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50.0 mL of 0.10 M HCl is mixed with 50.0 mL of 0.10 M NaOH. The solution temperature rises by 3.0°C Calculate the enthalpy of neutralization per mole of HCl. [take proper assumptions]
- a)-2.5 × 102 kJ
- b)-1.3 × 102 kJ
- c)-8.4 × 101 kJ
- d)-6.3 × 101 kJ
Correct answer is option 'A'. Can you explain this answer?
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50.0 mL of 0.10 M HCl is mixed with 50.0 mL of 0.10 M NaOH. The soluti...
No. of moles of HCl = 5 millimoles
No. of moles of NaOH = 5 millimoles
Mass of solution mixed = 50 gm+50 gm=100 gm
ΔH=−cmΔT(c=4.18 kJKg−1)
⇒ ΔH=−4.18×0.1×3
⇒ ΔH=−1.254 kJ (For 5 millimoles of water formed)
For 1 mole water = −1.254/5×10−3
=−2.5×102kJ
No. of moles of NaOH = 5 millimoles
Mass of solution mixed = 50 gm+50 gm=100 gm
ΔH=−cmΔT(c=4.18 kJKg−1)
⇒ ΔH=−4.18×0.1×3
⇒ ΔH=−1.254 kJ (For 5 millimoles of water formed)
For 1 mole water = −1.254/5×10−3
=−2.5×102kJ
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50.0 mL of 0.10 M HCl is mixed with 50.0 mL of 0.10 M NaOH. The solution temperature rises by 3.0°C Calculate the enthalpy of neutralization per mole of HCl. [take proper assumptions]a)-2.5 × 102kJb)-1.3 × 102kJc)-8.4 × 101kJd)-6.3 × 101kJCorrect answer is option 'A'. Can you explain this answer? for Class 11 2025 is part of Class 11 preparation. The Question and answers have been prepared according to the Class 11 exam syllabus. Information about 50.0 mL of 0.10 M HCl is mixed with 50.0 mL of 0.10 M NaOH. The solution temperature rises by 3.0°C Calculate the enthalpy of neutralization per mole of HCl. [take proper assumptions]a)-2.5 × 102kJb)-1.3 × 102kJc)-8.4 × 101kJd)-6.3 × 101kJCorrect answer is option 'A'. Can you explain this answer? covers all topics & solutions for Class 11 2025 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for 50.0 mL of 0.10 M HCl is mixed with 50.0 mL of 0.10 M NaOH. The solution temperature rises by 3.0°C Calculate the enthalpy of neutralization per mole of HCl. [take proper assumptions]a)-2.5 × 102kJb)-1.3 × 102kJc)-8.4 × 101kJd)-6.3 × 101kJCorrect answer is option 'A'. Can you explain this answer?.
50.0 mL of 0.10 M HCl is mixed with 50.0 mL of 0.10 M NaOH. The solution temperature rises by 3.0°C Calculate the enthalpy of neutralization per mole of HCl. [take proper assumptions]a)-2.5 × 102kJb)-1.3 × 102kJc)-8.4 × 101kJd)-6.3 × 101kJCorrect answer is option 'A'. Can you explain this answer? for Class 11 2025 is part of Class 11 preparation. The Question and answers have been prepared according to the Class 11 exam syllabus. Information about 50.0 mL of 0.10 M HCl is mixed with 50.0 mL of 0.10 M NaOH. The solution temperature rises by 3.0°C Calculate the enthalpy of neutralization per mole of HCl. [take proper assumptions]a)-2.5 × 102kJb)-1.3 × 102kJc)-8.4 × 101kJd)-6.3 × 101kJCorrect answer is option 'A'. Can you explain this answer? covers all topics & solutions for Class 11 2025 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for 50.0 mL of 0.10 M HCl is mixed with 50.0 mL of 0.10 M NaOH. The solution temperature rises by 3.0°C Calculate the enthalpy of neutralization per mole of HCl. [take proper assumptions]a)-2.5 × 102kJb)-1.3 × 102kJc)-8.4 × 101kJd)-6.3 × 101kJCorrect answer is option 'A'. Can you explain this answer?.
Solutions for 50.0 mL of 0.10 M HCl is mixed with 50.0 mL of 0.10 M NaOH. The solution temperature rises by 3.0°C Calculate the enthalpy of neutralization per mole of HCl. [take proper assumptions]a)-2.5 × 102kJb)-1.3 × 102kJc)-8.4 × 101kJd)-6.3 × 101kJCorrect answer is option 'A'. Can you explain this answer? in English & in Hindi are available as part of our courses for Class 11.
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50.0 mL of 0.10 M HCl is mixed with 50.0 mL of 0.10 M NaOH. The solution temperature rises by 3.0°C Calculate the enthalpy of neutralization per mole of HCl. [take proper assumptions]a)-2.5 × 102kJb)-1.3 × 102kJc)-8.4 × 101kJd)-6.3 × 101kJCorrect answer is option 'A'. Can you explain this answer?, a detailed solution for 50.0 mL of 0.10 M HCl is mixed with 50.0 mL of 0.10 M NaOH. The solution temperature rises by 3.0°C Calculate the enthalpy of neutralization per mole of HCl. [take proper assumptions]a)-2.5 × 102kJb)-1.3 × 102kJc)-8.4 × 101kJd)-6.3 × 101kJCorrect answer is option 'A'. Can you explain this answer? has been provided alongside types of 50.0 mL of 0.10 M HCl is mixed with 50.0 mL of 0.10 M NaOH. The solution temperature rises by 3.0°C Calculate the enthalpy of neutralization per mole of HCl. [take proper assumptions]a)-2.5 × 102kJb)-1.3 × 102kJc)-8.4 × 101kJd)-6.3 × 101kJCorrect answer is option 'A'. Can you explain this answer? theory, EduRev gives you an
ample number of questions to practice 50.0 mL of 0.10 M HCl is mixed with 50.0 mL of 0.10 M NaOH. The solution temperature rises by 3.0°C Calculate the enthalpy of neutralization per mole of HCl. [take proper assumptions]a)-2.5 × 102kJb)-1.3 × 102kJc)-8.4 × 101kJd)-6.3 × 101kJCorrect answer is option 'A'. Can you explain this answer? tests, examples and also practice Class 11 tests.
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