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Question

Follow data is given for the reaction: CaCO3CaO(s)+CO2(g)
ΔfH[CaO(s)]=635.1kJmol1
ΔfH[CO2(g)]=393.5kJmol1
ΔfH[CaCO3(s)]=1206.9kJmol1
Predict the effect of temperature on the equilibrium constant of the above reaction.
  1. If T increases, reaction proceeds in forward direction.
  2. If T increases, reaction proceeds in backward direction.
  3. If T decreases, reaction proceeds in forward direction.
  4. If T increases, reaction remains at equilibrium.

A
If T increases, reaction proceeds in forward direction.
B
If T increases, reaction remains at equilibrium.
C
If T increases, reaction proceeds in backward direction.
D
If T decreases, reaction proceeds in forward direction.
Solution
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ΔrH=ΔrH[CaO(s)]+ΔrH[CO2(9)]ΔrH[CaCO3(s)]
ΔrH=178.3kJmol1
The reaction is endothermic.
Hence, according to Le-Chatelier's principle, reaction will proceed in forward direction on increasing temperature.

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Q1
Follow data is given for the reaction: CaCO3CaO(s)+CO2(g)
ΔfH[CaO(s)]=635.1kJmol1
ΔfH[CO2(g)]=393.5kJmol1
ΔfH[CaCO3(s)]=1206.9kJmol1
Predict the effect of temperature on the equilibrium constant of the above reaction.
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Q2
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ΔfH[CaO(s)]=635.1kJ mol1
ΔfH[CO2(g)]=393.5kJ mol1
ΔfH[CaCO3(s)]=1206.9kJ mol1
Predict the effect of temperature on the equilibrium constant of the above reaction.
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Q3
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ΔfHo[CaCO3(s)]=1206.9 kJ mol1
Predict the effect of temperature on the equilibrium constant of the above reaction.
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