For the reaction-2 A-g- B-g- displaystyle rightarrow 2D-g- displaystyle bigtriangleup U-ominus -10-5KJ and bigtriangleup S-ominus-44-1 JK-1- Calculate displaystyle bigtriangleup G-ominus - the reaction and predict whether the reaction may occur spontaneously-

Question

For the reaction-2 A-g- B-g-  displaystyle rightarrow  2D-g-  displaystyle bigtriangleup U-ominus -10-5KJ and  bigtriangleup S-ominus-44-1 JK-1- Calculate  displaystyle bigtriangleup G-ominus -  the reaction and predict whether the reaction may occur spontaneously-

Toppr Admin · Accepted Answer

The change in the number of moles of gaseous species, $Δ n_{g} = 2 - 3 = - 1$

$Δ H^{0} = Δ U^{0} + Δ n_{g} R T = - 10.5 + (- 1) \times 8.314 \times 10^{- 3} \times 298 = - 12.98 k J$
$Δ G^{0} = Δ H^{0} - T Δ S^{0} = - 12.98 - 298 (- 44.10 \times 10^{- 3}) = 0.16 k J$

For the reaction,2 A(g)+ B(g) → 2D(g), △U⊖=−10.5KJ and △S⊖=−44.1JK−1Calculate △G⊖ for the reaction and predict whether the reaction may occur spontaneously.

The change in the number of moles of gaseous species, Δng=2−3=−1ΔH0=ΔU0+ΔngRT=−10.5+(−1)×8.314×10−3×298=−12.98kJΔG0=ΔH0−TΔS0=−12.98−298(−44.10×10−3)=0.16kJ

For the reaction,
2 A(g)+ B(g) $\to$ 2D(g), $△ U^{⊖} = - 10.5 K J$ and $△ S^{⊖} = - 44.1 J K^{- 1}$

Calculate $△ G^{⊖}$ for the reaction and predict whether the reaction may occur spontaneously.

The change in the number of moles of gaseous species, $Δ n_{g} = 2 - 3 = - 1$

$Δ H^{0} = Δ U^{0} + Δ n_{g} R T = - 10.5 + (- 1) \times 8.314 \times 10^{- 3} \times 298 = - 12.98 k J$
$Δ G^{0} = Δ H^{0} - T Δ S^{0} = - 12.98 - 298 (- 44.10 \times 10^{- 3}) = 0.16 k J$