The equilibrium constant for the reaction given below is 2.0×10−7 a

1.	The equilibrium constant for the reaction given below is 2.0×10−7 at 300 K. PCl5(g)⇌PCl3(g)+Cl2(g). The value of \|S∘\| is −x J mol−1 K−1. Calculate the value of x if ΔH∘=28.4 kJ mol−1 (Give your answer upto one deimal only)
Answer» The equilibrium constant for the reaction given below is $2.0 \times 10^{- 7} a t 300 K$ . $P C l_{5} (g) ⇌ P C l_{3} (g) + C l_{2} (g)$ . The value of $\| S^{\circ} \|$ is $- x J m o l^{- 1} K^{- 1}$ . Calculate the value of $x$ if $Δ H^{\circ} = 28.4 k J m o l^{- 1}$ (Give your answer upto one deimal only)

The equilibrium constant for the reaction given below is 2.0×10−7 at 300 K. PCl5(g)⇌PCl3(g)+Cl2(g). The value of |S∘| is −x J mol−1 K−1. Calculate the value of x if ΔH∘=28.4 kJ mol−1 (Give your answer upto one deimal only)

Answer»

The equilibrium constant for the reaction given below is $2.0 \times 10^{- 7} a t 300 K$ .

$P C l_{5} (g) ⇌ P C l_{3} (g) + C l_{2} (g)$ . The value of $| S^{\circ} |$ is $- x J m o l^{- 1} K^{- 1}$ . Calculate the value of $x$ if $Δ H^{\circ} = 28.4 k J m o l^{- 1}$ (Give your answer upto one deimal only)

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The equilibrium constant for the reaction given below is 2.0×10−7 at 300 K. PCl5(g)⇌PCl3(g)+Cl2(g). The value of |S∘| is −x J mol−1 K−1. Calculate the value of x if ΔH∘=28.4 kJ mol−1 (Give your answer upto one deimal only)

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