If at 298 K the bond energies of C-H, C-C, C=C and H-H bonds are respectively 414,347,615 and 43

step 1 conclusion, we are going to find the condition for the non spontaneity and we know that delta G

If at 298 K the bond energies of C-H, C-C, C=C and H-H bonds...

If at 298 K the bond energies of $\mathrm{C}-\mathrm{H}, \mathrm{C}-\mathrm{C}, \mathrm{C}=\mathrm{C}$ and $\mathrm{H}-\mathrm{H}$ bonds are respectively $414,347,615$ and $435 \mathrm{~kJ} \mathrm{~mol}^{-1}$, the value of enthalpy change for the reaction $\mathrm{H}_2 \mathrm{C}=\mathrm{CH}_2(\mathrm{~g})+\mathrm{H}_2(\mathrm{~g}) \longrightarrow \mathrm{H}_3 \mathrm{C}-\mathrm{CH}_3(\mathrm{~g})$ at 298 K will be (a) +250 kJ (b) -250 kJ (c) +125 kJ (d) -125 kJ

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Key Concepts

Bond Energy

Bond energy is the amount of energy required to break one mole of a specific chemical bond in the gas phase. It is a measure of bond strength, and these values are used to estimate the energy changes involved in chemical reactions by summing the energies required to break bonds and the energies released upon forming new bonds.

Reaction Enthalpy Calculation Using Bond Energies

The enthalpy change of a reaction can be estimated using bond energies by calculating the difference between the total energy needed to break the bonds in the reactants and the energy released when new bonds form in the products. This method involves summing the bond energies for all bonds broken and subtracting the sum of the bond energies for all bonds formed.

Exothermic and Endothermic Reactions

Exothermic reactions release energy to the surroundings (negative enthalpy change), whereas endothermic reactions absorb energy (positive enthalpy change). Determining whether a reaction is exothermic or endothermic using bond energy calculations helps in understanding the energy flow and spontaneity of the reaction.

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