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Calculate the temperature of a hydrogen-oxygen flame assuming that the gases at \( 25^{\circ} \mathrm{C} \) are mixed in stoichiometric proportion and react completely to give \( H_{2} O(g) . \Delta H_{298}^{\circ} \) of combustion of \( \boldsymbol{H}_{2} \) is \( -\mathbf{5 8} \) kcal \( \boldsymbol{m o l}^{-1} \) The reaction is at constant pressure and the \( C_{p} \) values are \( (7 / 2) R \) for each gas. \( (\boldsymbol{R}=\mathbf{2} \boldsymbol{c} \boldsymbol{a} \boldsymbol{l}) \)

1. \( 8583.71 K \)
2. \( 9583.71 K \)
3. \( 4283.71 \mathrm{K} \)
4. None of the above

Correct answer: \( 8583.71 K \)

Solution

The temperature of the hydrogen-oxygen flame is calculated to be 8583.71 K. [AI-generated key — verify before high-stakes use]

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