) Suppose the rate of formation of H₂O(l)is 3.0 mol/(L ∙ s).Which of the following statements is true?

For the reaction 6CH₂O(aq)+ 4NH₃(aq)→ (CH₂)₆N₄(aq)+ 6H₂O(l) The rate of the reaction may be expressed as )What is an equivalent expression for the rate of the reaction?

Identify the rate equation of the termolecular elementary reaction given below. A + B + C $\rarr$ D + E

Consider the reaction AA + bB DD + eE C = catalyst The rate law is Rate = k[A]^q[B]^r[C]s Which of the following statements is incorrect?

For the hypothetical second-order reaction A → products,k = 0.379 M^-1 s^-1.If the initial concentration of A is 0.799 M,how long would it take for A to be 39.7% consumed?

Which of the following statements is true concerning the reaction given below? 2H₂S(g)+ O₂(g)→ 2S(s)+ 2H₂O(g)

A proposed mechanism for the decomposition of N₂O₅ is as follows: N₂O₅ NO₂ + NO₃ Slow step NO₂ + NO₃ NO₂ + O₂ + NO Fast step NO + N₂O₅ 3NO₂ Fast step What is the rate law predicted by this mechanism?

A suggested mechanism for the decomposition of ozone is as follows: O₃ O₂ + O fast equilibrium O + O₃ 2O₂ slow step What is the rate law predicted by this mechanism?