Question

B. Select the correct answer from the list given in the brackets:
i. An aqueous electrolyte consists of the ions mentioned in the list, the ion which could be discharged most readily during electrolysis. (Fe2+, Cu2+, Pb2+, H+)
ii. The graph of PV vs P for a gas is…… (Parabolic, hyperbolic, a straight line parallel to X-axis, a straight line passing through the origin.)
iii. During silver plating of an article using potassium argentocyanide as an electrolyte, the anode should be ………… (Cu, Ag, Pt, Fe)
iv. The relationship between volume of a dry gas and temperature is given by………….. (Boyle’s law, Charle’s law, Gay-Lussac’s law)
v. The aqueous solution of a compound which contains both ions and molecules is………….. (H2SO4, HCl, HNO3, CH3COOH)

C. Answer the following briefly:
i. Why do mountaineers carry oxygen cylinders with them? ii. Pure nitric acid is colourless, but the acid obtained in the laboratory is slightly yellow. Explain.
iii. What is the mass of 4.5 moles of sodium carbonate? (RMM of Sodium carbonate is 83)
iv. Only molecules are present in sugar solution. Why?
v. Why is concentrated Sulphuric acid used for the preparation of nitric acid?
vi. What is passivity?
vii. Why is electrolysis of water considered as an example of catalysis?
viii. Copper though a good conductor of electricity is a non-electrolyte. Explain.
ix. Calculate the number of atoms in 35.5g Cl2. (Cl=35.5).
x. Calculate the gram atoms in 160g of SO2. (S=32, O=16).

D. State your observations for the following:
i. At anode during electrolysis of acidulated water
. ii. At cathode during electrolysis of molten lead bromide.
iii. Thermal decomposition of potassium nitrate.
iv. Nitric acid is exposed to sunlight.
v. At anode during electrolysis of molten lead bromide.

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E. Match the following pairs:
(GAM of H=1, O=16, C=12, S=32)

F. Give a balanced chemical equation for the reactions given below: [5]
i. Magnesium reacts with 1% dil. Nitric acid.
ii. Potassium sulphite reacts with dil. Nitric acid.
iii. Iron is oxidized using conc. Nitric acid.
iv. Electroplating of Nickel using aqueous Nickel sulphate.

G. 4.5 moles of calcium carbonate are reacted with dilute hydrochloric acid. [5] (Ca=40, C=12,O=16, H=1, Cl=35.5)
i. Write the equation for the reaction.
ii. What is the mass of 4.5 moles of calcium carbonate? (GMM of calcium carbonate= 100).
iii. What is the volume of carbon dioxide liberated at STP?
iv. What is the mass of Calcium Chloride formed?
v. How many moles of HCl are used in the reaction?

Answer 1

Answer:

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