For the hypothetical reaction- A 2 g- B 2 g- 2ABg - r G o and - r S o is 20 kJ-mol and -20 JK -1 mol -1 respectively at 200K- If - r C p is 20 JK -1 mol -1 then - r H o at 400K is -

The correct option is C 20 kJ/mol As we know, Δ G =Δ H T #160;Δ S; ⇒ 20=Δ H 200× 201000; ⇒Δ H = 16kJ/mol Also, Δ H= #160;Δ_r C_p (T_2 T_1) ...

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Standard XII

Chemistry

Gibbs Free Energy & Spontaneity

For the hypot...

Question

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

20 k J / m o l

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7.98 k J / m o l

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28 k J / m o l

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none of these

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Solution

The correct option is C $20 k J / m o l$
As we know,
$Δ G = Δ H - T Δ S; \Rightarrow 20 = Δ H - 200 \times \frac{- 20}{1000}; \Rightarrow Δ H = 16 k J / m o l$
Also,
$Δ H = Δ_{r} C_{p} (T_{2} - T_{1}); Δ H = 16 + 20 \times \frac{200}{1000} = 20 k J / m o l$

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Similar questions

For the hypothetical reaction,

A_{2} (g) + B_{2} (g) ⇌ 2 A B (g)

, if

Δ_{r} G^{o}

and

Δ_{r} S^{o}

are

20 k J / m o l

and

- 20 {J K}^{- 1} {m o l}^{- 1}

respectively at 200 K.

Δ_{r} C_{p}

20 J K^{- 1} m o l^{- 1}

Then value

\frac{Δ_{r} H^{o}}{10}

of (

k J / m o l

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Q. For the hypothetical reaction,

A_{2} (g) + B_{2} (g) ⇌ 2 A B (g)

Δ_{r} G^{\circ}

and

Δ_{r} S^{\circ}

are

20 kJ/mol

and

- 20 {JK}^{- 1} {mol}^{- 1}

respectively at 200 K. If

Δ_{r} C_{p}

20 {JK}^{- 1} {mol}^{- 1}

then

Δ_{r} H^{\circ}

at 400K is:

Q. The value of

{log}_{10} K

for a reaction

A ⇌ B

is____________.
Given

Δ_{r} H_{298 K}^{o} = - 54.07 k J {m o l}^{- 1}, Δ_{r} S_{298 K}^{o} = 10 J K^{- 1} {m o l}^{- 1}, R = 8.314 J K^{- 1} {m o l}^{- 1}

Q. For a chemical reaction

A + B ⇌ C + D (Δ_{r} H^{o} = 80 k J m o l^{1})

the entropy change

Δ_{r} S^{o}

depends on the temperature

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(in

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) as

Δ_{r} S^{o} = 2 T (J K^{- 1} m o l^{- 1})

. Minimum temperature at which it will become spontaneous is ________

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Q. Calculate

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(in

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from the

Δ_{r} G^{o}

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4 C r (s) + 3 O_{2} (g) ⟶ 2 {C r}_{2} O_{3} (s)

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Δ_{r} G^{o} = - 2093.4 k J / m o l

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For the hypothetical reaction: A2(g)+B2(g)⇌2AB(g)ΔrGo and ΔrSo is 20kJ/mol and −20JK−1mol−1 respectively at 200K. If ΔrCp is 20JK−1mol−1 then ΔrHo at 400K is :

The correct option is C 20 kJ/molAs we know,ΔG=ΔH−TΔS;⇒20=ΔH−200×−201000;⇒ΔH=16kJ/molAlso,ΔH=ΔrCp(T2−T1);ΔH=16+20×2001000=20kJ/mol

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

The correct option is C $20 k J / m o l$
As we know,
$Δ G = Δ H - T Δ S; \Rightarrow 20 = Δ H - 200 \times \frac{- 20}{1000}; \Rightarrow Δ H = 16 k J / m o l$
Also,
$Δ H = Δ_{r} C_{p} (T_{2} - T_{1}); Δ H = 16 + 20 \times \frac{200}{1000} = 20 k J / m o l$