Atomic Mass Empirical formula Yield CC9 Calculating Involving Masses p2630 1 O 2 C 3Mg 4Ca 5N 4 Empirical formula the simplest ratio of atoms in a ID: 803295
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Slide1
1. Define
-Formula massAtomic MassEmpirical formulaYield
CC9 - Calculating Involving Masses (p26-30)
1: O 2: C 3:Mg 4:Ca 5:N
4. Empirical
formula (the simplest ratio of atoms in a compound) e.g. The empirical formula of C2H4 (ethene) is CH2.What is the empirical formula of the following?C2H6C4H8H2OC6H12O6In a reaction 20g of calcium reacts with 6g of carbon and 24g of oxygen.
8. (Higher) Moles is the name given to a certain number of particles.1 mole = 6.02x1023 particlesHow many particles in a mole of oxygen?How many particles in 4 moles of nitrogen?
9. (Higher) Moles - calculating the number of moles in a mass of compound.Use the equation Number of moles = Mass of compound Formula mass of compoundHow many moles in 18g of H2O.How many moles in 200g of CaCO3.How many moles in 48g of CH4.What is the mass of 4 moles of CO2
5. Calculating % yield - identify two figures, the predicted yield and the actual yield the use the equation:% Yield = Actual Yield x 100 Predicted yieldCalculate predicted yield in the following experiment.40g of CO2 produced when CaCO3 is heated when the expected yield was 44g80g of CaCO3 produced when CaCO3 heated when the expected yield was 100g
7. Calculating concentration - divide the mass dissolved by the volume (in litres).Concentration (g/dm3)= mass (g) volume (dm3)1 25g of copper sulphate is dissolved in 500cm3 of water.2 What is the mass of sodium chloride in 300cm3 of solution with concentration of 12g/dm3
3.
Relative
formula mass - calculate the formula mass of the following compoundsH20CO2CH4NH3H2SO4(NH3)2NO3
2. Using the periodic table – find the mass of the elements below using a periodic table
6. Converting dm
3
--> cm
3
1000 cm
3
= 1 dm
3
= 1 litre
20 cm
3
= _____dm
3
_____cm
3
= 0.76dm
3
Slide2Define:
Formula mass: mass of all atoms in a molecule or compoundAtomic Mass: mass of protons and neutrons
Empirical formula: simplest ration of atoms in a compound
Yield: mass produced in an experiment
CC9 Calculating With Mass (p26-30)
You must use the mass figures from the periodic table symbolsCalculate the formula mass of the following compounds?H20 18CO2 44CH4
16NH3 17H2
SO4 98(NH3)2NO3 96What is the mass of the following elements?1,O 16 2,C 12 3, Mg 24 4, Ca 40
5, N 14 Empirical formula is the simplest ratio of atoms in a compound.e.g. The empirical formula of C2H4 (ethene) is CH2.What is the empirical formula of the following?
C2H6 CH3C4H8 C2H
4H
2
O H2OC6H12O6 CH2O
Moles is the name given to a certain number of particles.It is 6.02x1023.
How many particles in a mole of oxygen?
6.02 x 10
23
How many particles in 4 moles of nitrogen?
2.4 x 10
24
Calculating the number of moles in a mass of compound.
Use the equation Number of moles =
Mass of compound
Formula mass of compound
How many moles in 18g of H2O. 1How many moles in 200g of CaCO3. 2How many moles in 48g of CH4. 3What is the mass of 4 moles of CO2 176
Calculating % Yield.You need to identify two figures, the predicted yield and the actual yield the use the equation:% Yield = Actual Yield x 100 Predicted yieldCalculate predicted yield in the following experiment.40g of CO2 produced when CaCO3 is heated when the expected yield was 44g91%80g of CaCO3 produced when CaCO3 heated when the expected yield was 100g 80%
Calculating concentration.Simply divide the mass dissolved by the volume (in litres).Concentration (g/dm3)= mass (g) volume (dm3)1 25g of copper sulphate is dissolved in 500cm3 of water.50g/dm32 What is the mass of sodium chloride in 300cm3 of solution with concentration of 12g/dm33.6g
1dm3 = 100cm3 =1000ml = 1litre
Finding empirical formula.
Find the empirical formula in the following:
In a reaction 20g of calcium reacts with 6g of carbon and 24g of oxygen.
CaCO3