rates of reaction Flashcards

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1
Q

rate

A

change in a measurable quantity per unit time

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2
Q

what is an ineffective collision

A

not useful as it produces no product

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3
Q

what is an effective collision dependent on

A

correct orientation (right way around)
speed (sufficient kinetic energy equal to or greater than the activation energy of the reaction)

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4
Q

pressure relationship

A

pressure is inversely proportional to volume

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5
Q

pressure collision theory

A

-a higher pressure of gas,caused by the decreased volume of a container, results in a greater number of particles per unit volume
-this causes an increase in the number of collisions between reactant particles per unit time
-and therefore there is an increase in the number of effective collisions per unit time,
-an effective collision being one that has the correct orientation + sufficient kinetic energy (Ek >= Ea)
-This leads to a higher reaction rate

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6
Q

surface area

A

outside contact points of a chemical

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7
Q

surface area relationship

A

increased surface area, more particles exposed

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8
Q

surface area collision theory

A

-an increase in surface area means a greater number of surface particles are exposed to collisions
-this causes an increase in the no. of collisions between reactant particles per unit time,
-and therefore there is an increase in the no. of effective collisions per unit time,
-an effective collision being one that has the correct orientation and sufficient kinetic energy (Ek>=Ea)
-This leads to a higher reaction rate.

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9
Q

concentration relationships

A

c=n/V

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10
Q

increase concentration result

A

there is no increase in fraction of particles in the sample with sufficient kinetic energy, equal to or greater than activation energy
There is a bulk increase in the number of particles, and therefore an increase in the number of particles capable of having effective collisions

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11
Q

concentration collision theory

A

-An increased concentration of solution leads to a greater number of particles per unit volume( c=n/v)
-this causes an increase in the no. of collisions between reactant particles per unit time,
-and therefore there is an increase in the no. of effective collisions per unit time,
-an effective collision being one that has the correct orientation and sufficient kinetic energy (Ek>=Ea)
-This leads to a higher reaction rate.

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12
Q

catalyst

A

a substance that increases the rate of the reaction but remains unchanged at the end of the reaction

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13
Q

ways catalyst works

A

-lowers activation energy
-aids correct orientation and facilitates chance of reaction
-bonds to one of reactants, changes bonding- weakens forces w/in temporary transition state, making it easier for other reactant to bond, then catalyst removed

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14
Q

catalyst collision theory

A

-a catalyst offers a reaction pathway of lower activation energy
-there is thus a greater proportion of particles w sufficient kinetic energy to overcome the activation energy (refer to maxwell -boltzman distribution curve)
-and therefore there is an increase in the no. of effective collisions per unit time,
-an effective collision being one that has the correct orientation and sufficient kinetic energy (Ek>=Ea)
-This leads to a higher reaction rate.

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15
Q

temperature

A

measure of average kinetic energy of a substance

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16
Q

temperature relationship

A

Ek = 1/2mv^2

17
Q

effect of increased temp. on maxwell curve

A

peak decreases as bigger range of kinetic energies (increase in no. of particles w Ek>= Ea

18
Q

temperature collision theory

A

-A higher temperature means that particles move w/greater velocity and have a greater average kinetic energy
-the effect of this is 2-fold
-minor: there is an increase in the no. of collisions per unit time
-major- there is a greater proportion of particles w/ sufficient Ek to overcome Ea
-and therefore there is an increase in the no. of effective collisions per unit time,
-an effective collision being one that has the correct orientation and sufficient kinetic energy (Ek>=Ea)
-This leads to a higher reaction rate.

19
Q

reaction rate

A

the change in amount or concentration per unit time of either a reactant or product
directly proportional to no. of effective collisions per unit time

20
Q

molecular collision theory

A

3.2reactant particles must collide with or have sufficient kinetic energy for successful collision. only those collisions with sufficient potential and kinetic energy equivalent to that of the activated complex will be successful, allowing for
-enough energy to break bonds OR
-gain enough energy to form activated complex OR
-activated complex is at a higher energy and is unstable

21
Q

what factors affect the rate of chemical reactions

A

the nature of reacting substances, SA of a solid, concentration of a soln, pressure of gas, catalyst and temp.

22
Q

what is the collision theory

A

model that explains that a reaction will only proceed when reactant particles collide effectively

23
Q

reaction rate relationship

A

reaction rate is directly proportional to the no. of effective collisions per unit time

24
Q

reverse reaction

A

A reaction that proceeds from the products to the reactants (using the same balanced equation).