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Chem 203 > Gasses > Flashcards

Gasses Flashcards

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1
Q

What is the equation for partial pressure

A

Pa=XaPtot

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2
Q

Assumptions four for ideal gas

A

Consist of many particles moving through space randomly and colliding with each other

Gas particle very small compare to distances between them

Interactions are relatively weak between them

Avg KE depend only on temp

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3
Q

What is zero point motion

A

When temp is 0 K, not all motion stops

There’s still motion called zero point motion

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4
Q

What is compressed factor

A

Compares the gases molar volume to ideal volume

=molar V of gas/molar V of ideal gas

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5
Q

Non Ideal bass assumption

A

Gases move randomly and collide

Avg kinetic NRG of gas particles depends of temp

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6
Q

What does the rate of reaction depend on

5 things

A
  1. the nature of the reactants ionic, covalent, size, bond strengths
  2. Physical form: homo, hetero, solid. liquid, gas
  3. reactant concentrations: higher= more collisions
  4. temp: more collisions = more energy and faster rxn
  5. catalysts
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7
Q

What is the reaction mechanism

A

Sequence of molecular events that turns reactants into products

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8
Q

What is the reaction rate

A

Change on concentration of reactants per unit time

Rate= []/t

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9
Q

What is rate of disappearance

Rate appearance

A

The avg rate of the thing being used up:
2H2
Rate = -1/2[H2]/t

Avg rate of thing appearing
3HCL
Rate=1/3[HCL]/t

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10
Q

What does the rate law tell us

A

Extent of concentrations affect on the reaction

Tells us what species affects which reaction

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11
Q

Equations of intial rates to find rate order for species

A

Log (rate1/rate2)
____________________
Log ([A1]/[A2])

Only works if all concentration except A ARE constant

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12
Q

Why do we use the integrated rate law equations?

A

To predict concentrations of reactant of product at and given time

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13
Q

What is the half life of a species defined as

A

Time it takes for half staring material to be consumed

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14
Q

What happens to the half life at each order?

A

0: decreases
1: constant
2: increases

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15
Q

What is the other form of the 1st order integrated rate law

A

[A]t= [A]0•e^-kt

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16
Q

What happens to rate law if we have one reactant a lot bigger than other

A

The change in B as reaction occurs is very small (negligible)

So We can assume [B] is constant

So rate law is just rate = k[A]

This is called pseudo first order

17
Q

What does the Arrhenius equation tell us

A

How the rate constant changes with temp

18
Q

What is A and Ea in the Arrhenius equation

A

A= frequency factor constant (find mathematically)

Ea= activation energy

19
Q

What is the first method in finding A and Ea

The second?

A

Two point method

Graphical method

20
Q

What is the slope in the graphical method Arrhenius equation

The intercept?

A

-Ea/R

Ln A

21
Q

What are the condition that must be met for a reaction to occur according to collision theory

A

Reacting molecules must collide
Colliding molecules must have sufficient energy
Colliding molecules must have correct orientation

Also assume that reactants come together to form and intermediate called transition state

22
Q

What does the probability of a reaction depend on

A

Number of collisions

Geometric factors (orientation of molecules)

Energy of collisions

23
Q

What is the reaction of enthaoly is positive

A

Endo

24
Q

What is the reaction if enthaoly negative

A

Exothermic

25
Q

If reaction is endothermic where are the reactant on the graph

A

Below products

26
Q

If reaction is exothermic where are the reactant on the graph

A

Above products

27
Q

Units of activation energy

A

J/mol convert to kj/mol

28
Q

Wait is amontons law

A

P1/T1 = P2/T2
Pressure proportional to T
Volume is kept constant

29
Q

What is Charles law

A

V1/T1 = V2/T2

Volume proportionally to T
Pressure kept constant

30
Q

What is boyles law

A

P1V1=P2V2

Pressure is inversely proportional to volume

31
Q

What is the combined gas law

A

P1V1/T1=P2V2/T2

32
Q

What is avogardros law

A

V1/n1=V2/n2
V is proportional to n
Pressure and temp are constant

Chem 203 (6 decks)

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