Write a note on entropy and spontaneity. - Vidyadip

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Write a note on entropy and spontaneity.

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Match the correct ionisation enthalpies and electron gain enthalpies of the following elements:

	Elements		$\Delta\text{H}_1$	$\Delta\text{H}_2$	$\Delta_{\text{eg}}\text{H}$
i.	Most reactive non metal	A.	419	3051	-48
ii.	Most reactive metal	B.	1681	3374	-328
iii.	Least reactive element	C.	738	1451	-40
iv.	Metal forming binary halide	D.	2372	5251	+8

Derive the relationship between $\Delta\text{H}$ and $\Delta\text{U}$ for an ideal gas. Explain each term involved in the equation.

Comment on following :
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(ii) Estimation of sulphur by Carius process

One mole of $H_2O$ and one mole of CO are taken in 10L vessel and heated to 725K. At equilibrium 40% of water (by mass) reacts with CO according to the equation,
$\text{H}_2\text{O (g) + CO (g)}\rightleftharpoons\text{H}_2\text{ (g) + CO}_2\text{ (g)}$
Calculate the equilibrium constant for the reaction.

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i. An athlete is given 100 g of glucose of energy equivalent to 1560 kJ . He utilises $50 \%$ of this gained energy in the event. In order to avoid storage of energy in the body, calculate the weight of water that would need to perspire. The enthalpy of vaporisation of water is $44 kJ mol ^{-1}$.
ii. Compound with carbon-carbon double bond, such as ethylene, $C _2 H _4$, add hydrogen in a reaction called hydrogenation, $C _2 H _4(g)+ H _2(g) \rightarrow C _2 H _6(g)$
Calculate enthalpy change for the reaction, using the following combustion data,

$\text{C}_2\text{H}_4(\text{g})+3\text{O}_2(\text{g})\overrightarrow{\ \ \ \ \ }\ 2\text{CO}_2(\text{g})+2\text{H}_2\text{O(l)};$ $\Delta_\text{c}\text{H}^\circ=-1401\text{kJ mol}^{-1}\dots(\text{i})$

$\text{C}_2\text{H}_6(\text{g})+\frac{7}{2}\text{O}_2(\text{g})\overrightarrow{ \ \ \ \ \ \ \ }\ 2\text{CO}_2(\text{g})+3\text{H}_2\text{O(l)}$ $\Delta_\text{c}\text{H}^\circ=-1550\text{kJ mol}^{-1}\dots(\text{ii})$

$\text{H}_2(\text{g})+\frac{1}{2}\text{O}_2(\text{g})\overrightarrow{ \ \ \ \ }\ \text{H}_2\text{O(l)};$ $\Delta_\text{c}\text{H}^\circ=-286.0\text{kJ mol}^{-1}\dots(\text{iii})$

Write the expression for the equilibrium constant, $K _{ C }$ for each of the following reactions:
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b. $2 Cu \left( NO _3\right)_2(s) \rightleftharpoons 2 CuO ( s )+4 NO _2(g)+ O _2(g)$
c. $CH _3 COOC _2 H _5( aq )+ H _2 O ( l ) \rightleftharpoons CH _3 COOH ( aq )+ C _2 H _5 OH ( aq )$
d. $Fe ^{3+}( aq )+3 OH ^{-}( aq ) \rightleftharpoons Fe ( OH )_3(s)$
e. $I _2(s)+5 F_2 \rightleftharpoons 2 IF _5$

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State Le Chatelier's principle.
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