Inorganic Chemistry AQA AS and A2 Equations – Flashcards
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Chlorine and water
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Cl2 +H20 -> HClO (contains chlorate ion-strong oxidising-kills bacteria) + HCl
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Chlorine and water in sunlight
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2Cl2 + 2H20-> 4HCl (acidic) + 02
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Chlorine + alkali (production of sodium chlorate- bleach)]
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Cl2 + 2NaOH -> NaClO + NaCl + H20
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Sodium chlorate + water (alternative to chlorine +water to produce chloric acid (HClO) to kill bacteria in water)
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NaClO + H20-> Na+ + OH- + HClO (If alkali added, eqm shifts to left, so swimming pools eg. are kept slightly acidic)
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Acid base reaction of chloride ions with concentrated sulphuric acid
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Cl- + H2SO4 -> HSO4- +HCl (acidic fumes)
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Acid base reaction with bromide ions and conc H2SO4
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Br- + H2SO4 -> HSO4- + HBr (acidic white fumes)
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Redox reaction with bromide ions and conc H2SO4
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2Br- + 2H+ +H2SO4 -> Br2 + SO2 + 2H2O (SO2 is known as choking gas)
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Acid base reaction of iodide ions with conc H2SO4
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I- + H2SO4 -> HSO4- + HI (acidic white gas)
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Redox reaction 1 for iodide ions and conc H2SO4
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2I- + 2H+ +H2SO4 -> I2 + SO2 + 2H2O
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Redox reaction 2 of iodide ions and conc H2SO4
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6I- + 6H+ + H2SO4 -> 3I2 + S(yellow solid) + 4H2O
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Redox reaction 3 for iodide ions with conc H2SO4
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8I- + 8H+ +H2SO4 -> 4I2 + H2S + 4H2O
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Autocatalysis
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4Mn2+ + MnO4- + 8H+ -> 5Mn3+ +4H2O 2Mn3+ + C2O4 2- -> 2CO2 + 2Mn2+
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Catalysis: Peroxodisulphate ions with iodide ions
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2Fe2+ + S2O8 2- -> 2SO4 2- + 2Fe3+ 2Fe3+ + 2I- -> I2 + 2Fe2+ (Needs a catalyst because both reactants are negative ions and repel each other so reaction has a high activation energy)
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Catalysis: Contact Process
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2V2O5 + 2SO2 -> 2V2O4 + 2SO3 2V2O4 + O2 -> 2V2O5 (Used in production of sulphuric acid)
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Redox reaction in titration of MnO4- and Fe2+
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MnO4- + 5Fe2+ + 8H+ -> Mn2+ + 5Fe3+ + 4H2O
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Redox reaction in titration of MnO4- and C2O4 2-
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2MnO4- + 16H+ + 5C2O4 2- -> 2Mn2+ + 10CO2 + 8H2O
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Redox half equation for MnO4
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MnO4- + 8H+ + 5e- -> Mn2+ + 4H2O
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Redox half equation for C2O4 2-
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C2O4 2- -> 2CO2 + 2e-
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Redox half equation for Fe2+
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Fe2+ -> Fe3+ + e-
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Sodium + oxygen
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4Na + O2 ->2Na2O (basic)
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Magnesium + oxygen
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2Mg + O2 -> 2MgO (basic)
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Aluminium +oxygen
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4Al + 3O2 -> 2Al2O3 (amphoteric)
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Silicon + oxygen
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Si + O2 -> SiO2 (Silicon dioxide)
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Phosphorus + oxygen
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P4 + 5O2 -> P4O10 (acidic)
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Sulfur+ oxygen
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S + O2 -> SO2 S +3/2O2 -> SO3 (acidic)
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Sodium oxide + water
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Na2O + H2O -> 2NaOH (basic)
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Magnesium oxide + water
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MgO + H2O -> Mg(OH)2 (basic)
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Aluminium oxide + water
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Insoluble in water
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Silicon oxide + water
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Insoluble in water
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Phosphorus oxide + water
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P4O10 + 6H2O -> 4H3PO4 (phosphoric acid)
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Sulfur oxide + water
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SO2 +H2O -> H2SO3 (sulfurous acid) SO3 +H2O -> H2SO4 (sulfuric acid)
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Sodium oxide + acid
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Na2O + 2H+ -> 2Na+ + H2O
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Magnesium oxide + acid
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MgO + 2H+ -> Mg2+ + H2O
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Aluminium oxide + acid
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Al2O3 + 6H+ -> 2Al3+ + 3H2O
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Aluminium oxide + base (1)
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Al2O3+ 2OH- +3H2O -> 2Al(OH)4 -
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Aluminium oxide + base (2)
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Al2O3 + 6OH- + 3H20 -> 2Al(OH)6 3-
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Silicon oxide + base
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SiO2 + 2OH- -> SiO3 2- + H2O
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Phosphorus oxide + base
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P4O10 + 12OH- -> 4PO4 3- + 6H2O
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Sulfur oxide + base
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SO2 + 2OH- -> SO3 2- + H2O SO3 + 2OH- -> SO4 2- + H2O
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Sodium + water
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2Na + 2H2O -> 2NaOH + H2
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Magnesium + water
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Mg + 2H2O -> Mg(OH)2(s) + H2
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Aluminium hydroxide with base
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[Al(OH)3(H2O)3] + 3OH- -> [Al(OH)6]3- +3H2O
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Aluminium hydroxide with acid
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[Al(OH)3(H2O)3] + 3H+-> [Al(H2O)6]3+
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Alkaline hydrogen-oxygen fuel cell (+ve electrode)
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O2 + 2H2O + 4e- -> 4OH-
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Alkaline hydrogen-oxygen fuel cell (-ve electrode)
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4OH- + 2H2 -> 4H2O + 4e-
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Lithium cell (+ve electrode)
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Li-> Li+ + e-
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Lithium cell (-ve electrode)
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Li+ + CoO2 + e- -> LiCoO2
