Question 1

The Haber process is the synthesis of ammonia gas from hydrogen and nitrogen on a hot metal surface.What is the catalyst and what type of catalysis is occurring?

Accepted Answer

The catalyst for the Haber process is a metal surface, specifically iron, which acts as a heterogeneous catalyst by providing a surface for the reaction to occur on. None of the other choices listed match this description.

Question 2

The reaction below is second order in ClO₂ and first order in OH^-.When the concentration of ClO₂ is 0.020 M and the concentration of OH^- is 0.10 M,the initial rate of reaction is 8.00 × 10^-4 M/s.What is the rate constant,k,for this reaction? 2 ClO₂(aq)+ 2 OH^-(aq)→ ClO₃^-(aq)+ ClO₂^-(aq)+ H₂O(l)

Accepted Answer

The answer of The reaction below is second order in...

Question 3

A catalyst increases the rate of a reaction by providing a different reaction pathway that

Accepted Answer

A catalyst lowers the activation energy required for a reaction, allowing it to happen more quickly. It does not affect the energy of the products or reactants, only the activation energy.

Question 4

For the reaction shown below,if the rate of formation of O₂ is 6.5 × 10^-6M/s,the rate of decomposition of N₂O₅ over the same time interval is ________. 2 N₂O₅(g)→ 4 NO₂(g)+ O₂(g)

Accepted Answer

The answer of For the reaction shown below,if the rate...

Question 5

A gaseous compound,C,undergoes catalytic decomposition at an initial rate of 0.45 M/s when [C]_o = 3.0 × 10^-3 M and 0.45 M/s when [C]_o = 9.0 × 10^-3 M.Therefore,this is a ________ order reaction.

Accepted Answer

The answer of A gaseous compound,C,undergoes catalytic decomposition at an...

Question 6

A reaction is second order in NO and first order in O₂ has a rate constant,k = 1.4 × 10⁴ M^-2s^-1.What is the initial rate of reaction when the concentrations of NO and O₂ are 0.015 M and 0.030 M,respectively?

Accepted Answer

The answer of A reaction is second order in NO...

Question 7

For the reaction shown below,the rate of reaction of Br^-is ________ times the rate of formation of Br₂ over the same time period. ClO₂^-(aq)+ 4 Br^-(aq)+ 4 H⁺(aq)→ Cl^-(aq)+ 2 Br₂(aq)+2 H₂O(l)

Accepted Answer

The answer of For the reaction shown below,the rate of...

Question 8

A reaction has the rate law Rate = k[NO]²[H₂].If the concentration of NO is reduced by 1/3,the rate of reaction will be ________ (increased,decreased)by ________.

Accepted Answer

The answer of A reaction has the rate law Rate...

Question 9

At 55° the decomposition of N₂O₅ is first order,having a rate constant,k = 1.7 × 10^-3 s^-1.If the initial concentration of N₂O₅ is 6.4 × 10^-3 M,the number of half-lives that are required for the N₂O₅ concentration to fall to 2.0 × 10^-⁴ M is ________,and the amount of time required is ________ minutes.

Accepted Answer

The answer of At 55° the decomposition of N₂O₅ is...

Question 10

The decomposition of hydrogen peroxide occurs according to the equation 2 H₂O₂(aq)→ 2 H₂O(l)+ O₂(g) A concentration-time study of this reaction produces a straight line when ln[H₂O₂] is plotted versus time.Therefore,this is a ________ order reaction.

Accepted Answer

The answer of The decomposition of hydrogen peroxide occurs according...

Question 11

Biological reactions are catalyzed by

Accepted Answer

Enzymes are specialized proteins that act as catalysts in biological reactions. They increase the rate of the reaction by lowering the activation energy needed for the reaction to occur. Sugars, fats, and water do not have catalytic properties.

Question 12

At 300°C decomposition of NO₂(g)occurs with a rate law: Rate = - k[NO₂]^x.If the initial rate of decomposition is 3.2 × 10^-5M/s when [NO₂]_o = 8.0 × 10^-3 M and the initial rate of decomposition is 8.0 × 10^-6M/s when [NO₂]_o = 4.0 × 10^-3 M,then the order of reaction with respect to NO₂,x = ________.

Accepted Answer

The answer of At 300°C decomposition of NO₂(g)occurs with a...

Question 13

The reaction below is first order in H₂ and one-half order in Br₂.The rate law for this reaction is ________. H₂(g)+ Br₂(g)→ 2 HBr(g)

Accepted Answer

The answer of The reaction below is first order in...

Question 14

A reaction has the rate law Rate = k[NO]²[H₂].If the concentration of NO is reduced by half and the concentration of H₂ is quadrupled,the rate of reaction will ________ (increase,decrease,not change).

Accepted Answer

The answer of A reaction has the rate law Rate...

Question 15

For the reaction shown below,if the rate of formation of Br₂ is 1.5 × 10^-6 M/s,over the same time period the rate of consumption of H⁺ is ________ M/s. ClO₂^-(aq)+ 4 Br^-(aq)+ 4 H⁺(aq)→ Cl^-(aq)+ 2 Br₂(aq)+2 H₂O(l)

Accepted Answer

The answer of For the reaction shown below,if the rate...

Question 16

A mechanism for a naturally occurring reaction that destroys ozone is: Step 1: O₃(g)+ HO(g)→ HO₂(g)+ O₂(g) Step 2: HO₂(g)+ O(g)→ HO(g)+ O₂(g) Which species is a catalyst and what type of catalysis is occurring?

Accepted Answer

HO is the catalyst in this mechanism as it appears in the first step as a reactant, but is regenerated in the second step as a product. This is an example of homogeneous catalysis, as the catalyst and reactants are all in the same phase (gaseous).

Question 17

The reaction shown below has the rate law: Rate = k[BrO₃^-][Br^-][H⁺]².The order of reaction with respect to H⁺ is ________ and the overall order is ________. BrO₃^-(aq)+ 5 Br^-(aq)+ 6 H⁺(aq)→ 3 Br₂(aq)+ 3 H₂O(l)

Accepted Answer

The answer of The reaction shown below has the rate...

Question 18

The decomposition of hydrogen peroxide is given by the following reaction: 2 H₂O₂(aq)→ 2 H₂O(l)+ O₂(g) In the presence of KI the reaction is thought to occur by the following mechanism: Step 1: H₂O₂ + I^- → H₂O + IO^- Step 2: IO^- + H₂O₂ → H₂O + O₂ + I^- What is the role of I^- in this mechanism?

Accepted Answer

I^- acts as a catalyst because it is consumed in step 1 and regenerated in step 2, thus not being consumed overall in the reaction.

Question 19

An aqueous reaction occurs by a two-step mechanism,shown below. Step 1: A₂X₂ + Y → A₂X + XY Step 2: A₂X₂ + XY → A₂X + X₂ + Y What is the catalyst in this reaction?

Accepted Answer

A catalyst is a substance that is consumed and then regenerated in the reaction mechanism. In this mechanism, Y is consumed in Step 1 and regenerated in Step 2, making it the catalyst.

Question 20

The reaction below is second order in ClO₂ and first order in OH^-.If the rate is expressed in M/s,the rate constant,k,has the units ________. 2 ClO₂(aq)+ 2 OH^-(aq)→ ClO₃^-(aq)+ ClO₂^-(aq)+ H₂O(l)

Accepted Answer

The answer of The reaction below is second order in...

Quiz 13: Chemical Kinetics

The Haber process is the synthesis of ammonia gas from hydrogen and nitrogen on a hot metal surface.What is the catalyst and what type of catalysis is occurring?

A catalyst increases the rate of a reaction by providing a different reaction pathway that

For the reaction shown below,if the rate of formation of O₂ is 6.5 × 10^-6M/s,the rate of decomposition of N₂O₅ over the same time interval is ________. 2 N₂O₅(g)→ 4 NO₂(g)+ O₂(g)

A gaseous compound,C,undergoes catalytic decomposition at an initial rate of 0.45 M/s when [C]_o = 3.0 × 10^-3 M and 0.45 M/s when [C]_o = 9.0 × 10^-3 M.Therefore,this is a ________ order reaction.

A reaction is second order in NO and first order in O₂ has a rate constant,k = 1.4 × 10⁴ M^-2s^-1.What is the initial rate of reaction when the concentrations of NO and O₂ are 0.015 M and 0.030 M,respectively?

For the reaction shown below,the rate of reaction of Br^-is ________ times the rate of formation of Br₂ over the same time period. ClO₂^-(aq)+ 4 Br^-(aq)+ 4 H⁺(aq)→ Cl^-(aq)+ 2 Br₂(aq)+2 H₂O(l)

A reaction has the rate law Rate = k[NO]²[H₂].If the concentration of NO is reduced by 1/3,the rate of reaction will be (increased,decreased)by .

The decomposition of hydrogen peroxide occurs according to the equation 2 H₂O₂(aq)→ 2 H₂O(l)+ O₂(g) A concentration-time study of this reaction produces a straight line when ln[H₂O₂] is plotted versus time.Therefore,this is a ________ order reaction.

Biological reactions are catalyzed by

The reaction below is first order in H₂ and one-half order in Br₂.The rate law for this reaction is ________. H₂(g)+ Br₂(g)→ 2 HBr(g)

A reaction has the rate law Rate = k[NO]²[H₂].If the concentration of NO is reduced by half and the concentration of H₂ is quadrupled,the rate of reaction will ________ (increase,decrease,not change).

For the reaction shown below,if the rate of formation of Br₂ is 1.5 × 10^-6 M/s,over the same time period the rate of consumption of H⁺ is ________ M/s. ClO₂^-(aq)+ 4 Br^-(aq)+ 4 H⁺(aq)→ Cl^-(aq)+ 2 Br₂(aq)+2 H₂O(l)

A mechanism for a naturally occurring reaction that destroys ozone is: Step 1: O₃(g) + HO(g) → HO₂(g) + O₂(g) Step 2: HO₂(g) + O(g) → HO(g) + O₂(g) Which species is a catalyst and what type of catalysis is occurring?

The reaction shown below has the rate law: Rate = k[BrO₃^-][Br^-][H⁺]².The order of reaction with respect to H⁺ is and the overall order is . BrO₃^-(aq)+ 5 Br^-(aq)+ 6 H⁺(aq)→ 3 Br₂(aq)+ 3 H₂O(l)

An aqueous reaction occurs by a two-step mechanism,shown below. Step 1: A₂X₂ + Y → A₂X + XY Step 2: A₂X₂ + XY → A₂X + X₂ + Y What is the catalyst in this reaction?

The reaction below is second order in ClO₂ and first order in OH^-.If the rate is expressed in M/s,the rate constant,k,has the units ________. 2 ClO₂(aq)+ 2 OH^-(aq)→ ClO₃^-(aq)+ ClO₂^-(aq)+ H₂O(l)

Quiz 13: Chemical Kinetics

The Haber process is the synthesis of ammonia gas from hydrogen and nitrogen on a hot metal surface.What is the catalyst and what type of catalysis is occurring?

The reaction below is second order in ClO2 and first order in OH-.When the concentration of ClO2 is 0.020 M and the concentration of OH- is 0.10 M,the initial rate of reaction is 8.00 × 10-4 M/s.What is the rate constant,k,for this reaction? 2 ClO2(aq)+ 2 OH-(aq)→ ClO3-(aq)+ ClO2-(aq)+ H2O(l)

A catalyst increases the rate of a reaction by providing a different reaction pathway that

For the reaction shown below,if the rate of formation of O2 is 6.5 × 10-6 M/s,the rate of decomposition of N2O5 over the same time interval is ________. 2 N2O5(g)→ 4 NO2(g)+ O2(g)

A gaseous compound,C,undergoes catalytic decomposition at an initial rate of 0.45 M/s when [C]o = 3.0 × 10-3 M and 0.45 M/s when [C]o = 9.0 × 10-3 M.Therefore,this is a ________ order reaction.

A reaction is second order in NO and first order in O2 has a rate constant,k = 1.4 × 104 M-2s-1.What is the initial rate of reaction when the concentrations of NO and O2 are 0.015 M and 0.030 M,respectively?

For the reaction shown below,the rate of reaction of Br - is ________ times the rate of formation of Br2 over the same time period. ClO2-(aq)+ 4 Br-(aq)+ 4 H+(aq)→ Cl-(aq)+ 2 Br2(aq)+2 H2O(l)

A reaction has the rate law Rate = k[NO]2[H2].If the concentration of NO is reduced by 1/3,the rate of reaction will be ________ (increased,decreased)by ________.

The decomposition of hydrogen peroxide occurs according to the equation 2 H2O2(aq)→ 2 H2O(l)+ O2(g) A concentration-time study of this reaction produces a straight line when ln[H2O2] is plotted versus time.Therefore,this is a ________ order reaction.

Biological reactions are catalyzed by

The reaction below is first order in H2 and one-half order in Br2.The rate law for this reaction is ________. H2(g)+ Br2(g)→ 2 HBr(g)

A reaction has the rate law Rate = k[NO]2[H2].If the concentration of NO is reduced by half and the concentration of H2 is quadrupled,the rate of reaction will ________ (increase,decrease,not change).

For the reaction shown below,if the rate of formation of Br2 is 1.5 × 10-6 M/s,over the same time period the rate of consumption of H+ is ________ M/s. ClO2-(aq)+ 4 Br-(aq)+ 4 H+(aq)→ Cl-(aq)+ 2 Br2(aq)+2 H2O(l)

A mechanism for a naturally occurring reaction that destroys ozone is: Step 1: O3(g) + HO(g) → HO2(g) + O2(g) Step 2: HO2(g) + O(g) → HO(g) + O2(g) Which species is a catalyst and what type of catalysis is occurring?

The reaction shown below has the rate law: Rate = k[BrO3-][Br-][H+]2.The order of reaction with respect to H+ is ________ and the overall order is ________. BrO3-(aq)+ 5 Br-(aq)+ 6 H+(aq)→ 3 Br2(aq)+ 3 H2O(l)

An aqueous reaction occurs by a two-step mechanism,shown below. Step 1: A2X2 + Y → A2X + XY Step 2: A2X2 + XY → A2X + X2 + Y What is the catalyst in this reaction?

The reaction below is second order in ClO2 and first order in OH-.If the rate is expressed in M/s,the rate constant,k,has the units ________. 2 ClO2(aq)+ 2 OH-(aq)→ ClO3-(aq)+ ClO2-(aq)+ H2O(l)

For the reaction shown below,if the rate of formation of O₂ is 6.5 × 10^-6M/s,the rate of decomposition of N₂O₅ over the same time interval is ________. 2 N₂O₅(g)→ 4 NO₂(g)+ O₂(g)

A gaseous compound,C,undergoes catalytic decomposition at an initial rate of 0.45 M/s when [C]_o = 3.0 × 10^-3 M and 0.45 M/s when [C]_o = 9.0 × 10^-3 M.Therefore,this is a ________ order reaction.

A reaction is second order in NO and first order in O₂ has a rate constant,k = 1.4 × 10⁴ M^-2s^-1.What is the initial rate of reaction when the concentrations of NO and O₂ are 0.015 M and 0.030 M,respectively?

For the reaction shown below,the rate of reaction of Br^-is ________ times the rate of formation of Br₂ over the same time period. ClO₂^-(aq)+ 4 Br^-(aq)+ 4 H⁺(aq)→ Cl^-(aq)+ 2 Br₂(aq)+2 H₂O(l)

A reaction has the rate law Rate = k[NO]²[H₂].If the concentration of NO is reduced by 1/3,the rate of reaction will be (increased,decreased)by .

The decomposition of hydrogen peroxide occurs according to the equation 2 H₂O₂(aq)→ 2 H₂O(l)+ O₂(g) A concentration-time study of this reaction produces a straight line when ln[H₂O₂] is plotted versus time.Therefore,this is a ________ order reaction.

The reaction below is first order in H₂ and one-half order in Br₂.The rate law for this reaction is ________. H₂(g)+ Br₂(g)→ 2 HBr(g)

A reaction has the rate law Rate = k[NO]²[H₂].If the concentration of NO is reduced by half and the concentration of H₂ is quadrupled,the rate of reaction will ________ (increase,decrease,not change).

For the reaction shown below,if the rate of formation of Br₂ is 1.5 × 10^-6 M/s,over the same time period the rate of consumption of H⁺ is ________ M/s. ClO₂^-(aq)+ 4 Br^-(aq)+ 4 H⁺(aq)→ Cl^-(aq)+ 2 Br₂(aq)+2 H₂O(l)

A mechanism for a naturally occurring reaction that destroys ozone is: Step 1: O₃(g) + HO(g) → HO₂(g) + O₂(g) Step 2: HO₂(g) + O(g) → HO(g) + O₂(g) Which species is a catalyst and what type of catalysis is occurring?

The reaction shown below has the rate law: Rate = k[BrO₃^-][Br^-][H⁺]².The order of reaction with respect to H⁺ is and the overall order is . BrO₃^-(aq)+ 5 Br^-(aq)+ 6 H⁺(aq)→ 3 Br₂(aq)+ 3 H₂O(l)

An aqueous reaction occurs by a two-step mechanism,shown below. Step 1: A₂X₂ + Y → A₂X + XY Step 2: A₂X₂ + XY → A₂X + X₂ + Y What is the catalyst in this reaction?

The reaction below is second order in ClO₂ and first order in OH^-.If the rate is expressed in M/s,the rate constant,k,has the units ________. 2 ClO₂(aq)+ 2 OH^-(aq)→ ClO₃^-(aq)+ ClO₂^-(aq)+ H₂O(l)