| (i)\[{{H}^{+}}(aq)+O{{H}^{-}}(aq)\to {{H}_{2}}O(l);\] | \[\Delta H =-{{X}_{1}}\,kJ\,mo{{l}^{-1}}\] |
| (ii) \[{{H}_{2}}(g)+\frac{1}{2}{{O}_{2}}(g)\to {{H}_{2}}O(l);\] | \[\Delta H =-{{X}_{2}}\,kJ\,mo{{l}^{-1}}\] |
| (iii) \[C{{O}_{2}}(g)+{{H}_{2}}(g)\to CO(g)+{{H}_{2}}O(l);\] | \[\Delta H =-{{X}_{3}}kJ\,mo{{l}^{-1}}\] |
| (iv) \[{{C}_{2}}{{H}_{2}}(g)+\frac{5}{2}{{O}_{2}}(g)\to 2C{{O}_{2}}g+{{H}_{2}}O(l);\] | \[\Delta H =+{{X}_{4}}\,kJ\,mo{{l}^{-1}}\] |
A) \[-{{x}_{2}}\,\,kJ\,mo{{l}^{-1}}\]
B) \[+{{x}_{3}}\,\,kJ\,mo{{l}^{-1}}\]
C) \[-{{x}_{4}}\,\,kJ\,mo{{l}^{-1}}\]
D) \[-{{x}_{1}}\,\,kJ\,mo{{l}^{-1}}\]
Correct Answer: A
Solution :
The amount of heat evolved or absorbed during the formation of 1 mole of a compound from its constituent is known as heat of formation. So, the correct answer is \[{{H}_{2}}(g)+\frac{1}{2}{{O}_{2}}(g)\to {{H}_{2}}O(l);\,\Delta H =-{{X}_{2}}\,kJ\,mo{{l}^{-1}}\]
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