733114
Description
Flashcards by DauntlessAlpha, updated more than 1 year ago
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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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