Chemical Reactions and Equations Flashcards
Calcium oxide and water
CaO + H2O»_space; Ca(OH)2
Calcium Carbonate is heated
CaCO3»_space; CO2 + CaO
Calcium Hydroxide and Carbon Dioxide
Ca(OH)2 + CO2»_space; CaCO3 + H2O
Methyl Alcohol
CH3OH
Potassium Chlorate
KClO
Magnesium + Oxygen
2Mg + O2»_space; 2MgO
Sulphuric Acid
H2SO4
Zinc + Sulphuric Acid
Zn + H2SO4»_space; ZnSO4 + H2
zinc sulphate
Iron(4) + Water
3 Fe + 4 H2O»_space; Fe3O4 + 4 H2
CaO + H2O
Ca(OH)2 + Heat
Quick lime
CaO (s)
Slaked Lime
Ca(OH)2 (aq)
Observations when we add water to quick lime
Rise in the temperature, formation of bubbles
Formation of white ppt [Ca(OH)2 or slaked lime]
Burning of coal
C + O2»_space; CO2
Formation of water
O2 + 2H2»_space; 2H2O
Burning of gas (Methane)
CH4 + 2O2»_space; CO2 + 2H2O
Is respiration exothermic
Yes, it releases energy from food molecules
3 examples of exothermic reactions
- Burning of natural gas
- Respiration
- Decomposition
Ferrous Sulphate is heated
2FeSO4»_space; Fe2O3 + SO2 + SO3
Ferric oxide
Sulphur Dioxide/Trioxide
Ferrous Sulphate Crystals are heated
eqn + obs
FeSO4.7H2O»_space; FeSO4
light green to white
Anhydrous Ferrous Sulphate
Ferrous Sulphate is heated observations
reddish brown solid is left out (Fe2O3)
smell of a gas having the odour of burning sulphur
Lime Stone
CaCO3
Calcium carbonate is heated
CaCO3»_space; CO2 + CaO
Quick Lime uses
CaO
white washing
manufacturing of cement, paper
preparing bleaching powder
calcium hydroxide uses
sewage treatment,
paper production,
food processing.
Lead nitrate is heated
2Pb(NO3)2»_space; O2 + 4NO2 + 2PbO
nitrogen dioxide
lead oxide
Silver Chloride in sun
2AgCl»_space; Cl2 + 2Ag
Silver Bromide in sun
2AgBr»_space; Br2 + 2Ag
Silver bromide and chloride are used for
bnw photography
Barium Hydroxide and Ammonium chloride
Ba(OH)2 + 2NH4Cl»_space; BaCl2 + 2NH3 + 2H2O
endothermic
Electrolysis
Process of decomposing ionic compounds into their elements by passing a direct electric current through the compound in a fluid form
In electrolysis of water, which gas is formed where
oxygen at the anode
hydrogen at the cathode
Iron and copper sulphate
Fe + CuSO4»_space; FeSO4 + Cu
Iron and Copper sulphate: observations
Iron nail has red coating (Cu deposit)
Blue CuSO4 becomes green (FeSO4)
Zinc + copper sulphate
Zn + CuSO4»_space; ZnSO4 + Cu
Lead and copper chloride
Pb + CuCl2»_space; PbCl2 + Cu
sodium sulphate and barium chloride
Na2SO4 + BaCl2»_space; 2NaCl + BaSO4
sodium sulphate and barium chloride obs
white ppt is formed (BaSO4)
Copper and oxygen
eqn obs
Black substance on copper powder
Copper Oxide (CuO)
2Cu + O2»_space; 2CuO
Copper oxide and hydrogen
eqn obs
CuO + H2»_space; Cu + H2O
black turns brown (Cu)
Redox
A reaction where one reactant gets oxidised, the other gets reduced simultaneously
Zinc oxide and carbon
ZnO + C»_space; CO + Zn
Manganese dioxide and Hydrochloric acid
MnO2 + 4HCl»_space; MnCl2 + Cl2 + 2H2O
Potassium iodide + Lead nitrate
2KI + Pb(NO3)2»_space; PbI2 + 2KNO3
Potassium iodide + Lead nitrate obs
yellow ppt is formed (lead iodide)
example of endothermic reaction
Ba(OH)2 + 2NH4Cl»_space; BaCl2 + 2NH3 + 2H2O