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Question

Variation of equilibrium constant K for the reaction ; 2A(s)+B(g)C(g)+2D(g) is plotted against absolute T in figure as- lnKVs(1/T) :

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A
the forward reaction is exothermic
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B
the forward reaction is endothermic
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C
the slope of line is proportional to ΔH
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D
adding 'A' favours forward reaction
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E
removing C favours forward reaction
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Solution

The correct options are
A the forward reaction is exothermic
C the slope of line is proportional to ΔH
D adding 'A' favours forward reaction
E removing C favours forward reaction
The relation between Equilibrium constant and Temperature is given by Van't Hoff equation,
lnKeq=ΔH0RT+ΔS0R.
For the lnKeqvs1T plot, ΔH0R is the slope.
The graph suggests positive slope, hence ΔH0R is positive or ΔH0 is negative. Hence, the reaction is exothermic. Slope line is proportional to ΔH Also, by Le Chatelier's principle, removing C favours forward reaction.

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