For the hypothetical reaction A2 g - B2g - 2ABgIf - r G- and - r S- are 20 kJ-mole and -20 JK-1 mol-1 respectively at 200 K- - r Cp is 20 JK-1 mol-1 then determine - H- at 400 K-

The correct option is A 20 kJ/mol Δ H_1 = Δ G^o + TΔ S^o = 20+ 200( 20)= 3980 #160;KJ Δ H^o= Δ E + C_pΔ T Δ E = Δ H_1 Δ H^o= 3980 + 20(4 ...

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Standard XII

Chemistry

Hess' Law

For the hypot...

Question

For the hypothetical reaction $A_{2} (g) + B_{2} (g) ⇌ 2 A B (g)$
If $Δ_{r} G^{\circ}$ and $Δ_{r} S^{\circ}$ are 20 kJ/mole and $- 20 J K^{- 1} m o l^{- 1}$ respectively at 200 K.
$Δ_{r} C_{p}$ is 20 $J K^{- 1} m o l^{- 1}$ then determine $Δ H^{\circ}$ at 400 K.

20 kJ/mol

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30 KJ/MOLE

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12kj/mole

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23kj/mole

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Solution

The correct option is A 20 kJ/mol
$Δ H_{1} = Δ G^{o} + T Δ S^{o} = 20 + 200 (- 20) = - 3980 K J$
$Δ H^{o} = Δ E + C_{p} Δ T$
$Δ E = Δ H_{1}$
$Δ H^{o} = - 3980 + 20 (400 - 200) = - 3980 + 4000 = 20 k J / m o l e$

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For the hypothetical reaction A2(g)+B2(g)⇌2AB(g)If ΔrG∘ and ΔrS∘ are 20 kJ/mole and −20JK−1mol−1 respectively at 200 K.ΔrCp is 20 JK−1mol−1 then determine ΔH∘ at 400 K.

The correct option is A 20 kJ/molΔH1=ΔGo+TΔSo=20+200(−20)=−3980KJΔHo=ΔE+CpΔTΔE=ΔH1ΔHo=−3980+20(400−200)=−3980+4000=20kJ/mole

For the hypothetical reaction $A_{2} (g) + B_{2} (g) ⇌ 2 A B (g)$
If $Δ_{r} G^{\circ}$ and $Δ_{r} S^{\circ}$ are 20 kJ/mole and $- 20 J K^{- 1} m o l^{- 1}$ respectively at 200 K.
$Δ_{r} C_{p}$ is 20 $J K^{- 1} m o l^{- 1}$ then determine $Δ H^{\circ}$ at 400 K.

The correct option is A 20 kJ/mol
$Δ H_{1} = Δ G^{o} + T Δ S^{o} = 20 + 200 (- 20) = - 3980 K J$
$Δ H^{o} = Δ E + C_{p} Δ T$
$Δ E = Δ H_{1}$
$Δ H^{o} = - 3980 + 20 (400 - 200) = - 3980 + 4000 = 20 k J / m o l e$