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Which of the following equation depicts reducing nature of \[\ce{H2O2}\]?
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Some of the properties of water are described below. Which of them is/are not correct?
(i) Water is known to be a universal solvent.
(ii) Hydrogen bonding is present to a large extent in liquid water.
(iii) There is no hydrogen bonding in the frozen state of water.
(iv) Frozen water is heavier than liquid water.
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If same mass of liquid water and a piece of ice is taken, then why is the density of ice less than that of liquid water?
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Give reasons: Lakes freeze from top towards bottom.
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Give reasons: Ice floats on water.
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\[\ce{H2O2}\] is a better oxidising agent than water. Explain.
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Melting point, enthalpy of vapourisation and viscosity data of \[\ce{H2O}\] and \[\ce{D2O}\] is given below :
| \[\ce{H, O}\] | \[\ce{D2O}\] | |
| Melting point / K | 373.0 | 374.4 |
| Enthalpy of vapourisation at (373 K)/kJ mol–1 | 40.66 | 41.61 |
| Viscosity/centipoise | 0.8903 | 1.107 |
On the basis of this data explain in which of these liquids intermolecular forces are stronger?
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Explain why \[\ce{HCl}\] is a gas and \[\ce{HF}\] is a liquid.
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Why does water show high boiling point as compared to hydrogen sulphide? Give reasons for your answer.
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How will you account for 104.5° bond angle in water?
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Write two reactions to explain amphoteric nature of water.
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Which of the following are the correct reasons for anomalous behaviour of lithium?
(i) Exceptionally small size of its atom.
(ii) Its high polarising power.
(iii) It has high degree of hydration.
(iv) Exceptionally low ionisation enthalpy.
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Write the general outer electronic configuration of f- block elements.
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An element with mass number 81 contains 31.7% more neutrons as compared to protons. Assign the atomic symbol.
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An ion with mass number 37 possesses one unit of negative charge. If the ion contains 11.1% more neutrons than the electrons, find the symbol of the ion.
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An ion with mass number 56 contains 3 units of positive charge and 30.4% more neutrons than electrons. Assign the symbol to this ion.
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What is Kc for the following equilibrium when the equilibrium concentration of each substance is: [SO2] = 0.60 M, [O2] = 0.82 M and [SO3] = 1.90 M?
\[\ce{2SO2(g) + O2(g) ⇌ 2SO3(g)}\]
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Write the expression for the equilibrium constant, Kc for each of the following reactions:
\[\ce{2NOCl (g) ⇌ 2NO (g) + Cl2 (g)}\]
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Write the expression for the equilibrium constant, Kc for the following reactions:
\[\ce{2Cu(NO3)2 (s) ⇌ 2CuO (s) + 4NO2 (g) + O2 (g)}\]
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Write the expression for the equilibrium constant, Kc for the following reactions:
\[\ce{CH3COOC2H5(aq) + H2O(l) ⇌CH3COOH (aq) + C2H5OH (aq)}\]
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