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CH 302 > Unit 1 > Flashcards

Unit 1 Flashcards

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1
Q

Same molec
Same T
Different V
VP?

A

Same VP

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2
Q

Same molec
Diff Temp
VP?

A

Higher temp -> higher KE -> more molec in gas phase -> higher VP

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3
Q

Which molecule would you expect to have a lower H(l) at room temperature?
A. H2CO
B. CH3OH

A

Lower H(l) -> most stable -> the one with H bonding
Strong IMF -> most stable -> lowest E and lowest H(l)
Answer: B

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4
Q

Which molecule would you expect to have a lower H(g) at room temperature?
A. H2CO
B. CH3OH

A

Lower H(g) -> most stable -> IMF
Ideal gas -> no IMF
Answer: same

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5
Q

🔺S equation

A

🔺S = qrev/T = 🔺H/T

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6
Q

Which molecule would you expect to have a higher S(g) at room temperature?
A. H2CO
B. CH3OH

A 
Higher S(g) -> more molec in gas phase -> weaker IMF
Answer: A
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7
Q

🔺G° equation

A

🔺G° = 🔺H° - T🔺S°

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8
Q

What is 🔺G and 🔺Suniv for a spontaneous process?

A

Favored
Spontaneous -> 🔺G = negative
🔺Suniv = positive

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9
Q

What is 🔺G and 🔺Suniv for a nonspontenous process?

A

“Uphill”
🔺G = positive
🔺Suniv = negative

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10
Q

Does breaking IMFs require energy or release energy? Endo or exo? Sign of 🔺H? Examples?

A

Requires energy
Endo
🔺H = positive
Ex. Vaporization (l -> g), fusion (s -> l), sublimation (s -> g)

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11
Q

Does forming IMFs require energy or release energy? Endo or exo? Sign of 🔺H? Examples?

A

Releases energy
Exo
🔺H = negative
Ex. Condensation (g -> l), freezing (l -> s), deposition (g -> s)

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12
Q

At equilibrium, 🔺G = ? Greactants = ?

A 
🔺G = 0
Greactants = Gproducts
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13
Q

MP/FP equation

A

T = 🔺Hfus / 🔺Sfus

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14
Q

Boiling point definition

A

When VP = the current atmospheric pressure -> liquid boils

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15
Q

Normal boiling point definition

A

Boiling point at atmospheric pressure (1 atm)

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16
Q

What will be the boiling point of water in Denver? Assume the atmospheric pressure is 0.82 atm.
A. >100 °C
B. <100 °C
C. 100 °C

A

0.82 atm -> not as many molecules in the gas phase
Patm ⬇️, Tbp⬇️
BP ⬇️
Answer: B

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17
Q

What’s the difference between boiling point and evaporation?

A

BP specific @ P

Evaporation -> room temp -> min KE needed to break IMF

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18
Q

Partial pressure equation

A

PV = nRT

* PA = nRT / V *

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19
Q

BP equation

A

T = 🔺Hvap / 🔺S

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20
Q

Which of the below substances would you expect to have the largest value for 🔺Hvap?
A. Methane
B. Water
C. Acetone

A

B

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21
Q

Clausius-Clapeyron Equation

A 
ln(P2/P1) = 🔺Hvap/R (1/T1 - 1/T2)
1 molec. 2 temps
🔺Hvap -> J/mol
R -> 8.314 J/mol•K
T -> K
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22
Q

Warming solid/liquid/gas equation

A

q = mC🔺T

Comes out in J or kJ

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23
Q

Phase change equation

A

Melting solid -> q = n🔺Hfus
Boiling liquid -> q = n🔺Hvap
Comes out in J or kJ

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24
Q

For a phase change, we assume that 🔺T=? 🔺G=?

A

🔺T=0
🔺G=0
Equilibrium

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25
Triple point definition
All 3 phases exist at this T & P
26
Critical point definition
The T & P limits for gas/liquid phases | Cannot distinguish gas/liquid above critical
27
If there is a positive slope, can you melt dry ice by applying a higher pressure? Is the solid or liquid more dense?
No | The solid
28
If there is a negative slope, can you melt ice by applying a higher pressure? Is the solid or liquid more dense?
Yes | The liquid
29
🔺Hsolution equation
🔺Hsolution = 🔺HLE + 🔺Hsolvation
30
Is dissolution for a solid solute endothermic or exothermic? Why?
``` Endothermic 🔺Hsolution = 🔺HLE + 🔺Hsolvation Positive = positive + negative 🔺HLE > 🔺Hsolvation Solute bonds > solvent bonds Ionic/ ion-ion bonds > H bonds ```
31
What is the sign of 🔺Ssolution when we dissolve a solid solute in a liquid solvent?
🔺Ssolution = positive
32
What will happen to a supersaturated aqueous sodium chloride solution when the temperature is increased? A. No change. B. The solubility will increase C. The solubility will decrease
``` Solid solute ⬆️ T, ⬆️ KE ⬆️ solubility Breaking the solute-solute bonds in the lattice Answer: B ```
33
Is dissolution for a gaseous solute endothermic or exothermic? Why?
Exothermic 🔺Hsolution = 🔺HLE + 🔺Hsolvation Negative = 0 + negative No LE for gas solute
34
What is the sign of 🔺Ssolution when we dissolve a gaseous solute in a liquid solvent?
🔺Ssolution = negative
35
What will happen to a carbonated soda when the temperature is increased? A. No change B. The solubility will increase C. The solubility will decrease
``` Gas solute ⬆️ T, ⬆️ KE ⬇️ solubility Break solute-solvent bonds (IMFs) Answer: C ```
36
Henry’s Law equations
Cgas = kH * Pgas kH -> Henry’s constant [M/atm] Pgas = K * Xgas Xgas = # mol A / tot mol
37
Strong electrolyte definition
100% dissociation AB -> A + B Ionic = strong
38
Weak electrolyte definition
<100% dissociation | AB -> A + B, AB
39
Nonelectrolyte definition
0% dissociation AB -> AB Covalent, i = 1
40
How to calculate van’t Hoff factor
i = moles of particles in solution / moles of formula units dissolved
41
Molarity equation
M = moles solute / L solution
42
What does “concentration of particles” mean?
Molarity with the van’t Hoff factor -> iM = i(moles solute) / L solution
43
Molality equation
♍️ = moles of solute / kg solvent
44
Molality of the particles of a solution equation
♍️ = (i) mol solute / kg solvent
45
What is the effect of ⬆️ mixing?
⬆️ mixing, ⬆️ S, ⬇️ G, more stable, ⬇️ VP, ⬆️ BP
46
Gsolvent ? Gsolution | Ssolvent ? Ssolution
Gsolvent > Gsolution | Ssolvent < Ssolution
47
Raoult’s Law for VPsolution
VPsolution = Xsolvent * VPsolvent Xsolvent = # moles solvent / tot moles VPsolvent -> p°
48
Raoult’s Law for 🔺VP
``` 🔺VP = -Xsolute * VPsolvent Xsolute = mol solute / tot moles Xsolute -> watch for i! VPsolvent-> VP° * VPsolution = VP°solvent + 🔺VP * ```
49
What is Xsolute for 1 mole of sodium chloride in 55.55 mol H2O?
X = mol solute / tot mol = 1 mol Na+ + 1 mol Cl- / (55.55 + 1 + 1) = 0.035
50
Raoult’s Law (for liquids)
VPsolution = VPsolvent A + VPsolvent B
51
Dalton’s Law (for gases)
Ptotal = PGas A + PGas B
52
Sample A: 250 mL of water Sample B: 1 mole of sugar in 250 mL of water Which sample has the highest boiling point? Why?
B IMFs solute-solvent
53
Boiling Point Elevation equation
``` 🔺Tb = iKb♍️ 🔺BP = iKb♍️ 🔺BP -> °C Kb = BP elevation constant [°C/♍️] ♍️ -> molal Tbp’ = Tbp° + 🔺Tbp BP’ = BP° + 🔺BP ```
54
Nonvolatile solute van’t hoff factor
1
55
Sample A: 250 mL of water Sample B: 1 mole of sugar in 250 mL of water Which sample has the lowest freezing point? Why?
B | Solution is more stable over a wider Temp range
56
Freezing Point Depression equation
``` 🔺Tf = -iKf♍️ FP = -iKf♍️ FP -> °C Kf = FP depression constant [°C/♍️] FP’ = FP° + 🔺Tf ```
57
If there are 0.0719 mol NaCl, how many mol solute are there?
mol solute = 0.0719 mol Na+ + 0.0719 mol Cl- = 0.1438 mol
58
You find a U tube that has allowed for the solvent to pass through the barrier after a period of time. A is lower and B is higher. 1. Is A the solvent or the solution? 2. Is B the solvent or the solution? 3. Why?
1. Solvent 2. Solution 3. Solvent moves to solution to try to establish equilibrium
59
Osmotic Pressure equation
``` pi = iMRT pi -> atm M -> molarity ionic -> iM R = 0.08206 L•atm / mol•K T -> Kelvin ```
60
Magnitude of Q or K Very Small Reaction Progression? Spontaneity?
Reactant Favored | nonspon
61
Magnitude of Q or K 1-ish | Reaction Progression?
[Products] = [Reactants]
62
Magnitude of Q or K Very Large Reaction Progression? Spontaneity?
Product Favored | spon
63
KC vs. KP equation
``` KP = KC(RT)^🔺n R -> 0.08206 L•atm / mol•K T -> Kelvin 🔺n = products - reactants gases only! ```
64
Product Favored Reaction
Product Favored -> Exo | G° products is lower than G° reactants
65
Reactant Favored Reaction
Reactant Favored -> Endo | G° reactants is lower than G° products
66
How to find 🔺G° on free energy diagram
Right side of curve - left side of curve Low right side - high left side = negative (spon) High right side - low left side = positive (nonspon)
67
Which side of the curve is Q < K?
Left side is always Q < K
68
🔺G° vs. 🔺G equation
``` 🔺G = 🔺G° + RTlnQ RTlnQ -> mixing -> S 🔺G = standard + mixing (real) expt ```
69
🔺G° equation at equilibrium
``` 🔺G = 0 Q = K 🔺G° = -RTlnK R = 8.314 J / mol•K T = 298 K ```
70
When K is small, what is the sign of 🔺G°?
Positive
71
When K is big, what is the sign of 🔺G°?
Negative
72
What happens when I increase the reactants?
⬆️ Reactant, ⬇️ Q, shift to make more products Reactant —> Product want: Q=K “Add Away”
73
What happens when I decrease the reactants?
⬇️ Reactants, ⬆️ Q Q > K React ⬅️⬅️ Prod “Take Toward”
74
Where does the reaction shift when heat energy is added to an exothermic reaction?
``` Reactants -> Products + Heat ⬆️ Prod, ⬆️ Q Q > K ⬅️⬅️ The reaction shifts to “add” some reactants. ```
75
Where does the reaction shift when heat energy is added to an endothermic reaction?
``` Reactants + Heat -> Products ⬆️ React, ⬇️ Q Q < K ➡️➡️ The reaction shifts to “add” some products. ```
76
van’t Hoff Equation
``` ln(K2/K1) = (🔺H°/R) * (1/T1 - 1/T2) K -> eq constants 🔺H° -> J/mol R -> 8.314 J/mol•K T -> Kelvin ```
77
Where does the reaction shift when we decrease the volume of the container of gases?
⬇️ V, ⬆️ P, P is too high The reaction will shift in such a way to decrease the pressure. It will move towards the side of the reaction with fewer gas molecules. -> wants to remove gas particles in order to ⬇️ P
78
Where does the reaction shift when we increase the volume of the container of gases?
⬆️ V, ⬇️ P, P is too low The reaction will shift in such a way to increase the pressure. It will move towards the side of the reaction with the greater number of gas molecules. want more gas particles
79
How does decreasing the temperature of an exothermic reaction affect the value of K?
K will increase
80
How does increasing the temperature of an endothermic reaction affect the value of K?
K will increase
81
How does increasing the temperature of an exothermic reaction affect the value of K?
K will decrease
82
How does decreasing the temperature of an endothermic reaction affect the value of K?
K will decrease

CH 302 (5 decks)

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