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Stoichiometry

Stoichiometry. Reading Equations using Moles. 1. Ca + H 2 SO 4 CaSO 4 + H 2. 1. 1. 1. The above reaction reads: 1 amount of Ca reacts with 1 amount of H 2 SO 4 to give 1 amount of CaSO 4 and 1 amount of H 2 gas.

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Stoichiometry

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  1. Stoichiometry

  2. Reading Equations using Moles 1 Ca + H2SO4 CaSO4 + H2 1 1 1 The above reaction reads: 1 amount of Ca reacts with 1 amount of H2SO4 to give 1 amount of CaSO4 and 1 amount of H2 gas. (we don’t usually put in the ones – but if we did it would look like this) The amount we use is the mole Now the reaction reads: 1 mole of Ca reacts with 1 mole of H2SO4 to give 1 mole of CaSO4 and 1 mole of H2 gas.

  3. Reading Equations using Moles Ca + H2SO4 CaSO4 + H2 • Questions: • If we have 1 mole of Ca how many moles of H2SO4 are needed to fully react the Ca? • If we had 0.5 mole of Ca how many moles of H2SO4 would be required? • If 0.5 mole of Ca reacted with 0.5 mole of H2SO4 how many moles of CaSO4 and how many moles of H2 gas are formed? Ans: 1mole Ans: 0.5 mole Ans : 0.5 mole of H2 gas, 0.5 mole of CaSO4

  4. Reading Equations using Moles Ca + H2SO4 CaSO4 + H2 Questions: If 0.5 mole of Ca reacted with 0.5 mole of H2SO4 how many moles of CaSO4 and how many moles of H2 gas are formed? Ans : 0.5 mole of H2 gas, 0.5 mole of CaSO4 Given the Ar (atomic mass) values H = 1 gmol-1 Ca = 40 gmol-1 S = 32 gmol-1 O =16 gmol-1 Find the molar masses (Mr) of H2SO4 , CaSO4 and H2 Then use these and the mole (n) formula to work out the mass of H2 gas and the mass of CaSO4 formed (Hint you will need to rearrange the formula)

  5. Reading Equations using Moles Fe2O3 + 3CO 2Fe + 3CO2 Q1. If 200g of Fe2O3 is reacted in the above equation what mass of Fe is produced? (Mr Fe2O3 = 160 gmol-1, Mr Fe = 55.85 gmol-1) From the equation we see that for every mole of Fe2O3that reacts 2 moles of Fe are formed) This means that if we can find the number of moles of Fe2O3 we can then work out the number of moles of Fe and then the mass of Fe Using the mole ratio from the equation how many moles of Fe are formed? (unknown/known) You got it 2.5 moles of Fe is formed –now work out the mass of Fe

  6. Work out how many moles of HCl is used to completely react 60grams of Mg metal in the following reaction? Draw the grid Mg + 2 HClMgCl2 + H2 Mg HCl Mr 24.0 gmol-1 36.5 gmol -1 183 grams mass 60.0 grams ? = 2.5 moles 5.00 moles 1 2 Therefore (unknown/known) 2mol / 1mol x moles of Mg = moles of HCl Therefore 2 x 2.5 moles = 5 moles of HCl

  7. What was the mass of HCl used? m = 5 x Mr = 5 mol x 36.5 gmol-1 = 182.5 g = 183 g (3sf)

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