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DAT BIO > General Chemistry help > Flashcards

General Chemistry help Flashcards

1
Q

formula for molecule weight

A

molecular weight= molecular mass= (grams acid)/(moles acid)

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2
Q

first order reaction, half life formula

A

kt(.5)= .693

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3
Q

density formula

A

D= m/v

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4
Q

what does % (w/w) mean?

A

g of substance/ g of solution

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5
Q

diamagnetic

A

all electrons are paired, not deflected by a magnetic field

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6
Q

paramagnetic

A

there re unpaired electrons; deflected by a magnetic field

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7
Q

avogadro’s number

A

6e23

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8
Q

M

A

molarity= moles of solute/liters of solution

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9
Q

henderson hasselbach eqn

A

pH=pKa +log (salt/acid)

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10
Q

when does H has a -1 charge?

A

when in hydride NaH, KH, LiH

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11
Q

ΔH?

A

ΔH=mcΔT

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12
Q

ideal gas law

A

PV=nRT

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13
Q

voltaic cell

A

+ Eº

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14
Q

gas-density calculations

A

P(MW)= DRT

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15
Q

Boyle’s Law

A

increase P, decrease V; constant T

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16
Q

Gay Lussac’s Law

A

increase P, increase T; constant V

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17
Q

Charle’s Law

A

increase V, increase T; constant P

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18
Q

q=?

A

mΔHvap

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19
Q

at equilibrium include? exclude?

A

for equilibrium systems, omit all solids and pure liquids from K expression

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20
Q

m

A

molality= #moles solute/ kG solvent temperature independent

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21
Q

O order reaction slope

A

-k ; [A] vs. t

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22
Q

1st order reaction slope

A

-k; ln[A] vs. t (nuclear decay will also exhibit this, but a perbolic shape graph with negative slope)

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23
Q

2nd order reaction slope

A

+k; [1/[A]] vs. t

24
Q

increase P

A

drives rxn toward lower V

25
Q

decrease T

A

shifts rxn to left, exothermic rxns favored

26
Q

increase T

A

shifts rxn to right; favors endo rxn

27
Q

current eqn

A

I= q/t

28
Q

how many coloumbs in q?

A

36,000 C=q

29
Q

spontaneous rxn

A

goes to completion by 50%; +Eº, -ΔG, K>1

30
Q

Nernst Equation

A

E=Eº-(.0591/n)logQ ; Eº=standard electrode potential; E= EMF at a new concentration; n= # of e- given in the half-rxn; Q= run quotient

31
Q

estimate pH of Ka: 2e-5, 4e-5, 7e-5

A

4.7, 4.4, 4.2

32
Q

ΔG

A 
ΔG= ΔH-TΔS; 
ΔG= -nFEº
33
Q

work eqn

A

w= -PΔV (atm)

34
Q

alpha decay

A

4 (mass)

2 (atomic)

35
Q

beta decay

A

0(mass)

-1(atomic)

36
Q

osmotic pressure eqn

A

osmotic pressure=MRTi; (moles solute/Lsoln)(.0821)(K)(van’t hoff factor)

37
Q

precipitate examples

A

AgBr, PbCl2, BaSO4, CaCO3

38
Q

Raoult’s Law

A

VPof water over soln= VP of pure H2O(Xsolvent)

39
Q

SI unit for pressure

A

pascal

40
Q

osmolarity

A

solute conetration/Liter

41
Q

catalyst

A

lower the energy of activation for both the fwrd and reverse rxn, lower the potential energy of the transition state, change the reaction mechanism

42
Q

spectrum of visible light; wavelength and frequency

A

ROYGBIV; decrease wavelength towards R; decrease frequency and energy towards V

43
Q

energy eqn

A

E=hf; E=hc/wavelength

44
Q

bronsted-lowry acids

A

donate a proton

45
Q

bronsted-lowry bases

A

accepts a proton

46
Q

lewis acid

A

accept electron

47
Q

lewis base

A

donate electron

48
Q

gives color

A

transition metals, Cu

49
Q

strong bases

A

NaOH, KOH, LiOH, RbOH, CsOH, Ca(OH)2, Ba(OH)2

50
Q

ΔT

A

ΔT=(Kb)mi; (Kb)(moles of solute/kg of solvent)(van hoff factor)

51
Q

heat lost by metal= heat gained by h2o

A

mcΔT= mcΔT

52
Q

base

A

accepts protons

53
Q

acids

A

donate protons

54
Q

ΔH of formation

A

sum of bonds broken- sum of bonds formed

55
Q

n=1, n=2, n=3 electron capacity

A

2e-, 8e-, 18e-

DAT BIO (12 decks)

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