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In conversion of lime-stone to lime, CaCO3(s) → CaO(s) + CO2(g) the values of ΔHº and ΔSº are + 179.1 kJ mol-1 and 160.2 J/K respectively at 298K and 1 bar. Assuming that ΔHº and ΔSº do not change with temperature, temperature above which conversion of limestone to lime will be spontaneous is-
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- a)1008 K
- b)1200 K
- c)845 K
- d)1118 K
Correct answer is option 'D'. Can you explain this answer?
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Verified Answer
In conversion of lime-stone to lime, CaCO3(s) → CaO(s) + CO2(g) t...
We know, ∆G = ∆H-T∆S
So, lets find the equilibrium temperature, i.e. at which
∆G = 0
∆H-T∆S
T= 179.1 x 1000/160.2
= 1118 K
So, at the temperature above this, the reaction becomes will spontaneous.
Most Upvoted Answer
In conversion of lime-stone to lime, CaCO3(s) → CaO(s) + CO2(g) t...
Calculating the Spontaneity Temperature:
To determine the temperature above which the conversion of limestone to lime will be spontaneous, we can use the Gibbs free energy equation:
ΔG° = ΔH° - TΔS°
Given Values:
ΔH° = +179.1 kJ mol-1
ΔS° = 160.2 J/K
T = temperature (in Kelvin)
Calculating ΔG°:
ΔG° = +179.1 - T(0.1602) (Note: Convert ΔS° to kJ for consistency)
ΔG° = +179.1 - 0.1602T
For a spontaneous reaction, ΔG° must be negative. Therefore:
0 > +179.1 - 0.1602T
0 > +179.1 - 0.1602T
0.1602T > +179.1
T > 1118 K
Conclusion:
Therefore, the temperature above which the conversion of limestone to lime will be spontaneous is 1118 K. So, option 'D' is the correct answer.
To determine the temperature above which the conversion of limestone to lime will be spontaneous, we can use the Gibbs free energy equation:
ΔG° = ΔH° - TΔS°
Given Values:
ΔH° = +179.1 kJ mol-1
ΔS° = 160.2 J/K
T = temperature (in Kelvin)
Calculating ΔG°:
ΔG° = +179.1 - T(0.1602) (Note: Convert ΔS° to kJ for consistency)
ΔG° = +179.1 - 0.1602T
For a spontaneous reaction, ΔG° must be negative. Therefore:
0 > +179.1 - 0.1602T
0 > +179.1 - 0.1602T
0.1602T > +179.1
T > 1118 K
Conclusion:
Therefore, the temperature above which the conversion of limestone to lime will be spontaneous is 1118 K. So, option 'D' is the correct answer.
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In conversion of lime-stone to lime, CaCO3(s) → CaO(s) + CO2(g) the values of ΔHº and ΔSº are + 179.1 kJ mol-1and 160.2 J/K respectively at 298K and 1 bar. Assuming that ΔHº and ΔSº do not change with temperature, temperature above which conversion of limestone to lime will be spontaneous is-[ AIEEE 2007]a)1008 Kb)1200 Kc)845 Kd)1118 KCorrect answer is option 'D'. Can you explain this answer?
Question Description
In conversion of lime-stone to lime, CaCO3(s) → CaO(s) + CO2(g) the values of ΔHº and ΔSº are + 179.1 kJ mol-1and 160.2 J/K respectively at 298K and 1 bar. Assuming that ΔHº and ΔSº do not change with temperature, temperature above which conversion of limestone to lime will be spontaneous is-[ AIEEE 2007]a)1008 Kb)1200 Kc)845 Kd)1118 KCorrect answer is option 'D'. Can you explain this answer? for Class 11 2024 is part of Class 11 preparation. The Question and answers have been prepared according to the Class 11 exam syllabus. Information about In conversion of lime-stone to lime, CaCO3(s) → CaO(s) + CO2(g) the values of ΔHº and ΔSº are + 179.1 kJ mol-1and 160.2 J/K respectively at 298K and 1 bar. Assuming that ΔHº and ΔSº do not change with temperature, temperature above which conversion of limestone to lime will be spontaneous is-[ AIEEE 2007]a)1008 Kb)1200 Kc)845 Kd)1118 KCorrect answer is option 'D'. Can you explain this answer? covers all topics & solutions for Class 11 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for In conversion of lime-stone to lime, CaCO3(s) → CaO(s) + CO2(g) the values of ΔHº and ΔSº are + 179.1 kJ mol-1and 160.2 J/K respectively at 298K and 1 bar. Assuming that ΔHº and ΔSº do not change with temperature, temperature above which conversion of limestone to lime will be spontaneous is-[ AIEEE 2007]a)1008 Kb)1200 Kc)845 Kd)1118 KCorrect answer is option 'D'. Can you explain this answer?.
In conversion of lime-stone to lime, CaCO3(s) → CaO(s) + CO2(g) the values of ΔHº and ΔSº are + 179.1 kJ mol-1and 160.2 J/K respectively at 298K and 1 bar. Assuming that ΔHº and ΔSº do not change with temperature, temperature above which conversion of limestone to lime will be spontaneous is-[ AIEEE 2007]a)1008 Kb)1200 Kc)845 Kd)1118 KCorrect answer is option 'D'. Can you explain this answer? for Class 11 2024 is part of Class 11 preparation. The Question and answers have been prepared according to the Class 11 exam syllabus. Information about In conversion of lime-stone to lime, CaCO3(s) → CaO(s) + CO2(g) the values of ΔHº and ΔSº are + 179.1 kJ mol-1and 160.2 J/K respectively at 298K and 1 bar. Assuming that ΔHº and ΔSº do not change with temperature, temperature above which conversion of limestone to lime will be spontaneous is-[ AIEEE 2007]a)1008 Kb)1200 Kc)845 Kd)1118 KCorrect answer is option 'D'. Can you explain this answer? covers all topics & solutions for Class 11 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for In conversion of lime-stone to lime, CaCO3(s) → CaO(s) + CO2(g) the values of ΔHº and ΔSº are + 179.1 kJ mol-1and 160.2 J/K respectively at 298K and 1 bar. Assuming that ΔHº and ΔSº do not change with temperature, temperature above which conversion of limestone to lime will be spontaneous is-[ AIEEE 2007]a)1008 Kb)1200 Kc)845 Kd)1118 KCorrect answer is option 'D'. Can you explain this answer?.
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