Question
- Arrange Fe, Fe2+, Fe3+ in increasing order of radii.
- Explain why Be has higher ionization enthalpy than B.
- Predict the formula of compound which might be formed by silicon and bromine.
✓
Answer
- Fe3+ < Fe2+ < Fe is an increasing order of ionic radii.
- Be (4) has electronic configuration 1s2 2s2 whereas B(5) has 1s2 2s2 2p1.
The energy required to remove electron from completely filled 2s orbital is higher than the energy required to remove electron from 2p orbital.
- SiBr4 is a formula of compound which might be formed by Si and Br2.
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Ethyl acetate is formed by the reaction between ethanol and acetic acid and the equilibrium is represented as :
$CH _3 COOH ( l )+ C _2 H _5 OH ( l ) \rightleftharpoons CH _3 COOC _2 H _5( l )$$+ H _2 O ( l )$
(i) Write the concentration ratio (reaction quotient) $Q_c$, for this reaction (note : water is not in excess and is not a solvent in this reaction).
(ii) At 293 K , if one starts with 1.00 mol of acetic acid and 0.18 mol of ethanol, there is 0.171 mol of ethyl acetate in the final equilibrium mixture. Calculate the equilibrium constant.
(iii) Starting with 0.5 mol of ethanol and 1.0 mol of acetic acid and maintaining it at $293 K, 0.214 mol$ of ethyl acetate is found after sometime. Has equilibrium been reached?
→$CH _3 COOH ( l )+ C _2 H _5 OH ( l ) \rightleftharpoons CH _3 COOC _2 H _5( l )$$+ H _2 O ( l )$
(i) Write the concentration ratio (reaction quotient) $Q_c$, for this reaction (note : water is not in excess and is not a solvent in this reaction).
(ii) At 293 K , if one starts with 1.00 mol of acetic acid and 0.18 mol of ethanol, there is 0.171 mol of ethyl acetate in the final equilibrium mixture. Calculate the equilibrium constant.
(iii) Starting with 0.5 mol of ethanol and 1.0 mol of acetic acid and maintaining it at $293 K, 0.214 mol$ of ethyl acetate is found after sometime. Has equilibrium been reached?
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→
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→Determine the molecular formula of an oxide of iron, in which the mass per cent of iron and oxygen are 69.9 and 30.1, respectively.
Note: Given that the molar mass of the oxide is 159.69g mol-1
Note: Given that the molar mass of the oxide is 159.69g mol-1
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Calculate the volume of 02 at STP liberated by heating 12.25g of KClO3
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(At. wt. of K = 39, Cl = 35.5, 0 = 16u)