Short Answer TypeWater is a liquid while hydrogen sulphide is a gas. Explain.
The intermolecular forces, namely hydrogen-bonding, in H2O are stronger than in H2S. This is because in H2O the bonds are more ionic and there is a larger partial positive charge on H and partial negative on O, so neighboring H2O molecules can bind to each other and cause a stronger network of bonded molecules, thus requiring more energy (higher temperature) to break these bonds and form a gas (where intermolecular forces no longer act).
Nitrogen and chlorine have the same electronegativity but only former shows intermolecular hydrogen bonding. Discuss.
Long Answer TypeGive reasons for the following:
(i) The density of water is maximum at 277 K (4°C).
(ii) Why glycerol (glycerine) is more viscous than ethyl alcohol?
Short Answer TypeCalcualte the total pressure in a mixture of 8 g of dioxygen and 4 g of dihydrogen confined in a vessel of 1 dm3 at 
. R = 0.083 bar dm3 K-1 mol-1.
A mixture of dihydrogen and dioxygen at one bar pressure contains 20% by weight of dihydrogen. Calculate the partial pressure of dihydrogen.
Multiple Choice QuestionsIf average velocity of a sample of gas molecules at 300 K is 5 cm s-1, what is RMS velocity of same sample of gas molecules at the same temperature? (Given, α: u: v = 1:1.224: 1.127)
6.112 cm/s
4.605 cm/s
4.085 cm/s
5.430 cm/s
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