For the reaction at 298K,2A+B⟶C ΔH=...
Question
For the reaction at 298K,2A+B⟶C ΔH=100kcal and ΔS=0.050kcalK−1. If ΔH and ΔS are assumed to be constant over the temperature range, above what temperature will the r
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For the reaction at ( 298 mathrm{K}, 2 mathrm{A}+mathrm{B} longrightarrow mathrm{C} ) ( Delta mathrm{H}=100 mathrm{kcal} ) and ( Delta mathrm{S}=0.050 mathrm{kcal} mathrm{K}^{-1} . ) If ( Delta mathrm{H} ) and ( Delta mathrm{S} ) are assumed to be constant over the temperature range, above what temperature will the reaction become spontaneous?
(A) ( 1000 mathrm{K} )
(B) ( 1500 mathrm{K} )
(C) ( 2000 mathrm{K} )
(D) ( 2500 mathrm{K} )

JEE/Engineering Exams
Chemistry
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For the reaction at 298K,2A+B⟶C ΔH=100kcal and ΔS=0.050kcalK−1. If ΔH and ΔS are assumed to be constant over the temperature range, above what temperature will the reaction become spontaneous?
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ΔC = 0

ΔH = TΔS = 0

ΔH = TΔS

(T= frac{ΔH}{ΔS})

  = (frac{100}{0.050})

  = (frac{100 times 10}{50})  

  = 2000k

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