The value of H and S for the reaction- C graphite - CO 2 g - 2 CO g are 170kJ and 170JK -1- respectively- This reaction will be spontaneous at-

The correct option is C 1119K C_(graphite) + CO_2(g) #160; → 2CO(g) The Rn is spontaneous when Δ G ⩽ O ⇒Δ H TΔ S ≤ O ⇒ TΔ S ⩾Δ H ...

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Standard XII

Chemistry

Spontaneity

The value of ...

Question

The value of $△$ H and $△$ S for the reaction, $C_{(g r a p h i t e)} + {C O}_{2 (g)} \to 2 {C O}_{(g)}$ are 170kJ and ${170 J K}^{- 1}$ , respectively. This reaction will be spontaneous at:

510K

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710K

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910K

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1119K

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Solution

The correct option is C 1119K
$C_{(g r a p h i t e)} + C O_{2} (g) \to 2 C O (g)$
The $R n$ is spontaneous when $Δ G ⩽ O$
$\Rightarrow Δ H - T Δ S \leq O$
$\Rightarrow T Δ S ⩾ Δ H$
$\Rightarrow T ⩾ \frac{Δ H}{Δ S}$
$T ⩾ \frac{170 \times 10^{3}}{1170}$
$T ⩾ 1000 K$

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Similar questions

Q. The values of

Δ H

and

Δ S

for the reaction, C(graphite) +

C O_{2} (g) \to 2 C O (g)

are 170 kJ and

170 J K^{- 1}

respectively. This reaction will be spontaneous at:

C (s) + C O_{2} (g) ⇋ 2 C O (g)

For the given reaction, the partial pressures of

C O_{2}

and CO are 4.0 and 4.0 respectively at equilibrium, what is the value of

K_{p}

for this reaction?

Q. For the reaction

C O (g) + \frac{1}{2} O_{2} (g) \to C O_{2} (g), Δ H

and

Δ S

are

- 283 kJ

and

- 87 {J K}^{- 1} {mol}^{- 1}

respectively. It was intended to carry out this reaction at

1000, 1500, 3000

and

3500 K

. At which of these temperatures would this reaction be thermodynamically spontaneous?

Q. The enthalpy and entropy change for the reaction,

B r_{2} (l) + C l_{2} (g) \to 2 B r C l (g)

are

7.1 k c a l

m o l

and

25 c a l K^{- 1} m o l^{- 1}

respectively. This reaction will be spontaneous at:

For a reaction at $25^{\circ} C$ enthalpy change $(△ H)$ and entropy change $(△ S)$ are $- 11.7 \times 103 J m o l^{- 1}$ and $- 105 J m o l^{- 1} K^{- 1}$ respectively. Find out whether this reaction is spontaneous or not?

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The value of △H and △S for the reaction, C(graphite)+CO2(g)→2CO(g) are 170kJ and 170JK−1, respectively. This reaction will be spontaneous at:

The correct option is C 1119KC(graphite)+CO2(g)→2CO(g)The Rn is spontaneous when ΔG⩽O⇒ΔH−TΔS≤O⇒TΔS⩾ΔH⇒T⩾ΔHΔST⩾170×1031170T⩾1000K

The value of $△$ H and $△$ S for the reaction, $C_{(g r a p h i t e)} + {C O}_{2 (g)} \to 2 {C O}_{(g)}$ are 170kJ and ${170 J K}^{- 1}$ , respectively. This reaction will be spontaneous at:

The correct option is C 1119K
$C_{(g r a p h i t e)} + C O_{2} (g) \to 2 C O (g)$
The $R n$ is spontaneous when $Δ G ⩽ O$
$\Rightarrow Δ H - T Δ S \leq O$
$\Rightarrow T Δ S ⩾ Δ H$
$\Rightarrow T ⩾ \frac{Δ H}{Δ S}$
$T ⩾ \frac{170 \times 10^{3}}{1170}$
$T ⩾ 1000 K$