Rate of Reactions Flashcards

1
Q

What is a reaction’s rate?

A

The change in concentration per second.

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2
Q

whats the equation for rate?

A

rate = change in concentration / time
Rate = k[A]^x x [B]^y

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3
Q

What is rate measured in?

A

Mol dm^-3 s^-1

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4
Q

what does zero order mean?

A

rate ∝ [A]°

rate is NOT affected by concentration

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5
Q

what does first order mean?

A

rate ∝ [A]¹
rate changes by the same factor as concentration
so if concentration doubles as does rate

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6
Q

what does second order mean?

A

rate ∝ [A]²
rate changes by the factor concentration does squared
if [A] doubles rate quadruples

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7
Q

In a chemical reaction, if A is zero order, what effect would be seen if [A] is doubled?

A

Reaction rate would not change.

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8
Q

In a chemical reaction, if A is first order, what effect would be seen if [A] is doubled?

A

Reaction rate would double.

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9
Q

In a chemical reaction, if A is second order, what effect would be seen if [A] is doubled?

A

Reaction rate would quadruple.

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10
Q

what is the overall order?

A

if two reactants A and B with orders m and n

the overall order = m+n

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11
Q

How is the reaction rate at a specific time worked out using a concentration against time graph?

A

At the set time, draw a tangent to the curve and measure the gradient to get the rate.

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12
Q

If there are two reactants, A and B, what would be the rate equation?

A

rate = k x [A]^m x [B]^n
k - rate constant
m - order of A
n - order of B

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13
Q

What is initial rate?

A

The instantaneous rate at the beginning of an experiment when t=0.

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14
Q

what does a zero order and first order concentration time graphs look like?

A

0 order = Straight line angled down
1st order = Curved line down

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15
Q

what is a half life?

A

a half life of a reactant is the time take for its concentration to decrease by half.

a first order reaction has a constant half life

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16
Q

What are the two ways of continuous monitoring when a gas is produced?

A

the two ways of monitoring are
Gas collection
Mass loss

17
Q

What is a way of utilising light to monitor rate?

A

Using a colourimeter.

Measuring the amount of light absorbed by a solution.

18
Q

What is half life?

A

The time taken for half of a reactant to be used up.

19
Q

In a concentration time graph, how can you deduce whether the reactant is first or second order?

A

Measure multiple half lives.
If the half life is constant, it is first order.
If the half life is increasing, it is second order.

20
Q

If the rate is only affected by one reactant, which is first order, what is another way of determining the rate constant?

A

k = ln|2| / t(1/2)

21
Q

What is a reaction mechanism?

A

A series of steps that, together, make up the overall reaction.

22
Q

What is the rate determining step?

A

The slowest step in the reaction mechanism of a multi-step reaction.

23
Q

Why does temperature affect the rate constant?

A

Increasing the temperature, increases rate of reaction and thus rate constant.

24
Q

the Arrhenius equation is found on the data sheet what do the symbols stand for?
k = A x e^(-E(a)/RT)

A

k = A x e^(-E(a)/RT)
A - pre exponential factor
-E(a)/RT - exponential factor
R=gas constant= 8.314
T= temp in kelvin
ea=activation energy (jmol^-1)

25
Q

What is the logarithmic form of the Arrhenius equation?

A

ln|k| = -E(a)/RT + ln|A|

26
Q

What can the log form of the Arrhenius equation be modelled as?

A

A straight line graph in y=mx + c
ln|k|=-E(a)/R 1/T +ln|A|
Y= m X + c

ln[A] is the y intercept and -E(a)/RT ia the gradient

27
Q

what does the rate concentration graphs of zero, first and second order look like? explain there shapes

A

zero order
rate∝ [A]^0 therefore rate= constant (flat graph)

first order
rate∝[A]¹ so a linear shape upwards

second order
rate∝[A]² so curve upwards