Equations to remember

Description

Group 2 reactions, Extraction of metals reactions, Group 7 reactions, Ionic equation steps, Redox steps, Chlorine reactions
DauntlessAlpha
Flashcards by DauntlessAlpha, updated more than 1 year ago
DauntlessAlpha
Created by DauntlessAlpha over 10 years ago
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Question Answer
Write the equation for a reaction of a Group 2 metal with oxygen The group 2 metals will burn in oxygen. Mg burns with a bright white flame 2Mg(s) + O2(g) → 2MgO(s)
If testing for reaction rates with Mg and acid, why would uncleaned Mg give a false results? because both the Mg and MgO would react but at different rates. Mg + 2HCl → MgCl2 + H2 MgO + 2HCl → MgCl2 + H2O
Write an equation for the reaction of Mg with steam Mg (s) + H2O (g)→MgO (s) + H2 (g)
Write an equation for the reaction of Mg with warm water Mg + 2 H2O → Mg(OH)2 + H2
How to the rates of reaction compare for Mg's reaction with steam and warm water? Mg reacting with warm water is a much slower reaction and there's no flame (there's a bright white flame with steam)
What are the reactions of the other group 2 metals (not Mg) with COLD water? Ca+2H2O(l)→Ca(OH)2(aq)+H2 (g) Sr+2H2O(l)→Sr(OH)2(aq)+H2 (g) Ba+2H2O(l)→Ba(OH)2(aq)+H2 (g)
What observations would you expect to happen more vigorously down group 2 when it reacts with water? fizzing The metal dissolving The solution heating up With calcium a white precipitate appearing (less precipitate forms down group)
What's the reaction for the "milk of magnesia"? neutralises excess acid in the stomach and to treat constipation: Mg(OH)2 + 2HCl → MgCl2 + 2H2O
What's the chemical name for limewater and what reaction makes it turn milky white when testing for CO2 aqueous solution of calcium hydroxide white calcium carbonate is produced. Ca(OH)2(aq)+CO2(g)→CaCO3(s) +H2O(l)
What happens when Barium metal reacts with sulfuric acid? only react slowly as the insoluble Barium sulphate produced will cover the surface of the metal and act as a barrier to further attack. Ba + H2SO4 → BaSO4 + H2 The same effect will happen to a lesser extent with metals going up the group as the solubility decreases. The same effect does not happen with other acids like hydrochloric or nitric as they form soluble group 2 salts.
What's the simplest ionic equation when barium chloride is added to a solution with sulphate ions? Ba2+(aq)+SO4 2-(aq)→ BaSO4 (s)
How are sulphide ores converted to oxides? Roasted with oxygen
Give the equation for zinc sulphide being roasted in oxygen 2ZnS+3O2 → 2ZnO + 2SO2
Give the reaction for the reduction of iron oxides with Carbon and Carbon monoxide and state the conditions for each Fe2O3(s)+3CO(g)→2Fe(l)+3CO2(g) Occurs at about 1200degreesC Fe2O3(s)+3 C(s)→2Fe(l)+ 3 CO(g) Occurs at higher temps
What exothermic reaction keeps the blast furnace hot? C(s) + O2(g) → CO2(g)
What reaction produces the reducing agent in the blast furnace? C(s) + CO2 (g) → 2CO(g)
Give the reaction for copper and manganese for their extraction from their oxides MnO2 + C →  Mn + CO2 2CuO + C → 2Cu + CO2
Give the reaction for reactions of oxides of Tungsten and Titanium with carbon and state why it's not a way that works to reduce the metal TiO2(s)+3C(s)→TiC(s)+2CO(g) 2WO3+9C(g)→W2C3(s)+6CO(g) Reacts with the carbon to form carbide instead - impure
Give the reaction for the conversion of Titanium ore into chloride TiO2(s)+2C(s)+2Cl2(g)→TiCl4(g)+ 2CO(g)
Give the equation for the extraction of Titanium from its chloride by reduction with Magnesium or Sodium. Why is Argon used? TiCl4(g)+2Mg(l)→Ti(s)+2MgCl2(l) TiCl4(g)+4Na(l)→Ti(s)+4NaCl(l) Prevents the Mg and Na reacting with oxygen
Give the equation of the reaction of Tungsten with hydrogen gas and what role does H play in the reaction? WO3 + 3H2 → W + 3H2O Reducing agent
Give the half equations at the cathode and the anode for the extraction of aliminium cathode: Al 3+ + 3e- → Al(l) anode: 2O 2- → O2(g) + 4e-
Give the overall equation for the extraction of aliminium by electrolysis 2Al2O3 → 4Al(l) + 3O2(g)
Give 4 ways in which metal can be extracted also stating what is the general reaction happening during extraction The extraction of metals involves reduction, usually of metal oxides. •by heating with carbon (in the form of coke) •by heating with hydrogen •by heating with a more reactive metal (active metal) •by electrolysis
Give the reaction for the reduction of copper ions using scrap iron Cu 2+(aq)+Fe(s)→Cu(s)+Fe 2+(aq)
Give the equations and observations of the reaction of the halogens with Silver Nitrate solution Fluorides produce no precipitate Chlorides produce a white precipitate Ag+(aq) + Cl- (aq) →  AgCl(s) Bromides produce a cream precipitate Ag+(aq) + Br- (aq) → AgBr(s) Iodides produce a pale yellow precipitate Ag+(aq) + I- (aq) → AgI(s)
Give the equations and observations of the reaction of F- and Cl- ions with sulfuric acid and what role does the acid play? NaF(s)+H2SO4(l)→NaHSO4(s)+HF(g) Observations: White steamy fumes of HF are evolved. NaCl(s)+H2SO4(l)→NaHSO4(s)+ HCl(g) Observations: White steamy fumes of HCl are evolved. These are acid–base reactions and not redox. H2SO4 plays the role of an acid (proton donor).
Give the 2 step process of Br- ions reducing sulfuric acid Acid- base step: NaBr(s) + H2SO4(l)→NaHSO4(s) + HBr(g) Redox step: 2HBr + H2SO4 → Br2(g) + SO2(g) + 2H2O(l)
What are the oxidation and reduction half equations for the reduction of sulfuric acid by Br- ions? Ox ½ equation: 2Br-→Br2 + 2e- Re ½ equation H2SO4 + 2H+ +2e- →SO2+2H2O
How does the role of sulfuric acid differ in the two different steps in the reduction of it by bromide ions? H2SO4 plays the role of acid in the first step producing HBr and then acts as an oxidising agent in the second redox step
What are the 4 redox equations for reaction of Iodide with sulfuric acid? 1)NaI(s)+H2SO4(l)→NaHSO4(s)+HI(g) 2)2HI + H2SO4→I2(s)+SO2(g)+ 2H2O(l) 3)6HI+H2SO4→3I2+S(s)+4H2O(l) 4)8HI+H2SO4→4I2(s)+H2S(g)+ 4H2O(l)
What are the redox half equations for the reaction of iodide with sulfuric acid? Ox ½ equation: 2I- →  I2 + 2e- Re ½ equation: H2SO4 + 2H+ + 2e- → SO2 + 2H2O Re ½ equation: H2SO4+6H+ + 6e- → S + 4H2O Re ½ equation: H2SO4+8 H+ + 8e- → H2S+4 H2O
Give the equation for the reaction of between chlorine and water Cl2(aq) + H2O(l) → HClO(aq) + HCl (aq)
Give the equation of the reaction of Chlorine and water bright sunlight 2Cl2 + 2H2O →  4H+ + 4Cl- + O2
Give the equation for the reaction of chlorine with cold, dilute NaOH and state a use for the product Cl2(aq)+2NaOH(aq)→ NaCl(aq)+NaClO(aq)+H2O(l) The mixture of NaCl and NaClO is used as Bleach and to disinfect/ kill bacteria
Give the overall reaction between methane and chlorine in the presence of UV light CH4 + Cl2 → CH3Cl + HCl methane chloromethane
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