Test 5 Flashcards

1
Q

eqn for work

A

force * distance

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2
Q

eqn for PV work & what happens when pressure = constant

A
w = -P∆V
w = 0 when pressure is constant
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3
Q

what type of energy do chem bonds have

A

potential

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4
Q

x cal = how many Cal

A

1000

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5
Q

1st law of thermodynamics

A

smth gains E when smth loses it

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6
Q

define system

A

chemicals in a rxn

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7
Q

define surroundings

A

the environment around the chemicals

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8
Q

define exothermic

A

system loses E, surroundings gain it

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9
Q

def endothermic

A

system gains E, surroundings lose it

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10
Q

define ∆V

A

change in volume: V₂ - V₁

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11
Q

define ∆T

A

change in temp: T₂ - T₁

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12
Q

define ∆E

A

all internal system E: w + q (work + heat)

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13
Q

define ∆H

A

enthalpy of a rxn; change in enthalpy = heat of rxn

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14
Q

eqn for heat transfer enthalpy @ constant pressure

A

∆H = qₚ

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15
Q

exothermic rxn x 4

A
heat E = product
A + B → C + D + Heat E
Reactant E > Product E
q, ∆E, ∆H = all negative
heat transferred to surroundings
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16
Q

endothermic rxn x 4

A
heat E = reactant
A + B + heat E → C + D
Reactant E < Product E
q, ∆E, ∆H = all positive
heat transferred to system
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17
Q

is ∆H intensive or extensive

A

extensive

18
Q

units to write ∆H in

A

±kJ/x mol (write the + or - out, I swear to god)

19
Q

enthalpy of formation rxn, how to write & what it is

A

∆Hբ

forming 1 mol of substance from elements in products in standard conditions

20
Q

define specific heat capacity and units used for it, plus one extra thing about it

A

amt heat needed to raise temp of 1 g substance by 1° C
units in J/(g * °C)
super high for water

21
Q

A piece of copper with a mass of 218 g has a heat capacity of 83.9 J/°C. What is the specific heat of copper? (1 step)

A

divide J/g, bc specific heat capacity is in J/gC

22
Q

Hess’s Law x 3

A

1) Bc you can combine rxn A→B and rxn B→C to make rxn A→C, you can add their ∆Hs to get overall ∆H
2) Multiply rxn coefficients and ∆H by the same factor
3) To reverse the rxn, change the sign of the ∆H

23
Q

how to show work for hess’s law combination rule, 4 steps

A
1) Write out both rxns:
A+B→C+D with ∆H = -10kJ & C+D→E+F with ∆H = -20kJ
2) Combine: 
A + B + C + D → C + D + E + F
3) Cross out what you don't need:
 A + B +  ̶C̶ ̶+̶ ̶D̶  → C̶ ̶+̶ ̶D̶  + E + F
4) Rewrite overall rxn and add ∆Hs:
A + B → E + F
-10kJ + (-20kJ) = -30kJ ∆H
24
Q

standard conditions for thermochem

A

25°C, 1 atm

25
Q

def kinetic & potential E

A
kinetic = E of moving object
potential = stored E
26
Q

liquid → gas

A

vaporization

27
Q

gas → solid

A

deposition

28
Q

2 rules for when ∆Hᵣₓₙ ≠ ∆Hբ of product

A

1) when 1+ mol of substance is being created in product

2) when reactants aren’t in their regular state of matter

29
Q

formula to solve smth like “Benzene’s specific heat capacity is 1.74 J/g·°C. If 16.7 kJ of energy is absorbed by a 225-g sample of benzene at 20.0°C, what is its final temperature?”

A

qₛᵤᵣᵣ = m * Cₛ * ∆T

heat gained/lost in J = mass * specific heat * temp change in °C

30
Q

what does a bomb calorimeter measure and thru what

A

combustion rxns; constant-volume type (?)

31
Q

def calorimeter heat capacity for bomb calorimeter

A

AKA calorimeter constant

qₛᵤᵣᵣ in kJ = (kJ/°C)(Tբᵢₙₐₗ)

32
Q

relation between qₛᵧₛ and qₛᵤᵣᵣ

A

-qₛᵤᵣᵣ = qₛᵧₛ

33
Q

how to find ∆Hₛᵧₛ from qₛᵧₛ

A

∆Hₛᵧₛ = qₛᵧₛ/mol comp. used in rxn

34
Q

how to do bomb calorimetry probs like “T rises from 25°C to 29°C in bomb calorimeter when 3.5 g sucrose combusts. Find ∆Hᵣₓₙ for sucrose combustion in kJ/mol sucrose. Heat capacity is 4.90 kJ/°C. Mol mass of sugar is 342.3 g/mol.”

A

1) find qₛᵤᵣᵣ with calorimeter constant (kJ/°C)(Tբᵢₙₐₗ)
2) get ∆H of qₛᵧₛ by reversing sign on qₛᵤᵣᵣ
3) divide qₛᵧₛ by mol of the substance used to find ∆Hₛᵧₛ

35
Q

how to do coffee cup calorimetry probs like “Two solutions, initially at 24.6°C, mix in a coffee cup calorimeter. When 100 mL of 0.1 M AgNO₃ solution mixes with 100 mL of 0.2 M NaCl solution, calorimeter T rises to 25.3°C. Find ∆H°rxn. Assume density & heat capacity of the solutions = that of water.”

A

1) find qₛᵤᵣᵣ with calorimeter constant (kJ/°C)(Tբᵢₙₐₗ)
2) get ∆H of qₛᵧₛ by reversing sign on qₛᵤᵣᵣ
3) divide qₛᵧₛ by mol of the substance used to find ∆Hₛᵧₛ

36
Q

what is a coffee cup calorimeter like x 3

A

constant-pressure
not air-tight
water surrounding temp measured

37
Q

heat of formation formula

A

∆Hᵣₓₙ = Σn∆Hբ(products) - Σn∆Hբ(reactants)
n = balanced rxn coefficients
basically sum of heat enthalpy products - h. e. reactants

38
Q
Steps for: "Solid Na2O2 reacts with liquid water to make aqueous Na2O2 and O gas. How much heat is released if 327.2 g of O gas is made from the reaction of Na2O2 and water under standard conditions?"
Substance	ΔH°f(kJ/mol)
  Na2O2(s)	–510.9  
  NaOH(aq)	–469.6  
  H2O(l)	        –285.8
A

1) balance eqn: Na2O2 + 2H2O → 2NaOH + O2
2) write out sum of product coeffs * their ΔH°fs - reactant coeffs * their ΔH°fs
3) take that number & multiply by # mol listed in the eqn

39
Q

heat needed to convert 10g ice @ 20°C into 110°C steam?

A

1) H₂O (s) @ -20°C → H₂O (s) @ 0°C
(ice at its temp now to ice at its maximum temp before turning states)
find q₁ with your specific heat eqn
2) … → H₂O (l) @ 0°C
(ice at 0°C to water at 0°C)
multiply mol H₂O by fusion heat (bc s → l) for q₂
3) … → H₂O (l) @ 100°C
(water at its temp to water at max temp before turning states)
find q₃ w/ specific heat eqn
4) …→ H₂O (g) @ 100°C
(water at 100°C to gas at 100°C)
multiply mol by vaporization heat (bc l → g) for q₄
5) …→ H₂O (g) @ 110°C
(steam @ temp now to steam at final temp)
use specific heat eqn to get q₅
6) add up q₁₋₅ to get total E

40
Q

when changing states but not temps, what number do you use for s → l and l → s?

A

fusion

41
Q

when changing states but not temps, what number do you use for g → l and l → g?

A

vaporization