 how the molar mass of a compound is calculated  calculating the amount of reactant needed to make a certain amount of product  using the relationship moles = mass / molar mass 1.Calculate the molar mass of the following compounds; MgCl 2 NH 4 ClMg(NO 3 ) 2 2.Calculate the molar mass of the following ; 3 moles of H 2 SO moles of C 2 H 5 OH 3.Calculate the number of moles in; 17 g of NaNO 3 24 g of (NH 4 ) 2 CO 3 4.In the following reaction; 2Fe + 3Cl 2  2FeCl 3 What mass of iron chloride would be produced from 0.5 moles of iron? When 100 g of iron reacts, how many moles of chlorine react?

 finding the mass of an element in a compound  calculating percentage mass of an element in a compound  calculating empirical formula  calculating empirical formulas from mass or percentage mass 1.Justin takes a Calcium Carbonate tablet to help with his indigestion. What is the % of Calcium in Calcium Carbonate? The tablet weighs 10g, what is the actual mass of Calcium in the tablet? 2.Find the percentage mass (to the nearest whole number) of: nitrogen in copper nitrate, which has a formula of Cu(NO 3 ) 2. 3.What is the empirical formula of a compound containing: 29.1% sodium, 40.5% sulfur and 30.4% oxygen 4.Caffeine contains 49.48% C, 5.15% H, 28.87% N and 16.49% O. Find the empirical formula.

 using the relationship between moles, concentration and volume  calculating concentration using titrations 1.In a titration, 14 cm 3 of 0.15 mol/dm 3 nitric acid (HNO 3 ) is neutralised by 20 cm 3 of ammonium hydroxide (NH 4 NO 3 ) solution. What was the concentration of the alkali?  how to measure reaction rate  what rates graphs show  what limiting factors are  calculating gas volumes in a reaction 2.The nitric acid was added to magnesium ribbon. 12 cm 3 of hydrogen gas was evolved in 60s. What would you expect to happen if you used 0.3 mol/dm 3 of acid? Explain your prediction in terms of particles. How many moles of hydrogen are evolved in this experiment.

 reversible reactions  equilibria  explaining the Contact process  how to alter the equilibrium position  the difference between how weak and strong acids react  ionisation  why weak acids react more slowly  what happens when weak and strong acids are electrolysed  precipitation reactions  the tests for sulphates and halides  how to make an insoluble salt  why precipitation reactions are very fast