Question

For the reaction: $H_2\left(g\right)+O_2\left(g\right)=H_{2}O\left(l\right),\Delta C_p=7.63cal/deg;\Delta H_{{25}^{o}C}=68.3Kcal$, what will be the value (in Kcal) of $\Delta H$ at ${100}^{o}C$?

• A. $7.63\times (373-298)-68.3$
• B. $7.63\times {10}^{-3}(373-298)-68.3$
• C. $7.63\times {10}^{-3}(373-298)+68.3$
• D. $7.63\times (373-298)+68.3$

Answer 1

Answer: (C)

$7.63\times {10}^{-3}(373-298)+68.3$

$\Delta C_P=7.63$ $cal/degree$

$\Delta H_{{25}^{o}C}=68.3$ $kcal$

$\Delta H_{{100}^{o}C}=\underset{SensibleHeat}{\underset{}{C_P{\int }_{298}^{373}dT}}+\Delta H_{{25}^{o}C}$

$⟹\Delta H_{{100}^{o}C}=7.63\times {10}^{-3}(373-298)+68.3$