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A. Sulphur dioxide
The solution turns from orange to green
B. The gas B is basic
Ammonia
C. Hydrogen chloride
Ammonium chloride
Neutralisation reaction
D. It is acidic in nature
Chlorine

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. Colourless
. Odourless
. Tastless
. It is neutral towards moist litmus paper
. A glowing splinter starts to burn in prescence of oxygen.

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Heat heavy metallic gases
(on heat)
Heavy metallic oxide -----> Metal oxide/ metal

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. Colourless
. Orourless
. Tasteless gas
. Neutral towards moist litmus paper
. A burning splinter is brought near it, it burns with a pale blue flame and a pop sound is heard.

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- colorless
- odorless
- It turns lime water milky and has no effect on potassium dichromate(acidified)
- acidic in nature

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It is colourless gas and it has a smell of rotten eggs
It is an acidic gas.
It turns moist lead acetate paper black.

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Add dil. acid to any carbonate
CaCO3 + HCl ——> CaCl2 + H20 + CO2 (laboratory preparation)
Heating of metallic carbonates:
CuCO3 ——> CuO + CO2

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- Colourless
- Odourless
- Neutral towards litmus.
- Turns blue cobalt chloride paper pink.
- Turns white anhydrous copper sulphate blue.

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Add dilute HCl or dilute H2SO4 to reactive metals  like magnesium, zinc, iron etc.( metals above hydrogen in reactivity series.
( on heat)
Active metal+dil acid -------> salt + hydrogen

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- Colourless
- Odourless

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It is a reddish brown gas and it has a pungent and a irritating smell.
It is an acidic gas.
It turns moist potttasium iodide paper brown.

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Add dil. HCl do dil. H2SO4 to metallic sulphides
FeS + H2SO4 ——> FeSO4 + H2S

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Heat a crystalline substance like hydrated sodium like hydrated sodium carbonate.
(on heat)
Hydrated salt --------> Anhydrous salt+ water vapour

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Heat a heavy metal nitrate
2Cu(NO3)2 + heat ——> 2CuO + O2 + 4NO2

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- colorless
- very little smell of burnt Sulphur
- Acidic in nature
- It turns acidified potassium dichromate green.

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. Nitric oxide (N2O)
. Nitrous oxide (NO2)

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Add dil. HCl or dil. H2SO4 to metallic sulphites
Na2SO3 + 2HCl ——> 2NaCl + H2O + SO2

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heating an aqueous solution of ammonium chloride and sodium nitrite.

ammonium dichromate -------> water+ chromium (III)oxide + nitrogen

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a)Nitrogen dioxide
b)sulphur dioxide
c)oxygen

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a. The gas is hydrogen sulphide(H2S). Moist lead acetate paper turns silvery grey when exposed to H2S.
b. Sulphur and hydrogen

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i) the gas in setup A is basic in nature. The gas in srt up B in acidic in nature.
ii) The deposit x seen is
iii) The gas released is Carbon Dioxide.
iv) We can confirm that the gas evolved in setup B is Carbon Dioxide as it does not have any effect acidified potassium dichromate.
v) The deposit in C is Copper Sulphate as it is a blue hydrous salt.
vi) Deposit Y is Copper sulphate.If the gas produced turns moist cobalt chloride paper pink then it is water vapour thus the copper sulphate is formed.And when water is added to copper sulphate, if it turns blue it is copper sulphate
vii)When the sample D is heated for a long time then the solid iodine would change into iodine gas which is violet in colour.Thus we can tell that the substance in sample D which is iodine is easily sublimable.
viii)The residue formed is PbO which is reddish brown when hot and is yellow on cold.It also sticks to the sides of the test tube due to which it is very difficult to remove the residue.
(ix) This gas is NO2 / Nitrogen dioxide. It turns moist potassium iodide paper brown.
(x) The other gas released in the Setup E is Oxygen. A glowing splinter starts to burn in the presence of this gas.
(xi) .A: NH4Cl ---> NH3 + HCl
B: CuCO3 ---> CuO + CO2
C: CuSO4.5H2O ---> CuSO4 + 5 H2O
D: I2 ---> I 2
E:  Pb(NO3)2 ---> 2 PbO + 4 NO2 + O2
(xii) Thermal Decompostition:
B, C, E ( As one reactant gives multiple products on heating.)

Thermal Dissociation:
A ( As it is a reversable thermal decomposition reaction )

None:
D ( As there is only 1 reactant and 1 product )