MCQ
Covalent compounds have low melting point because
- ACovalent bond is less exothermic
- BCovalent molecules have definite shape
- CCovalent bond is weaker than ionic bond
- ✓Covalent molecules are held by weak Vander Waal's force of attraction
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| $Cl_2(g) \rightarrow 2Cl(g),$ | $242.3\,kJ\,mol^{-1}$ |
| $I_2(g) \rightarrow 2I(g),$ | $151.0\,kJ\,mol^{-1}$ |
| $ICl(g) \rightarrow I(g)+Cl(g),$ | $211.3\,kJ\,mol^{-1}$ |
| $I_2(s) \rightarrow I_2(g),$ | $62.76\,kJ\,mol^{-1}$ |
Given that the standard states for iodine and chlorine are $I_2(s)$ and $Cl_2(g),$ the standard enthalpy of formation for $ICl(g)$ is : ............... $\mathrm{kJ\,mol}^{-1}$