UNIT 0 | EQUATION SHEET | 12U
Date: ________________
Name: ________________
SCH4U - Equation Sheet
Constants
Basic Equations
Avogadro’s Number (Na)
Universal Gas Constant (R)
Speed of Light
Specific Heat Capacity of Water (C)
Molar Volume
Ionic Product Constant of Water (Kw)
STP conditions/SATP
6.022x1023
8.314 J/molK or 0.0821 L•atm/mol•K
3.00 x 108 m/s
4.18 J/gK or 4.18 J/g•ºC
22.1 L/mol
1.00x10-14 (mol/L)2 at 298 K (25 C)
273 K and 100 kPa/ 298 K and 100 kPa
^
𝑛=_
𝑛 = 𝑐𝑉
𝑃𝑉 = 𝑛𝑅𝑇
𝐶` 𝑉` = 𝐶a 𝑉a
𝑂𝑟𝑑𝑒𝑟 𝑜𝑓 𝑅𝑒𝑎𝑐𝑡𝑖𝑜𝑛 = 𝑚 + 𝑛
Conversion Factors
1 atm = 101.325 kPa
0ºC = 273.15 K
1nm = 10-9 m
1 atm = 760 torr = 760 mm Hg
1 dm3 = 1 L = 1x10-3 m3 = 1x103 cm3 = 1 x 103 mL
1 amu = 1.66 x10-27 kg
Acid-Base Chemistry
𝑝𝐻 = −log [𝐻! 𝑂" ]
Thermodynamics
𝑞 = Δ𝐻 𝑎𝑡 𝑐𝑜𝑛𝑠𝑡𝑎𝑛𝑡 𝑝𝑟𝑒𝑠𝑠𝑢𝑟𝑒
[𝐻! 𝑂" ] = 10#$%
𝑄 = 𝑚𝑐Δ𝑇
𝐾& = 𝐾' × 𝐾(
𝑄/0/1-2 + 𝑄/+..3+45647 = 0
𝑝𝐾' + 𝑝𝐾( = 𝑝𝐾)
ΔH/0/1-2 = 𝑄/0/1-2
𝑝𝐾' = −𝑙𝑜𝑔𝐾'
ΔH = nΔH.94
𝑝𝐾( = − log 𝐾(
ΔH°.94 = ΣD(broken) − ΣD(formed)
𝑝𝐾( = 14 − 𝑝𝐾'
ΔH°.94 = ΣSΔH°,(;) T − ΣSΔH°,(=) T
Chemical Kinetics & Equilibrium
ΔC
𝑅𝑎𝑡𝑒 =
Δ𝑡
𝑅𝑎𝑡𝑒 𝑅𝑒𝑎𝑐𝑡𝑖𝑜𝑛 = 𝑘[𝐴]2 [𝐵]4
𝐾=
[?]A [B]C
[D]E [*]F
𝑝𝐻 + 𝑝𝑂𝐻 = 14
𝑝𝑂𝐻 = −log [𝑂𝐻# ]
[𝑂𝐻# ] = 10#$%
[𝐻𝐴]
𝑝𝐻*+,,-. = 𝑝𝐾' − log 5 # 7
[𝐴
Redox
𝐶ℎ𝑎𝑟𝑔𝑒 = 𝐶𝑢𝑟𝑟𝑒𝑛𝑡 𝑥 𝑇𝑖𝑚𝑒
𝐸°G-HH = 𝐸°G'1I35- − 𝐸°'435-
Solubility
Qc
Kc
Q
Ksp (Precipiate)
<
Products Favoured
<
No
=
EQ
=
No
>
Reactants Favoured
>
Yes (Super Saturated)
Formations
1. Acid + Metal = Salt (aq) + Hydrogen Gas
Ex. 2HCl(aq) + Zn(s) à ZnCl2(aq) + H2(aq)
2. Acid + Base = Salt (aq) + Water
Ex. HCl(aq) + NaOH(aq) à NaCl(aq) + H2O(l)
3. Acid + Metal Carbonate = CO2 + H2O + Salt (aq)
Ex. CaCO3(s) + 2HCl(aq) à H2O(l) + CO2(aq) + CaCl2(aq)
4. Metal Oxide + Acid à Salt (aq) + Water
Ex. MgO(s) + 2HCl(aq) à MgCl2(aq) + H2O(l)
UNIT 0 | EQUATION SHEET | 12U
Date: ________________
Polyatomic Ions
Periodic Table of Electronegativities
Name: ________________