Increasing temperature of a chemical reaction:

increases the number of collisions per second of chemical reactants

increases the speed of reaction

can increase the pressure of reactants

A chemical reaction can occur:

if the particles collide with enough energy

if the particles collide with sufficient activation energy

if the particles collide with correct orientation

In a chemical reaction which goes forward:

typically some of the reactants go forward toward the products

typically all reactants go forward toward the products

typically all reactants have just the right amount of activation energy to go forward toward the products

typically all reactants have just the right orientation to go forward toward the products

The mechanism of a chemical reaction is the sequence of actual events that take place as reactant molecules are converted into products. Which of the following is true?

Each of these events constitutes an elementary step that can be represented as a coming-together of discrete particles ("collision").

Each of these events constitutes an elementary step that can be represented as the breaking-up of a molecule ("dissociation") into simpler units.

The molecular entity that emerges from each step may be a final product of the reaction, or it might be an intermediate.

Consider the decomposition of nitrogen dioxide into nitric oxide and oxygen. The net balanced equation is: 2N O 2 (g) →2N O(g) + O 2 (g) The mechanism of this reaction is believed to involve the following two elementary steps: 1st: 2NO 2 →NO 3 +NO 2nd: NO 3 →NO+ O 2

NO 3 has only a transient existence and does not appear in the net equation. It is an intermediate.

NO 3 has a permanent existence and does appear in the overall net equation.

NO 3 would appear at the highest point of an Time Vs. Energy Curve when graphed.

NO 3 is known as an activated complex or transition state.

A useful reaction mechanism consists of a series of elementary steps (defined below) that:

can be written as chemical equations, and whose sum gives the net balanced reaction equation.

must agree with the experimental rate law.

may be different under different conditions.

Elementary reactions differ from ordinary net chemical reactions. Which of the following statements is false?

Some net reactions do proceed in a single elementary step, at least under certain conditions. The presence of a catalyst however cannot enable an alternative mechanism that greatly speeds up the rate of a reaction.

A bimolecular process always follows the second-order rate law.

Elementary steps often involve unstable or reactive species that do not appear in the net reaction equation.

Net reactions may have different proposed elementary steps, and all are viable if they solve simultaneously to the overall net reaction, unless proved experimentally false.

Which type of elementary reaction is most common?

none of the above, they are all equally common

Multi-step (Consecutive) Reactions: Mechanisms in which one elementary step is followed by another are very common. step 1: A + B → Q step 2: B + Q → C net reaction: A + 2B → C Which of the following is false?

Intermediates such as Q can appear in the rate law of a net reaction.

The net reaction is just the sum of its elementary steps.

The species Q is an intermediate, usually an unstable or highly reactive species.

If both steps proceed at similar rates, rate law experiments on the net reaction would not reveal that two separate steps are involved here.The rate law for the reaction would be rate=k[A][B ]2

The rate-determining step is also known as the rate-limiting step. Consider a 3 elementary step proposed mechanism. 1st step: fast 2nd step: slow 3rd step: fast Which of the following is false?

The rate law for the overall net reaction must simply include concentration(s), reaction orders, and a rate constant for that rate-determining step.

We can generally expect that one of the elementary reactions in a sequence of consecutive steps will have a rate constant that is smaller than the others.

The effect is to slow the rates of all the reactions.

The overall rate law must include information from both the slow step and any step(s) before it.

A "zeroth" order reaction for A-->B, will show:

a straight line for a graph: time vs. [A].

a straight line for a graph: time vs. ln [A]

a straight line for a graph: time vs. 1/[A]

A zeroth order rate law for reaction A--> B will match a graph:

which is straight and negative in slope for time vs. [A].

which is straight and positive in slope for time vs. [A].

which is non-linear and positive in slope for time vs. [A].

which is non-linear and positive in slope for time vs. ln[A].

A first order rate law for reaction A--> B will match a graph:

which looks linear and negative in slope for time vs. ln [A].

which looks linear and positive in slope for time vs. ln [A].

which looks non-linear and positive in slope for time vs. ln [A].

which looks non-linear and negative in slope for time vs. ln [A].

A 2nd order rate law for reaction A--> B will match a graph:

which looks linear and positive in slope for time vs. 1/ [A].

which looks linear and negative in slope for time vs. 1/ [A].

which looks non-linear and positive in slope for time vs. 1/ [A].

which looks non-linear and negative in slope for time vs. 1/[A].

What is true of the half-life of a chemical reaction?

For a 1st order reaction, the half-life ("t1/2") is not dependent upon initial concentration.

Half-life is a good estimate of reaction rate.

Half-life helps us determine how long it takes for half of the starting concentration to change into product.

usually part of the slope in the slope-intercept equation form of a line

Given the following data for this reaction: NH 4 + (aq) + NO 2 - (aq) N 2 (g) + 2H 2 O( l ) on your sheet. The rate law for the reaction is:

(d) Rate = k[NH 4 + ][NO 2 - ] 2

(b) Rate = k[NH 4 + ] 2 [NO 2 - ] 2

(c) Rate = k[NH 4 + ] 2 [NO 2 - ]

Elements which are good catalysts and have ability to change their oxidation number or charge and their ability to bond to reactants effectively tend to be of what kind of element:

Transition elements from the middle of the Periodic Table

For a first order reaction: A--> B the slope intercept for of the equation y=mx + b can help us study the reaction rate. Which of the following is true?

Natural log of the initial concentration =y

Natural log of the final concentration is = to the y intercept "b"

How do you calculate the overall reaction order of a chemical reaction?

add up the reaction orders of all elementary steps including only the slow step and any earlier steps

add up the coefficients of the slow step of a reaction mechanism

take the largest concentration reactant's coefficient

add up all coefficients of all slow and fast steps in a proposed reaction mechanism

Which one of the following changes would alter the rate constant (k) for a chemical reaction?

A. increasing the concentration of A

B. increasing the concentration of B

D. measuring k again after the reaction has run for a while

The rate law for a reaction is rate = k [A][B]2 Which one of the following statements is false?

D) The reaction is second order overall.

A) If [B] is doubled, the reaction rate will increase by a factor of 4.

B) The reaction is second order in B.

C) The reaction is first order in A.

If the concentration of a reactant has zeroth order, it means:

there is no effect of the concentration change on the reaction rate

the multiple of the concentration change affects the reaction rate by the same multiple

the multiple of the concentration change affects the reaction rate by a multiple of 2

the multiple of the concentration change affects the reaction rate by a multiple of 4

Activation energy when graphed can be calculated by:

finding the difference in energy between the reactants and the transition state

finding the energy between the transition state and the products

finding the difference in energy between the reactants and products

In an energy profile of: Time Vs. Energy , where are the intermediates found?

at the bottom of the valleys of the curve(s)

at the far left start of the curve

at the top of the hill of the curve(s)

For the elementary reaction NO 3 + CO -> NO 2 + CO 2 the molecularity of the reaction is _______, and the rate law is rate = _______.

A) 4, k[NO 3 ][CO][NO 2 ][CO 2 ]

C) 4, k[NO 2 ][CO 2 ]/[NO 3 ][CO]

Generally speaking, graphs of reaction rates for 1st order reactions, are steeper when:

the slope of the curve is higher

How do we find the instantaneous reaction rate?

draw a tangent line to the reaction rate curve and find the slope

take two plots on the rate curve and find the slope

find a point on the curve and estimate the slope

The rate law of the overall reaction A + B--> C is rate = k[A] 2 . Which of the following will not increase the rate of the reaction?

C) increasing the concentration of reactant B

A) increasing the concentration of reactant A

B) increasing the temperature of the reaction

D) adding a catalyst for the reaction

A fluctuating 3 hill curve energy profile will be provided. Which is the fastest forward reaction?

More than one of the curves has the fastest forward rate.

Kinetics: AP Chemistry

11th Grade - University

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72 Qs

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Kinetics: AP Chemistry

Quiz

•

Chemistry

•

11th Grade - University

•

Practice Problem

•

Hard

•

NGSS

HS-PS1-5, HS-PS1-4, HS-PS1-7

Standards-aligned

George Miles

Used 41+ times

FREE Resource

72 questions

Show all answers

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

What does kinetics mainly study?

concentration of (aq) mixtures

pressure of (g) mixtures

how much products are produced

reaction rates

Tags

NGSS.HS-PS1-5

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

Which factors significantly affect reaction rate?

temperature

presence of a catalyst

amount of chemical

all of the above and other factors

Tags

NGSS.HS-PS1-5

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

A catalyst:

appears in the reactants of an early elementary step of a proposed reaction mechanism

appears in the products of the last proposed reaction mechanism

can affect reaction rate, but is not used up in a chemical reaction

all of the above

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

A catalyst:

cannot infinitely increase reaction rate

helps reactants fit better together

must both bond reactants, and eventually be released from chemicals

all of the above

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

A catalyst:

increases activation energy of a chemical reaction

decreases activation energy of a chemical reaction

cannot be destroyed with high temperatures

all of the above

Tags

NGSS.HS-PS1-5

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

A catalyst:

is more efficient if it is homogeneous

is more efficient if its state matches that of the substrate reactants it originally bonds to

is more efficient if it is heterogeneous

all of the above

MULTIPLE CHOICE QUESTION

1 min • 1 pt

A catalyst:

should be eliminated when we solve elementary reaction steps of a proposed reaction mechanism simultaneously

should always be introduced and eliminated in the first elementary step of a proposed reaction mechanism

lowers the amount of energy released by an exothermic reaction

lowers the amount of energy added to a reaction

Tags

NGSS.HS-PS1-4

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Kinetics: AP Chemistry

72 questions

What does kinetics mainly study?

Which factors significantly affect reaction rate?

A catalyst:

A catalyst:

A catalyst:

A catalyst:

A catalyst:

Increasing temperature of a chemical reaction:

Many kinetics equations fit a slope intercept form. The Arrhenius equation is k = A e−(Ea/RT). The slope of a plot of ln k vs. 1/T is equal to:

What is the slope of an Arrhenius plot for the following reaction? 2NOCl → 2NO + Cl2
Temperature (K) k (L/mol·s) 400. 6.6 × 10−4 500. 2.9 × 10−1 600. 16.3

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Similar Resources on Wayground

Popular Resources on Wayground

Discover more resources for Chemistry

Kinetics: AP Chemistry

72 questions

What does kinetics mainly study?

Which factors significantly affect reaction rate?

A catalyst:

A catalyst:

A catalyst:

A catalyst:

A catalyst:

Increasing temperature of a chemical reaction:

Many kinetics equations fit a slope intercept form. The Arrhenius equation is k = A e−(Ea/RT). The slope of a plot of ln k vs. 1/T is equal to:

What is the slope of an Arrhenius plot for the following reaction? 2NOCl → 2NO + Cl2 Temperature (K) k (L/mol·s) 400. 6.6 × 10−4 500. 2.9 × 10−1 600. 16.3

Create a free account and access millions of resources

Similar Resources on Wayground

Popular Resources on Wayground

Discover more resources for Chemistry

What is the slope of an Arrhenius plot for the following reaction? 2NOCl → 2NO + Cl2
Temperature (K) k (L/mol·s) 400. 6.6 × 10−4 500. 2.9 × 10−1 600. 16.3