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Assertion (A): Though the central atom of both \[\ce{NH3}\] and \[\ce{H2O}\] molecules are sp3 hybridised, yet \[\ce{H -N - H}\] bond angle is greater than that of \[\ce{H - O - H}\].
Reason (R): This is because nitrogen atom has one lone pair and oxygen atom has two lone pairs.
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The volume of gas is reduced to half from its original volume. The specific heat will be ______.
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Heat capacity (Cp) is an extensive property but specific heat (c) is an intensive property. What will be the relation between Cp and c for 1 mol of water?
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For the reaction \[\ce{H2 (g) + I2 (g) ⇌ 2HI (g)}\], the standard free energy is ∆GΘ > 0. The equilibrium constant (K ) would be ______.
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On increasing the pressure, in which direction will the gas phase reaction proceed to re-establish equilibrium, is predicted by applying the Le Chatelier’s principle. Consider the reaction.
\[\ce{N2 (g) + 3H2 (g) ⇌ 2NH3 (g)}\]
Which of the following is correct, if the total pressure at which the equilibrium is established, is increased without changing the temperature?
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At 500 K, equilibrium constant, \[\ce{K_c}\], for the following reaction is 5.
\[\ce{1/2 H2 (g) + 1/2 I2 (g) ⇌ HI (g)}\]
What would be the equilibrium constant \[\ce{K_c}\] for the reaction
\[\ce{2HI (g) ⇌ H2 (g) + I2 (g)}\]
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For the reaction : \[\ce{N2 (g) + 3H2 (g) ⇌ 2NH3 (g)}\]
Equilibrium constant `K_C = ([NH3]^2)/([N_2][H_2]^3)`
Some reactions are written below in Column I and their equilibrium constants in terms of Kc are written in Column II. Match the following reactions with the corresponding equilibrium constant
| Column I (Reaction) | Column II (Equilibrium constant) |
| (i) \[\ce{2N2 (g) + 6H2 (g) ⇌ 4NH3 (g)}\] | (a) `2K_c` |
| (ii) \[\ce{2NH3 (g) ⇌ N2 (g) + 3H2 (g)}\] | (b) `K_c^(1/2)` |
| (iii) \[\ce{1/2 N2 (g) + 3/2 H2 (g) ⇌ NH3 (g)}\] | (c) `1/K_c` |
| (d) `K_c^2` |
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Match standard free energy of the reaction with the corresponding equilibrium constant.
| Column I | Column II |
| (i) ∆GΘ > 0 | (a) K > 1 |
| (ii) ∆GΘ > 0 | (b) K = 1 |
| (iii) ∆GΘ = 0 | (c) K = 0 |
| (d) K < 1 |
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The more positive the value of EΘ, the greater is the tendency of the species to get reduced. Using the standard electrode potential of redox couples given below find out which of the following is the strongest oxidising agent.
EΘ values: \[\ce{Fe^{3+} / Fe^{2+} = + 0.77; I2 (s) / I- = + 0.54}\];
\[\ce{Cu^{2+} / Cu = + 0.34; Ag+ / Ag = + 0.80V}\]
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Using the standard electrode potential, find out the pair between which redox reaction is not feasible.
EΘ values: \[\ce{Fe^{3+} / Fe^{2+} = + 0.77; I2/I- = + 0.54}\];
\[\ce{Cu^{2+} / Cu = + 0.34; Ag+ / Ag = + 0.80 V}\]
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Thiosulphate reacts differently with iodine and bromine in the reactions given below:
\[\ce{2S2O^{2-}3 + I2 -> S4O^{2-}6 + 2I-}\]
\[\ce{S2O^{2-}3 + 2Br2 + 5H2O -> 2SO^{2-}4 + 2Br- + 10H+}\]
Which of the following statements justifies the above dual behaviour of thiosulphate?
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Identify the correct statement (s) in relation to the following reaction:
\[\ce{Zn + 2HCl -> ZnCl2 + H2}\]
(i) Zinc is acting as an oxidant.
(ii) Chlorine is acting as a reductant.
(iii) Hydrogen ion is acting as an oxidant.
(iv) Zinc is acting as a reductant.
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Which of the following electrodes will act as anodes, when connected to Standard Hydrogen Electrode?
(i) \[\ce{Al/Al^{3+}; E^Θ = –1.66}\]
(ii) \[\ce{Fe/Fe^{2+}; E^Θ = – 0.44}\]
(iii) \[\ce{Cu/Cu2+ ; E^Θ = + 0.34}\]
(iv) \[\ce{F2 (g)/2F– (aq); E^Θ = + 2.87}\]
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On the basis of standard electrode potential values, suggest which of the following reactions would take place? (Consult the book for EΘ value).
\[\ce{Cu + Zn^{2+} -> Cu^{2+} + Zn}\]
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On the basis of standard electrode potential values, suggest which of the following reactions would take place? (Consult the book for EΘ value).
\[\ce{Mg + Fe^{2+} -> Mg^{2+} + Fe}\]
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On the basis of standard electrode potential values, suggest which of the following reactions would take place? (Consult the book for EΘ value).
\[\ce{Br2 + 2Cl- -> Cl2 + 2Br-}\]
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On the basis of standard electrode potential values, suggest which of the following reactions would take place? (Consult the book for EΘ value).
\[\ce{Fe + Cd^{2+} -> Cd + Fe^{2+}}\]
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Which method can be used to find out strength of reductant/oxidant in a solution? Explain with an example.
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Which of the following reactions is an example of use of water gas in the synthesis of other compounds?
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