Chemistry · Chemical Kinetics

JEE Advanced 2021 — Paper 1 — Question 40

The value of standard enthalpy,   ⁣ ⁣Δ ⁣ ⁣ H⊖(inkJmol−1)\text{ }\!\!\Delta\!\!\text{ }{{H}^{\ominus }}\left( \text{inkJmo}{{\text{l}}^{-1}} \right) for the given reaction is   ⁣ ⁣  ⁣ ⁣ \text{ }\!\!~\!\!\text{ } .

Answer: 166.28

Numerical answer — enter this value.

Step-by-step solution

\begin{array}{*{35}{r}}{} & X\left( s \right)\rightleftharpoons Y\left( s \right)+Z\left( g \right) \\ {} & \begin{array}{*{35}{r}}{} & {{K}_{p}}=\frac{{{p}_{z}}}{{{p}^{0}}},\text{ }\!\!~\!\!\text{ also }\!\!~\!\!\text{ }\!\!\Delta\!\!\text{ }{{G}^{0}}=-RT\text{ln}{{k}_{p}} \\{} & ~=-RT\text{ln}\left(\frac{{{p}_{z}}}{{{p}^{0}}} \right) \\\end{array} \\\end{array}

Now,   ⁣ ⁣Δ ⁣ ⁣ G0=  ⁣ ⁣Δ ⁣ ⁣ H0−T  ⁣ ⁣Δ ⁣ ⁣ S0\text{ }\!\!\Delta\!\!\text{ }{{\text{G}}^{0}}=\text{ }\!\!\Delta\!\!\text{ }{{\text{H}}^{0}}-\text{T }\!\!\Delta\!\!\text{ }{{\text{S}}^{0}} -RT kn (pzp0)=  ⁣ ⁣Δ ⁣ ⁣ H0−T  ⁣ ⁣Δ ⁣ ⁣ S0\left( \frac{{{p}_{z}}}{{{p}^{0}}} \right)=\text{ }\!\!\Delta\!\!\text{ }{{H}^{0}}-T\text{ }\!\!\Delta\!\!\text{ }{{S}^{0}}

ln(pzp0)=−(  ⁣ ⁣Δ ⁣ ⁣ H0R)1T+  ⁣ ⁣Δ ⁣ ⁣ S0R#(1)\begin{matrix}ln\left( \frac{{{p}_{z}}}{{{p}^{0}}} \right)=-\left( \frac{\text{ }\!\!\Delta\!\!\text{ }{{H}^{0}}}{R} \right)\frac{1}{T}+\frac{\text{ }\!\!\Delta\!\!\text{ }{{S}^{0}}}{R}\#\left( 1 \right) \\\end{matrix}

(1) ⇒ln(pzp0)=−(  ⁣ ⁣Δ ⁣ ⁣ H0104R)×104  ⁣ ⁣  ⁣ ⁣ T+  ⁣ ⁣Δ ⁣ ⁣ S0  ⁣ ⁣  ⁣ ⁣ T…\Rightarrow \text{ln}\left( \frac{{{p}_{z}}}{{{\text{p}}^{0}}} \right)=-\left( \frac{\text{ }\!\!\Delta\!\!\text{ }{{H}^{0}}}{{{10}^{4}}\text{R}} \right)\times \frac{{{10}^{4}}}{\text{ }\!\!~\!\!\text{ T}}+\frac{\text{ }\!\!\Delta\!\!\text{ }{{\text{S}}^{0}}}{\text{ }\!\!~\!\!\text{ T}}\ldots . (2)

Slope of the line =−  ⁣ ⁣Δ ⁣ ⁣ H0104R=[−7−(−3)]12−10=−2=-\frac{\text{ }\!\!\Delta\!\!\text{ }{{H}^{0}}}{{{10}^{4}}\text{R}}=\frac{\left[ -7-\left( -3 \right) \right]}{12-10}=-2 ∴  ⁣ ⁣Δ ⁣ ⁣ H0=2R×104\therefore \text{ }\!\!\Delta\!\!\text{ }{{H}^{0}}=2\text{R}\times {{10}^{4}} =2×8.314×10−3×104=1.66.28  ⁣ ⁣  ⁣ ⁣ kJ  ⁣ ⁣  ⁣ ⁣ mol−1  ⁣ ⁣  ⁣ ⁣ K−1=2\times 8.314\times {{10}^{-3}}\times {{10}^{4}}=1.66.28\text{ }\!\!~\!\!\text{ kJ }\!\!~\!\!\text{ mo}{{\text{l}}^{-1}}\text{ }\!\!~\!\!\text{ }{{\text{K}}^{-1}}

Solution figure

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Exam
JEE Advanced 2021
Paper
Paper 1
Subject
Chemistry
Chapter
Chemical Kinetics
Topic
Arrhenius Equation