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For the reaction, 2Cl(g) ⟶ Cl2(g), the correct option is :
- a)∆rH > 0 and ∆rS < />
- b)∆rH < 0="" and="" />rS > 0
- c)∆rH < 0="" and="" />rS < />
- d)∆rH > 0 and ∆rS > 0
Correct answer is option 'C'. Can you explain this answer?
Most Upvoted Answer
For the reaction, 2Cl(g) ⟶ Cl2(g), the correct option is :a)∆rH > 0 a...
Explanation:
The reaction given is 2Cl(g) ⟶ Cl2(g).
∆rH: The enthalpy change of the reaction is the difference between the enthalpies of the products and reactants. Here, the reaction involves the breaking of a bond in Cl2 molecule and the formation of two Cl atoms. This requires energy, so the enthalpy change will be positive.
∆rS: The entropy change of the reaction is the difference between the entropy of the products and reactants. In this reaction, the number of moles of gas decreases from 2 to 1, so the entropy change will be negative.
Option (c) is correct because both enthalpy and entropy changes are positive and negative respectively. The Gibbs energy change (∆rG) of the reaction can be calculated using the equation:
∆rG = ∆rH - T∆rS
where T is the temperature in Kelvin.
Since both ∆rH and ∆rS have opposite signs, the sign of the Gibbs energy change will depend on the temperature. At low temperatures, the reaction will be spontaneous as ∆rG will be negative. At high temperatures, the reaction will be non-spontaneous as ∆rG will be positive.
Therefore, option (c) is correct because it takes into account both enthalpy and entropy changes in the reaction.
The reaction given is 2Cl(g) ⟶ Cl2(g).
∆rH: The enthalpy change of the reaction is the difference between the enthalpies of the products and reactants. Here, the reaction involves the breaking of a bond in Cl2 molecule and the formation of two Cl atoms. This requires energy, so the enthalpy change will be positive.
∆rS: The entropy change of the reaction is the difference between the entropy of the products and reactants. In this reaction, the number of moles of gas decreases from 2 to 1, so the entropy change will be negative.
Option (c) is correct because both enthalpy and entropy changes are positive and negative respectively. The Gibbs energy change (∆rG) of the reaction can be calculated using the equation:
∆rG = ∆rH - T∆rS
where T is the temperature in Kelvin.
Since both ∆rH and ∆rS have opposite signs, the sign of the Gibbs energy change will depend on the temperature. At low temperatures, the reaction will be spontaneous as ∆rG will be negative. At high temperatures, the reaction will be non-spontaneous as ∆rG will be positive.
Therefore, option (c) is correct because it takes into account both enthalpy and entropy changes in the reaction.
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Community Answer
For the reaction, 2Cl(g) ⟶ Cl2(g), the correct option is :a)∆rH > 0 a...
We know that, Cl2(g) ⟶ 2Cl(g) is endothermic reaction because it required energy to break bond.
So reverse reaction, 2Cl(g) ⟶ Cl2(g) will be exothermic, ∆rH < 0="" also,="" two="" gaseous="" atom="" combine="" together="" to="" form="" 1="" gaseous="" />
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For the reaction, 2Cl(g) ⟶ Cl2(g), the correct option is :a)∆rH > 0 and ∆rS b)∆rH rS > 0c)∆rH rS d)∆rH > 0 and ∆rS > 0Correct answer is option 'C'. Can you explain this answer?
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