an animal that relies on external sources to regulate its body temperature

an animal that generates its own heat internally

an animal that lives only in water

an animal that migrates seasonally

Temperature increases the rate of reaction in lizards.

Temperature decreases the rate of reaction in lizards.

Temperature has no effect on the rate of reaction in lizards.

Rate of reaction is independent of temperature in lizards.

using enzymes

producing more blood

increasing body temperature

releasing hormones only

A fast reaction rate means the reaction happens quickly, while a slow reaction rate means the reaction happens slowly.

A fast reaction rate means the reaction happens slowly, while a slow reaction rate means the reaction happens quickly.

Both fast and slow reaction rates mean the reaction happens at the same speed.

Reaction rate does not affect how quickly a reaction occurs.

Always positive for both

Negative for reactants and positive for products

Positive for reactants and negative for products

Always negative for both

Rates for reactants are negative, while for products they are positive.

Rates for both are always positive.

Rates for both are always negative.

Rates for reactants are positive, while for products they are negative.

The rate of reaction at a specific moment in time

The average rate over a period of time

The total amount of product formed

The time taken for a reaction to complete

A method to measure concentration changes over time

A catalyst for the reaction

A high temperature

A large volume of reactants

Titration, colorimetry, gas collection, and mass measurement

Filtration, distillation, and crystallization

Centrifugation, chromatography, and decantation

Evaporation, sublimation, and extraction

$$rate = k[A]^n$$

rate = k[A] + n

rate = $$k + [A]^n$$

$$rate = n[A]^k$$

The sum of the powers of the concentration terms in the rate law

The number of reactant molecules

The rate constant of the reaction

The activation energy of the reaction

Order: Zero, Dependence: None (rate is independent of concentration)

Order: First, Dependence: Directly proportional to concentration

Order: Second, Dependence: Proportional to the square of concentration

Order: Third, Dependence: Proportional to the cube of concentration

Order: First, Dependence: Linear (rate is directly proportional to concentration)

Order: Second, Dependence: Quadratic (rate is proportional to the square of concentration)

Order: Zero, Dependence: Independent (rate does not depend on concentration)

Order: Third, Dependence: Cubic (rate is proportional to the cube of concentration)

Order: Second, Dependence: Quadratic (rate is proportional to the square of concentration)

Order: First, Dependence: Linear (rate is proportional to concentration)

Order: Zero, Dependence: Constant (rate is independent of concentration)

Order: Third, Dependence: Cubic (rate is proportional to the cube of concentration)

A straight line when concentration is plotted against time

A curve when concentration is plotted against time

A straight line when rate is plotted against concentration

A curve when rate is plotted against concentration

Photochemical decomposition of HI because rate is independent of concentration

Decomposition of N2O5 because rate is independent of temperature

Hydrogenation of ethene because rate is independent of catalyst

Decomposition of ammonia because rate is independent of pressure

A straight line when plotting concentration vs. time

A straight line when plotting rate vs. concentration

A straight line when plotting log(concentration) vs. time

A curve when plotting log(concentration) vs. time

A straight line when 1/[A] is plotted against time

A straight line when [A] is plotted against time

A straight line when ln[A] is plotted against time

A straight line when [A]^2 is plotted against time

A mathematical equation relating the rate of a reaction to the concentration of reactants

A description of the color change during a reaction

A list of products formed in a reaction

A method for separating mixtures

Reactions whose rate is independent of the concentration of reactants

Reactions whose rate depends on the concentration of reactants

Reactions that occur only at high temperatures

Reactions that require a catalyst

Reactions whose rate depends linearly on the concentration of one reactant

Reactions whose rate depends on the square of the concentration of one reactant

Reactions that do not depend on reactant concentration

Reactions that occur in two steps

Reactions whose rate depends on the concentration of two reactants or the square of the concentration of one reactant.

Reactions that proceed in a single step.

Reactions that do not depend on reactant concentration.

Reactions that occur only in the presence of a catalyst.

Measuring the rate of reaction at different concentrations

Measuring the temperature change

Observing color change only

Measuring the mass of the reactants

mol L^-1 s^-1

s^-1

L mol^-1 s^-1

mol^-1 L s^-1

The rate remains constant as the concentration changes

The rate increases with concentration

The rate decreases with concentration

The rate doubles when concentration doubles

mol^1-n L^n-1 s^-1

mol^n-1 L^1-n s^-1

molⁿ L^-n s^-1

mol^1-n Lⁿ s^-1

The sum of the exponents of the reactants in the rate law

The sum of the coefficients in the balanced equation

The number of products formed

The temperature of the reaction

True

False

The mechanism of the reaction

The rate of the reaction under given conditions

The equilibrium constant

The enthalpy change of the reaction

the relationship between concentration and time for a chemical reaction

the energy change during a reaction

the mechanism of a reaction

the equilibrium constant of a reaction

ln([A]) = -kt + ln([A]₀)

[A] = [A]₀ - kt

1/[A] = kt + 1/[A]₀

$$[A] = [A]₀e^{(kt)}$$

A plot of ln[A] versus time yields a straight line.

A plot of [A] versus time yields a straight line.

A plot of 1/[A] versus time yields a straight line.

A plot of [A]^2 versus time yields a straight line.

$$\frac{1}{[A]} = kt + \frac{1}{[A]_0}$$ , where [A] is concentration (mol/L), k is the rate constant (L/(mol·s)), t is time (s), and [A]_0 is initial concentration (mol/L).

$$[A] = [A]_0 e^{-kt}$$ , where [A] is concentration (mol/L), k is the rate constant (s^{-1}), t is time (s), and [A]_0 is initial concentration (mol/L).

$$\ln [A] = -kt + \ln [A]_0$$ , where [A] is concentration (mol/L), k is the rate constant (s^{-1}), t is time (s), and [A]_0 is initial concentration (mol/L).

\( [A] = [A]_0 - kt \), where [A] is concentration (mol/L), k is the rate constant (mol/(L·s)), t is time (s), and [A]_0 is initial concentration (mol/L).

A plot of 1/[A] vs. time gives a straight line

A plot of ln[A] vs. time gives a straight line

A plot of [A] vs. time gives a straight line

A plot of [A]^2 vs. time gives a straight line

[A] = [A]₀ - kt, where [A] is concentration (mol/L), k is rate constant (mol/L·s), t is time (s), [A]₀ is initial concentration (mol/L)

[A] = $$[A]₀e^{-kt}$$ , where [A] is concentration (mol/L), k is rate constant (s⁻¹), t is time (s), [A]₀ is initial concentration (mol/L)

ln[A] = ln[A]₀ - kt, where [A] is concentration (mol/L), k is rate constant (s⁻¹), t is time (s), [A]₀ is initial concentration (mol/L)

1/[A] = 1/[A]₀ + kt, where [A] is concentration (mol/L), k is rate constant (L/mol·s), t is time (s), [A]₀ is initial concentration (mol/L)

A plot of [A] vs. time is linear with a negative slope.

A plot of ln[A] vs. time is linear with a negative slope.

A plot of 1/[A] vs. time is linear with a positive slope.

A plot of [A] vs. time is exponential.

The time required for the concentration of a reactant to decrease by half

The time required for the reaction to complete

The time required for the product to double

The time required for equilibrium to be reached

It is independent of the rate constant.

It is directly proportional to the initial concentration.

It is inversely proportional to the rate constant.

It is equal to the rate constant.

t_1/2 = 0.693/k

t_1/2 = k/0.693

t_1/2 = 2k

t_1/2 = 0.5k

Directly proportional to the initial concentration

Inversely proportional to the initial concentration

Independent of the initial concentration

Equal to the rate constant

t_1/2 = 0.693/k

t_1/2 = 1/(k[A]₀)

t_1/2 = 1/(k[A]₀)

t_1/2 = [A]₀/k

t₁/₂ = [A]₀/2k

t₁/₂ = 0.693/k

t₁/₂ = 1/k[A]₀

t₁/₂ = k/[A]₀

t_1/2 = [A]₀ / 2k, where t_1/2 is half-life (s), [A]₀ is initial concentration (mol/L), and k is rate constant (mol/L·s^-1)

t_1/2 = 0.693 / k, where t_1/2 is half-life (s) and k is rate constant (s^-1)

t_1/2 = 1 / k, where t_1/2 is half-life (s) and k is rate constant (s^-1)

t_1/2 = k / [A]₀, where t_1/2 is half-life (s), [A]₀ is initial concentration (mol/L), and k is rate constant (mol/L·s^-1)

The rate law expresses the rate as a function of reactant concentrations, and the reaction order is the sum of the exponents of these concentrations.

The rate law is independent of reactant concentrations, and reaction order is always one.

The rate law only applies to equilibrium reactions, and reaction order is determined by the products.

The rate law is determined by temperature alone, and reaction order is unrelated to concentration.

k = $$A e^{-Ea/RT}$$ , where k is the rate constant (s⁻¹), A is the frequency factor (s⁻¹), Ea is activation energy (J/mol), R is the gas constant (J/(mol·K)), and T is temperature (K).

k = $$A e^{Ea/RT}$$ , where k is the rate constant (mol/L·s), A is the frequency factor (mol/L·s), Ea is activation energy (kJ/mol), R is the gas constant (kJ/(mol·K)), and T is temperature (°C).

$$k = A e^{-RT/Ea}$$ , where k is the rate constant (L/mol·s), A is the frequency factor (L/mol·s), Ea is activation energy (J), R is the gas constant (J/K), and T is temperature (K).

k = $$A e^{-Ea/RT}$$ , where k is the rate constant (mol/L), A is the frequency factor (mol/L), Ea is activation energy (cal/mol), R is the gas constant (cal/(mol·K)), and T is temperature (°C).

Relating the rate constant to temperature exponentially

Showing a linear relationship between rate and temperature

Indicating no effect of temperature on rate

Relating rate to pressure changes

The Arrhenius Plot is a graphical representation of the Arrhenius equation, plotting ln(k) versus 1/T.

The Arrhenius Plot shows the relationship between pressure and temperature.

The Arrhenius equation is used only for exothermic reactions, while the Arrhenius Plot is for endothermic reactions.

The Arrhenius Plot is unrelated to the Arrhenius equation.

A temporary, unstable arrangement of atoms formed during a chemical reaction

The final product of a chemical reaction

A stable intermediate compound

The initial reactant molecules

The minimum energy required to start a chemical reaction.

The energy released during a reaction.

The energy stored in reactants.

The energy lost as heat.

Higher activation energy increases reaction rate.

Lower activation energy increases reaction rate.

Activation energy does not affect reaction rate.

Activation energy only affects equilibrium.

A constant that indicates the frequency of collisions in a chemical reaction

The energy required to start a reaction

The rate at which products are formed

A measure of temperature change

A constant value in a reaction rate equation

A term that represents the fraction of molecules with enough energy to react

The total energy of the system

The temperature at which a reaction occurs

Higher temperature increases reaction rate.

Higher temperature decreases reaction rate.

Temperature has no effect on reaction rate.

Reaction rate is independent of temperature.

The mechanism of the reaction

The color of the reactants

The taste of the products

The boiling point of the solvent

ln(rate constant) vs 1/Temperature

rate constant vs Temperature

activation energy vs rate constant

Temperature vs activation energy

Arrhenius equation

Boyle's law

Charles's law

Dalton's law

F = ma, where F is force (N), m is mass (kg), a is acceleration (m/s²)

F = mv, where F is force (N), m is mass (kg), v is velocity (m/s)

F = m/a, where F is force (N), m is mass (kg), a is acceleration (m/s²)

F = a/m, where F is force (N), a is acceleration (m/s²), m is mass (kg)

the behavior of gases based on the motion and collisions of particles

the structure of atomic nuclei

the process of chemical bonding

the arrangement of electrons in atoms

Orientation factor and collision frequency

Activation energy and temperature

Molecular mass and velocity

Pressure and volume

The number of collisions per unit time per unit volume

The speed of a single molecule

The total energy of all molecules

The distance between two collisions

A measure of how often molecules collide in the correct orientation for a reaction to occur

The energy required to start a chemical reaction

The speed at which reactants are converted to products

A type of catalyst used in chemical reactions

Equations

Paragraphs

Lists

Tables

The overall change in energy during a reaction

The step-by-step sequence of elementary reactions by which overall chemical change occurs

The rate at which a reaction proceeds

The products formed in a chemical reaction

A single step in a reaction mechanism that describes a specific molecular event.

A process that always involves catalysts.

A reaction that occurs in multiple stages.

A step that does not involve any reactants.

A substance formed during a reaction that is not the final product

The starting material of a reaction

A catalyst used in the reaction

The solvent used in the reaction

Mechanism shows stepwise process, overall reaction shows only reactants and products

Both are the same

Overall reaction shows intermediates, mechanism does not

Mechanism ignores the order of steps

the number of molecules that participate as reactants in an elementary reaction

the speed at which a reaction occurs

the energy required to start a reaction

the total number of products formed in a reaction

One

Two

Three

Four

One

Two

Three

Four

The slowest step in a reaction mechanism

The fastest step in a reaction mechanism

The step with the highest concentration of reactants

The step that produces the most products

It satisfies the required motion and force conditions.

It is aesthetically pleasing.

It is made of expensive materials.

It is easy to manufacture.

The rate law always depends on the first step, regardless of its speed.

The rate law for a slow initial step is based on that step, while for a fast initial step, it depends on the next slow step.

The rate law is independent of the reaction mechanism.

The rate law is always determined by the fastest step.

A substance that increases the rate of a chemical reaction without being consumed

A reactant that is used up in a chemical reaction

A product formed at the end of a reaction

A substance that slows down a chemical reaction

Filtering out dust particles from exhaust gases

Converting harmful gases into less harmful substances

Increasing the engine's power output

Reducing the temperature of exhaust gases

A catalyst that exists in the same phase as the reactants

A catalyst that exists in a different phase than the reactants

A catalyst that is always solid

A catalyst that is always liquid

A catalyst that is in a different phase than the reactants.

A catalyst that is in the same phase as the reactants.

A catalyst that increases the activation energy of a reaction.

A catalyst that is consumed during the reaction.

Greenhouse gases

CFCs and other pollutants

Excess oxygen

Global warming

Addition of hydrogen to alkenes in the presence of a catalyst

Removal of hydrogen from alkenes

Addition of oxygen to alkenes

Polymerization of alkenes