OnlineCBT
Chemistry · CHEMICAL BONDING AND MOLECULAR STRUCTURE
हिन्दीFor the formation of one mole of gaseous hydrogen molecules from isolated atoms: \( 2\text{H(g)} \rightarrow \text{H}_2\text{(g)} \), the bond enthalpy released is \( 435.8\text{ kJ mol}^{-1} \). Calculate the energy released when \( 6.022 \times 10^{23} \) individual hydrogen atoms combine completely to form \( \text{H}_2\text{(g)} \).
Correct answer · Option 1
\( 217.9\text{ kJ} \)
Explanation
One mole of H atoms is 0.5 moles of H2 molecules. Therefore, energy released = 0.5 × 435.8 kJ = 217.9 kJ.
