The standard enthalpy of vaporization for water at 100 oC is 40.66 kJ mol-1.
The internal energy of vaporization of water at 100 oC (in kJ mol-1) is:
(Assume water vapour behaves like an ideal gas.)
1. +37.56
2. -43.76
3. +43.76
4. +40.66
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NEET MCQ Books for XIth & XIIth Physics, Chemistry & BiologyGiven the following reaction:
\(4H(g)\)→ \(2 H_{2}\)\((g)\)
The enthalpy change for the reaction is -869.6 kJ. The dissociation energy of the H-H bond is:
1. -869.6 kJ
2. +434.8kJ
3. +217.4kJ
4. -434.8 kJ
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NEET MCQ Books for XIth & XIIth Physics, Chemistry & BiologyConsider the following processes:
∆H (kJ/mol)
½ A → B + 150
3B → 2C + D –125
E + A → 2D +350
For B + D → E + 2C, ∆H will be-
1. 325 kJ/mol
2. 525 kJ/mol
3. –175 kJ.mol
4. –325 kJ/mol
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NEET MCQ Books for XIth & XIIth Physics, Chemistry & BiologyThe following two reactions are known
The value of H for the following reaction
is:
1. -43.3 kJ
2. -10.3 kJ
3. +6.2 kJ
4. +10.3 kJ
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NEET MCQ Books for XIth & XIIth Physics, Chemistry & Biology