1. Starter Number of moles of OH- in 10 moles of Mg(OH)2
Volume of 10 mol NH3(g)
volume of water( in cm3) needed to make a
0.1 moldm-3 solution from mol of NaOH.
Extension:
A sample of battery acid contains 1176 g of sulfuric acid, H2SO4, in 3.0 dm3 of liquid. Calculate the concentration of the sulfuric acid in g dm–3
Extension: 392 g dm–3

2. Moles and reactions L.O.:
Deduce the quantities/volumes of reactants and products from balanced equations.

3. Prep-work Research an example of a useful acid and a useful base.
You must include:
Definitions of acid and base.
At least one application for each.
Two facts about the acid and base.

4. Important equations: Working out moles: From volumes of solution
n = c x V n = number of moles
c = concentration
V = Volume
From mass
n = m/M m = mass,
M = molar mass
Allan (chem inorgI)

5. Simple stoichiometry

6. Calculate the mass of calcium oxide obtained when 20 g of calcium carbonate are thermally decomposed. [Relative atomic masses: Ca = 40, C = 12, O = 16]
ANS= 11.2G

7. Calculate the volume of carbon dioxide obtained, at room temperature and pressure, when 25 g of calcium carbonate undergoes thermal decomposition. CaCO3(s) → CaO(s) + CO2(g) [Relative atomic masses: Ca = 40, C = 12, O = 16]
Ans 6dm3

8. Worksheet 2.5 Allan (chem inorgI), worksheet 2.5
45 Min? rest of worksheet for HW?

9. 4Fe(NO3)3(s) → 2Fe2O3(s) + 12 NO2(g) + 3O2(g)
When heated, iron (III) nitrate (Mr = 241.8) is converted to iron(III) oxide, nitrogen dioxide and oxygen.
4Fe(NO3)3(s) → 2Fe2O3(s) + 12 NO2(g) + 3O2(g)
Calculate the amount, in moles, of iron(III) nitrate in the 2.16 g sample.
Calculate the amount, in moles, of oxygen gas produced in this reaction.
3) Calculate the volume, in m3, of nitrogen dioxide at 293 C and 100 KPa produced from 2.16 of Fe(NO3)3. (R = 8.31 J K-1 mol -1)
From AQA Q2 Jun14 Chem1

10. 2.16 ÷ = (mol)
n(O2) = × 0.75 (= mol)
T = 566 K and P = Pa
Moles NO2 = (mol)
V = nRT/p = m3

11. Aqa q5a from jun12/chem1