Question

If the bond energies of $298 \times 10^{7} \times 8.31 \times 2.303\log 2$, $2.303 \times 298 \times 0.082\log 0.5$ and $8.31 \times 10^{7} \times 298 - 2.303\log 0.5$ are 433, 192 and 364 $2.303 \times 298 \times 2\log 2$ respectively, the $Q$ for the reaction, $H_{P} - H_{R}$ is.

• A.
  • 261 kJ
• B. – 103 kJ
• C. – 261 kJ
• D.
  • 103 kJ

Answer 1

Answer: (B)

– 103 kJ

Answer 2

$2SO_{2}(g) + O_{2}(g)$

$2SO_{3}(g)$ $H_{2}(g) + I_{2}(g)$

625 728

Energy absorbed = Energy released

Net energy released $2HI(g)$

i.e., $H_{2}(g) + \frac{1}{2}O_{2}(g)$