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AQA A Level Chemistry
| Question | Answer |
|---|---|
| What is the relative atomic mass of an atom? | The average mass of an atom of an element (taking into account its naturally occurring isotopes)4 relative to 1/12 the relative atomic mass of an atom of carbon-12 |
| What is the relative molecular mass of a molecule? | The mass of a molecule compared to 1/12 the relative atomic mass of an atom of carbon-12 |
| How are the number of moles of a substance established from its mass? | Moles = mass/Mr |
| How many moles are in Xg of Y? | X/Mr of Y |
| How many moles are there in 4.00 kg of CuO | 50.3 |
| How many moles are there in 39.0 g of Al(OH)3 | 0.5 |
| How many moles are there in 1 tonne of NaCl | 17100 |
| How many moles are there in 20.0 mg of Cu(NO3)2 | 0.000107 |
| What is the mass of 0.200 moles of Al2O3 | 20.4g |
| What is the mass of 0.00200 moles of (NH4)2SO4 | 0.264 g |
| What is the mass of 0.300 moles of Na2CO3.10H2O | 85.8 g |
| Calculate the number of moles of Al3+ ions in 5.10 g of Al2O3. | 0.1 |
| It was found that 1.00 g of vitamin C contains 0.00568 moles of Vitamin C molecules. Calculate the Mr of vitamin C. | 176 |
| 0.8500 g of hexanone, C6H12O, is converted into its 2,4-dinitrophenylhyrazone during its analysis. After isolation and purification, 2.1180 g of product C12H18N4O4 are obtained. Calculate the percentage yield. | 88.40% |
| What is the mass of X moles of Y? | X x Mr of Y |
| X moles of a substance has a mass of Y. What is its Mr? | Y/X |
| In what molar ratio do hydrochloric acid with calcium hydroxide react? | One to two |
| In what molar ratio do nitric acid with ammonia react? | One to one |
| What mass of aluminium reacts with 258 mg of chlorine? 2Al + 3Cl2 → 2AlCl3 | 0.0654g |
| In what molar ratio do sulfuric acid with barium hydroxide react? | One to One |
| In what molar ratio do nitric acid and pottasium carbonate react? | Two to One |
| "Deduce the limiting reagent and calculate what mass of magnesium oxide is formed when 486 mg of magnesium reacts with 240 mg of oxygen 2Mg + O2 → 2MgO | Oxygen. 0.605g |
| What is the atom economy of a reaction? | A ratio of the mass of desired product to the mass of all products |
| How is atom economy calculated? | (Mr or mass of desired product/Mr or mass of all products) x 100 |
| What is the atom economy to make tungsten in this reaction: WO3 + 3H2 → W + 3H2O | 77.30% |
| "Calculate the mass of aluminium oxide that would be formed when 2.70 g of aluminium reacts with 2.56 g of oxygen.4Al + 3O2 → 2Al2O3 | 5.10g |
| At 273 K and 101000 Pa, 6.319 g of a gas occupies 2.00 dm3 . Calculate the relative molecular mass of the gas. | 71 |
| Calculate the atom economy when titanium is extracted from titanium chloride. TiCl4 + 2Mg → Ti + 2MgCl2 | 20.10% |
| What standard units are used for concentration of a solution? | mol/dm3 |
| How are cm³ converted to dm³? | Divide by 1000 |
| What are concordant titres? | Titres within 0.1cm³ of each other |
| What colour is phenolphthalein in acid and alkali? | Colourless in acid, purple in alkali |
| State the ideal gas equation | PV = nRT |
| What is the empirical formula of a substance? | The formula that represents the simplest whole number ratio of the atoms of each element present in the compound. |
| What is the molecular formula? | The actual number of atoms of each element in one molecule of a compound |
| What is an ionic equation? | A simplified equation showing the ions present in a reaction |
| What is a spectator ion? | An ion that does not take part in a reaction |
| Which substances produce ions in ionic equations? | Aqueous solutions of ionic compounds |
| "Write an ionic equation, including state symbols, for the reaction of aqueous ammonia with hydrochloric acid | H+(aq) + NH3(aq) → NH4+(aq) |
| Write an ionic equation, including state symbols for the precipitation of lead(II) bromide when aqueous lead(II) nitrate is mixed with aqueous sodium bromide | Pb2+(aq) + 2Br–(aq) → PbBr2(s) |
| "Write an ionic equation, including state symbols, for the reaction of potassim carbonate solution with nitric acid | H+(aq) + CO32-(aq) → H2O + CO2(g) |
| Write an ionic equation, including state symbols for the precipitation of lead(II) iodide when aqueous lead(II) nitrate is mixed with aqueous potassium iodide | Pb2+(aq) + 2Br–(aq) → PbBr2(s) |
| What volume of carbon dioxide gas, measured at 800 K and 100 kPa, is formed when 1.00 kg of propane is burned in a good supply of oxygen? C3H8 + 5 O2 → 3 CO2 + 4 H2O | 4.53 m3 |
| 0.140 moles of a gas has a volume of 2.00 dm3 at a pressure of 90.0 kPa. Calculate the temperature of the gas | 155 K |
| "What volume of oxygen is required to burn the following gases, and what volume of carbon dioxide is produced? 1 dm3 of methane CH4(g) + 2 O2(g) → CO2(g) + 2 H2O(l) | O2 2 dm3 , CO2 1 dm3" |
| If 4 dm3 of hydrogen sulphide is burned in 10 dm3 of oxygen, what is the final volume of the mixture (give the volume of each gas at the end)? 2 H2S(g) + 3 O2(g) → 2 H2O(g) + 2 SO2(g) | 4 dm3 O2, 4 dm3 H2O, 4 dm3 SO2, total 12 dm3 gas |
| Calculate the number of moles in the following. 2 dm3 of 0.05 mol dm-3 HCl | 0.1 |
| "Calculate the number of moles in the following. 50 litres of 5 mol dm-3 H2SO4 | 250 |
| Calculate the number of moles in the following. 10 cm3 of 0.25 mol dm-3 KOH | 0.0025 |
| Calculate the concentration of the following in both mol dm-3 and g dm-3 0.400 moles of HCl in 2.00 litres of solution | 0.2 mol dm-3 , 7.3 g dm-3 |
| Calculate the concentration of the following in both mol dm-3 and g dm-3 12.5 moles of H2SO4 in 5.00 dm3 of solution | 2.5 mol dm-3 245.3 g dm-3 |
| Calculate the concentration of the following in both mol dm-3 and g dm-3 1.05 g of NaOH in 500 cm3 of solution | 0.0512 mol dm-3 , 2.10 g dm-3 |
| 25.0 cm3 of a solution of sodium hydroxide required 18.8 cm3 of 0.0500 mol dm-3 H2SO4. H2SO4 + 2 NaOH → Na2SO4 + 2 H2O Find the concentration of the sodium hydroxide solution in mol dm-3 | 0.0752 mol dm-3 |
| What volume of 5.00 mol dm-3 HCl is required to neutralise 20.0 kg of CaCO3? 2 HCl + CaCO3 → CaCl2 + H2O + CO2 | 79.9 dm3 |
| Limestone is mainly calcium carbonate. A student wanted to find what percentage of some limestone was calcium carbonate. A 1.00 g sample of limestone is allowed to react with 100 cm3 of 0.200 mol dm-3 HCl. The excess acid required 24.8 cm3 of 0.100 mol dm | 87.70% |
| An impure sample of barium hydroxide of mass 1.6524 g was allowed to react with 100 cm3 of 0.200 mol dm-3 hydrochloric acid. When the excess acid was titrated against 0.228 mol dm-3 sodium hydroxide in a back titration, 10.9 cm3 of sodium hydroxide soluti | 90.80% |
| Write the empirical formula of each of the following substances. a) C2H6 b) P2O3 c) SO2 d) C6H12 | a CH3 b P2O3 c SO2 d CH2 |
| " The empirical formula and relative molecular mass of some simple molecular compounds are shown below. Work out the molecular formula of each one. b) C2H5 Mr = 58 c) CH2 Mr = 70 e) CH Mr = 78 f) CH2 Mr = 42 | b) C4H10 c) C5H10 e) C6H6 f C3H6 |
| 50.0 g of a compound contains 22.4 g of potassium, 9.2 g of sulphur, and the rest oxygen. Calculate the empirical formula of the compound. | K2SO4 |
| A compound contains 40.0 g of carbon, 6.7 g of hydrogen and 53.5 g of oxygen. It has a relative molecular formula of 60. Find both the empirical and the molecular formula of the compound. | CH2O, C2H4O2 |
| A compound contains 59.4% carbon, 10.9% hydrogen, 13.9% nitrogen and 15.8% oxygen, by mass. Find the empirical formula of the compound. | C5H11NO |
| 25.0 cm3 of 0.0400 mol dm-3 sodium hydroxide solution reacted with 20.75 cm3 of sulphuric acid in a titration. Find the concentration of the sulphuric acid. | 0.0241 mol dm-3 |
Created by:
JBearfield
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