In which of the following reactions- standard reaction entropy charge - So is positive and standard Gibb-s energy charge - Go decreases sharply with increasing temperature-

The correct option is A C (graphite) +1/2O_2(g)→ CO(g) C(graphite) + 1 2 O _ 2 (g) ⟶ CO(g) #160; Δ S ^∘ #160; is positive fo ...

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Standard XII

Chemistry

Entropy

In which of t...

Question

In which of the following reactions, standard reaction entropy charge $(Δ S^{o})$ is positive and standard Gibb's energy charge $(Δ G^{o})$ decreases sharply with increasing temperature?

M g (s) + \frac{1}{2} O_{2} (g) \to M g O (s)

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\frac{1}{2} C

(graphite)

+ \frac{1}{2} O_{2} (g) \to \frac{1}{2} C O_{2} (g)

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C

(graphite)

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

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

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Solution

The correct option is A $C$ (graphite) $+ \frac{1}{2} O_{2} (g) \to C O (g)$
$C (g r a p h i t e) + \frac{1}{2} O_{2} (g) ⟶ C O (g)$
$Δ S^{\circ}$ is positive for this reaction because $0.5$ mole of gas on reactant side is giving one mole of gas on product side after reacting with C (graphite). Also $Δ G$ decreases sharply with increase in temperature.

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Similar questions

Q. Given that:
(i)

C

(graphite)

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

;

Δ_{r} H^{o} = x k J m o l^{- 1}

.
(ii)

C

(graphite)

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

;

Δ_{r} H^{o} = y k J m o l^{- 1}

(iii)

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

;

Δ_{r} H^{o} = z k J m o l^{- 1}

Based on the given thermochemical equations, find out which one of the following algebraic relationships is correct?

Q. Considerthe following reactions,
I.

C (s) + \frac{1}{2} O_{2} (g) \to C O (g); Δ H_{1} = a

II.

C O (g) + \frac{1}{2} O_{2} (g) \to C O_{2} (g); Δ H_{2} = b

III.

C (s) + C O_{2} (g) \to 2 C O (g); Δ H_{3} = c

Select the correct statement

Q. Two reactions are given below:

(i)

C O_{(g)} + \frac{1}{2} O_{2} (g) \to C O_{2} (g)

(ii)

A g_{2} O_{(s)} \to 2 A g_{(s)} + \frac{1}{2} O_{2} (g)

Which of the following statements is true?

Q. Predict whether the reaction

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

at 300 K is spontaneous & exothermic or non-spontaneous & endothermic, when the standard entropy change is

- 0.094 k J m o l^{- 1} K^{- 1} .

The standard Gibb's free energies of formation for

C O_{2}

and

C O

are

- 394.4 a n d - 137.2 k J m o l^{- 1}

respectively.

C (s) + O_{2} (g) \to C O_{2} (g), Δ H = + 94.0 K c a l .

C O (g) + \frac{1}{2} O_{2} (g) \to C O_{2} (g), Δ H = - 67.7 K c a l .

From the above reactions find how much heat (Kcal mole

^{- 1}

) would be produced in the following reaction:

C (s) + \frac{1}{2} O_{2} (g) \to C O (g)

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In which of the following reactions, standard reaction entropy charge (ΔSo) is positive and standard Gibb's energy charge (ΔGo) decreases sharply with increasing temperature?

The correct option is A C (graphite) +12O2(g)→CO(g)C(graphite)+12O2(g)⟶CO(g) ΔS∘ is positive for this reaction because 0.5 mole of gas on reactant side is giving one mole of gas on product side after reacting with C (graphite). Also ΔG decreases sharply with increase in temperature.

In which of the following reactions, standard reaction entropy charge $(Δ S^{o})$ is positive and standard Gibb's energy charge $(Δ G^{o})$ decreases sharply with increasing temperature?