Flashcards
Equations to remember
Cards in this deck (36)
- 1Write the equation for a reaction of a Group 2 metal with oxygenThe group 2 metals will burn in oxygen.
Mg burns with a bright white flame
2Mg(s) + O2(g) → 2MgO(s) - 2If 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 - 3Write an equation for the reaction of Mg with steamMg (s) + H2O (g)→MgO (s) + H2 (g)
- 4Write an equation for the reaction of Mg with warm waterMg + 2 H2O → Mg(OH)2 + H2
- 5How 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)
- 6What 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) - 7What 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) - 8What's the reaction for the "milk of magnesia"?neutralises excess acid in the
stomach and to treat constipation:
Mg(OH)2 + 2HCl → MgCl2 + 2H2O - 9What's the chemical name for limewater and what reaction makes it turn milky white when testing for CO2aqueous solution of calcium hydroxide
white calcium carbonate is produced.
Ca(OH)2(aq)+CO2(g)→CaCO3(s) +H2O(l) - 10What 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. - 11What's the simplest ionic equation when barium chloride is added to a solution with sulphate ions?Ba2+(aq)+SO4 2-(aq)→ BaSO4 (s)
- 12How are sulphide ores converted to oxides?Roasted with oxygen
- 13Give the equation for zinc sulphide being roasted in oxygen2ZnS+3O2 → 2ZnO + 2SO2
- 14Give the reaction for the reduction of iron oxides with Carbon and Carbon monoxide and state the conditions for eachFe2O3(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 - 15What exothermic reaction keeps the blast furnace hot?C(s) + O2(g) → CO2(g)
- 16What reaction produces the reducing agent in the blast furnace?C(s) + CO2 (g) → 2CO(g)
- 17Give the reaction for copper and manganese for their extraction from their oxidesMnO2 + C → Mn + CO2
2CuO + C → 2Cu + CO2 - 18Give 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 metalTiO2(s)+3C(s)→TiC(s)+2CO(g)
2WO3+9C(g)→W2C3(s)+6CO(g)
Reacts with the carbon to form carbide instead - impure - 19Give the reaction for the conversion of Titanium ore into chlorideTiO2(s)+2C(s)+2Cl2(g)→TiCl4(g)+ 2CO(g)
- 20Give 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 - 21Give 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 - 22Give the half equations at the cathode and the anode for the extraction of aliminiumcathode: Al 3+ + 3e- → Al(l)
anode: 2O 2- → O2(g) + 4e- - 23Give the overall equation for the extraction of aliminium by electrolysis2Al2O3 → 4Al(l) + 3O2(g)
- 24Give 4 ways in which metal can be extracted also stating what is the general reaction happening during extractionThe 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 - 25Give the reaction for the reduction of copper ions using scrap ironCu 2+(aq)+Fe(s)→Cu(s)+Fe 2+(aq)
- 26Give the equations and observations of the reaction of the halogens with Silver Nitrate solutionFluorides 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) - 27Give 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). - 28Give the 2 step process of Br- ions reducing sulfuric acidAcid- base step:
NaBr(s) + H2SO4(l)→NaHSO4(s) + HBr(g)
Redox step:
2HBr + H2SO4 → Br2(g) + SO2(g) + 2H2O(l) - 29What 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 - 30How 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 - 31What 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) - 32What 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 - 33Give the equation for the reaction of between chlorine and waterCl2(aq) + H2O(l) → HClO(aq) + HCl (aq)
- 34Give the equation of the reaction of Chlorine and water bright sunlight2Cl2 + 2H2O → 4H+ + 4Cl- + O2
- 35Give the equation for the reaction of chlorine with cold, dilute NaOH and state a use for the productCl2(aq)+2NaOH(aq)→ NaCl(aq)+NaClO(aq)+H2O(l)
The mixture of NaCl and NaClO is used as Bleach and to disinfect/ kill bacteria - 36Give the overall reaction between methane and chlorine in the presence of UV lightCH4 + Cl2 → CH3Cl + HCl
methane chloromethane
Information
- Description
- Group 2 reactions, Extraction of metals reactions, Group 7 reactions, Ionic equation steps, Redox steps, Chlorine reactions
- Created by
- DauntlessAlpha
- Views
- 284
- Tags
- Rating