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How much heat will be required at constant pressure to form 1.28 kg of CaC2 from CaO(s) & C(s) ?
Given :
ΔfH°(CaO, s) = -152 kcal/mol
ΔfH°(CaC2, s) = -14 kcal/mol
ΔfH°(CO, g) = -26 kcal/mol
- a)+112 kcal
- b)224 kcal
- c)3840 kcal
- d)2240 kcal
Correct answer is option 'D'. Can you explain this answer?
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Verified Answer
How much heat will be required at constant pressure to form 1.28 kg of...
Reaction is CaO + C → CaC2+CO
1.28 kg of CaC2 means 20 mole CaC2 is needed
For 1 mole dH=-26-14-(-152)=112
For 20 Mole 112×20=2240
1.28 kg of CaC2 means 20 mole CaC2 is needed
For 1 mole dH=-26-14-(-152)=112
For 20 Mole 112×20=2240
Most Upvoted Answer
How much heat will be required at constant pressure to form 1.28 kg of...
Reaction is CaO+C->CaC2+CO
1.28 KG of CaC2 means 20 mole CaC2 is needed
For 1 mole dH=-26-14-(-152)=112
For 20 Mole 112*20=2240
1.28 KG of CaC2 means 20 mole CaC2 is needed
For 1 mole dH=-26-14-(-152)=112
For 20 Mole 112*20=2240
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Community Answer
How much heat will be required at constant pressure to form 1.28 kg of...
To calculate the heat required to form 1.28 kg of CaC2 from CaO(s), we need to use the enthalpy of formation for CaC2 and CaO. The balanced chemical equation for the reaction is:
CaO(s) + 3C(s) → CaC2(s) + CO(g)
The enthalpy of formation for CaC2 is -59.8 kJ/mol and for CaO is -635.1 kJ/mol.
First, we need to calculate the number of moles of CaO in 1.28 kg:
molar mass of CaO = 40.08 g/mol
number of moles of CaO = (1.28 kg) / (40.08 g/mol) = 31.92 mol
According to the balanced equation, 1 mole of CaO reacts to form 1 mole of CaC2. Therefore, the number of moles of CaC2 formed is also 31.92 mol.
Now, we can calculate the heat required using the enthalpy of formation values:
Heat required = (31.92 mol) * (-59.8 kJ/mol)
Heat required = -1908.096 kJ
Therefore, approximately 1908 kJ of heat will be required at constant pressure to form 1.28 kg of CaC2 from CaO(s).
CaO(s) + 3C(s) → CaC2(s) + CO(g)
The enthalpy of formation for CaC2 is -59.8 kJ/mol and for CaO is -635.1 kJ/mol.
First, we need to calculate the number of moles of CaO in 1.28 kg:
molar mass of CaO = 40.08 g/mol
number of moles of CaO = (1.28 kg) / (40.08 g/mol) = 31.92 mol
According to the balanced equation, 1 mole of CaO reacts to form 1 mole of CaC2. Therefore, the number of moles of CaC2 formed is also 31.92 mol.
Now, we can calculate the heat required using the enthalpy of formation values:
Heat required = (31.92 mol) * (-59.8 kJ/mol)
Heat required = -1908.096 kJ
Therefore, approximately 1908 kJ of heat will be required at constant pressure to form 1.28 kg of CaC2 from CaO(s).
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How much heat will be required at constant pressure to form 1.28 kg of CaC2from CaO(s) & C(s) ?Given :ΔfH°(CaO, s) = -152 kcal/molΔfH°(CaC2, s) = -14 kcal/molΔfH°(CO, g) = -26 kcal/mola)+112 kcalb)224 kcalc)3840 kcald)2240 kcalCorrect answer is option 'D'. Can you explain this answer?
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How much heat will be required at constant pressure to form 1.28 kg of CaC2from CaO(s) & C(s) ?Given :ΔfH°(CaO, s) = -152 kcal/molΔfH°(CaC2, s) = -14 kcal/molΔfH°(CO, g) = -26 kcal/mola)+112 kcalb)224 kcalc)3840 kcald)2240 kcalCorrect 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 How much heat will be required at constant pressure to form 1.28 kg of CaC2from CaO(s) & C(s) ?Given :ΔfH°(CaO, s) = -152 kcal/molΔfH°(CaC2, s) = -14 kcal/molΔfH°(CO, g) = -26 kcal/mola)+112 kcalb)224 kcalc)3840 kcald)2240 kcalCorrect 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 How much heat will be required at constant pressure to form 1.28 kg of CaC2from CaO(s) & C(s) ?Given :ΔfH°(CaO, s) = -152 kcal/molΔfH°(CaC2, s) = -14 kcal/molΔfH°(CO, g) = -26 kcal/mola)+112 kcalb)224 kcalc)3840 kcald)2240 kcalCorrect answer is option 'D'. Can you explain this answer?.
How much heat will be required at constant pressure to form 1.28 kg of CaC2from CaO(s) & C(s) ?Given :ΔfH°(CaO, s) = -152 kcal/molΔfH°(CaC2, s) = -14 kcal/molΔfH°(CO, g) = -26 kcal/mola)+112 kcalb)224 kcalc)3840 kcald)2240 kcalCorrect 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 How much heat will be required at constant pressure to form 1.28 kg of CaC2from CaO(s) & C(s) ?Given :ΔfH°(CaO, s) = -152 kcal/molΔfH°(CaC2, s) = -14 kcal/molΔfH°(CO, g) = -26 kcal/mola)+112 kcalb)224 kcalc)3840 kcald)2240 kcalCorrect 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 How much heat will be required at constant pressure to form 1.28 kg of CaC2from CaO(s) & C(s) ?Given :ΔfH°(CaO, s) = -152 kcal/molΔfH°(CaC2, s) = -14 kcal/molΔfH°(CO, g) = -26 kcal/mola)+112 kcalb)224 kcalc)3840 kcald)2240 kcalCorrect answer is option 'D'. Can you explain this answer?.
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