chemistry equations Flashcards

1
Q

R.A.M (Ar) =

A

∑(isotopic mass x % abundancy)/ 100 (no units)

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2
Q

R.M.M (Mr) =

A

∑Ar of all atoms in chemical formulae (no units)

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3
Q

= Mr

A

Molar mass (M)/ g mol-1

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4
Q

Moles/ mol =

A

mass (g)/ M (g mol-1)

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5
Q

Moles of a gas @ R.T.P/ mol =

A

volume (dm3)/ 24 (dm3 mol-1)

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6
Q

Concentration/ mol dm-3 =

A

moles (mol)/ volume (dm3)

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7
Q

Concentration/ g dm-3 =

A

mass (g)/ volume (dm3)

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8
Q

Concentration/ g dm-3 =

A

concentration (mol dm-3) x M (g mol-1)

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9
Q

Using the molar gas volume @ RTP: moles (mol)

A

= volume (dm3)/ Vm

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10
Q

where RTP =

molar gas volume =

A

room temperature & pressure (20oC & 101 kPa) Vm = 24.0 dm3 mol-1

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11
Q

Ideal Gas Equation:

A

pV = nRT

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12
Q
where p = 
V = 
n = 
mol R =
T =
A

pressure/ kPa or Pa
volume/ dm3 or m3 moles/
molar gas constant 8.314 J mol-1 K-1
temperature/ K

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13
Q

% yield =

A

actual yield (g) / theoretical yield (g) x 100

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14
Q

% atom economy =

A

mass of desired product from balanced equation / total mass of reactants from balanced equation
x 100

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15
Q

ΔrH =

A

∑E(bonds broken)- ∑E(bonds formed)

where ΔH = enthalpy change of reaction/ kJ mol-1 E = bond enthalpy/ kJ mol-1

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16
Q

ΔrH =

A

∑(ΔfH products) - ∑(ΔfH reactants)

where ΔrH = enthalpy change of reaction/ kJ mol-1 ΔfH = enthalpy change of formation/ kJ mol-1

17
Q

ΔrH =

A

∑(ΔcH reactants) - ∑ ΔcH(products)

where ΔrH = enthalpy change of reaction/ kJ mol-1 ΔcH = enthalpy change of combustion/ kJ mol-1

18
Q

q =

where 
q =
m=
 c =
 T=
A

mcΔT

heat transferred to or from water/ J

mass of water/ g

specific heat capacity of water/ 4.18 J g-1 K-1 Δ

change in temperature in water/ K

19
Q

ΔH =

enthalpy topic

20
Q

Rate of reaction =

A

gradient = change in Y /
change in X

21
Q

Equilibrium constants for the general reaction

A

: aA + bB ⇌ cC + dD

22
Q

Kc =

A

[C]c[D]d / [A]a[B]b

23
Q

General formula of an alkane =

24
Q

General formula of an alkene =

25
General formula of an alkyl group =
CnH2n+1
26
k = | where k = rate constant/
ln2/ t1/2 s-1 t1/2 = half-life/ s
27
k = | where k = rate constant/ various rate
A e-Ea/RT , taking natural logs, ln k = -Ea/ RT + ln A
28
``` k = A = Ea = R = T = ```
``` k = rate constant/ various units A = pre-exponential factor/ same units as k Ea = activation energy/ J mol-1 R = gas constant = 8.314 J mol-1 K-1 T = temperature/ K ```
29
Equilibrium gas constant, Kp, for the general reaction:
aA + bB ⇌ cC + dD
30
Kp =
p(C)c x p(D)d / p(A)a x p(B)b