Assuming ideal behavior, the magnitude of logK for the following reaction at 250C is x×10−1. The value of x is_____. (Integer answer).3HC≡CH(g)⇌C6H6(l)[Given : ΔfG0(HC≡CH)=−2.04×105 J mol−1;ΔfG0(C6H6)=−1.24×105 J mol−1; R=8.314 J K−1 mol−1 ]

3HC≡CH(g)→C6H6(l);ΔG0=−RTlnK ⇒ΔG0=Σ(ΔGf0)P−Σ(ΔGf0)R ⇒−RTlnK=1×(1.24×105)−(−3×2.04×105) ⇒−2.303×R×TlogK=4.88×105 ⇒logK=−4.88×1052.303×8.314×298 =−85.52=855×10−1⇒x=855.

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Assuming ideal behavior, the magnitude of $\log K$ for the following reaction at $25^{0} C$ is $x \times 10^{- 1} .$ The value of $x$ is_____. (Integer answer).
$3 H C \equiv C H (g) ⇌ C_{6} H_{6} (l)$
[Given : $Δ_{f} G^{0} (H C \equiv C H) = - 2.04 \times 10^{5} J m o l^{- 1};$
$Δ_{f} G^{0} (C_{6} H_{6}) = - 1.24 \times 10^{5} J m o l^{- 1};$ $R = 8.314 J K^{- 1} m o l^{- 1}$ ]

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answer is 855.

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Detailed Solution

$3 H C \equiv C H (g) \to C_{6} H_{6} (l); Δ G^{0} = - R T \ln K \Rightarrow Δ G^{0} = Σ {(Δ G_{f}^{0})}_{P} - Σ {(Δ G_{f}^{0})}_{R} \Rightarrow - R T \ln K = 1 \times (1.24 \times 10^{5}) - (- 3 \times 2.04 \times 10^{5}) \Rightarrow - 2.303 \times R \times T \log K = 4.88 \times 10^{5} \Rightarrow \log K = - \frac{4.88 \times 10^{5}}{2.303 \times 8.314 \times 298} = - 85.52 = 855 \times 10^{- 1} \Rightarrow x = 855.$

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