Calculate the temperature of a hydrogen-oxygen flame assuming that the gases at 25-C are mixed in stoichiometric proportion and react completely to give H2O g- - H-298 of combustion of H2 is -58 kcal mol-1- The reaction is at constant pressure and the Cp values are 7-2 R for each gas- R - 2cal

The correct option is A 8583.71 K H_2(g)+ (1/2)O_2(g) ⟶ #160; H_2O(g); Δ H^∘= 58 kcal The heat produced during combustion is used to heat the ...

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Standard XII

Chemistry

Molar and Specific Heat Capacity

Calculate the...

Question

Calculate the temperature of a hydrogen-oxygen flame assuming that the gases at $25^{\circ} C$ are mixed in stoichiometric proportion and react completely to give $H_{2} O (g)$ . $Δ H_{298}^{\circ}$ of combustion of $H_{2}$ is $- 58 k c a l m o l^{- 1}$ . The reaction is at constant pressure and the $C_{p}$ values are $(7 / 2) R$ for each gas. $(R = 2 c a l)$

8583.71 K

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4283.71 K

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None of the above

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Solution

The correct option is A $8583.71 K$
$H_{2} (g) + (1 / 2) O_{2} (g) ⟶ H_{2} O (g); Δ H^{\circ} = - 58 k c a l$
The heat produced during combustion is used to heat the product $H_{2} O (g)$ of heat capacity $7 / 2 R$ .
Thus, $Δ H = n . C_{p} . Δ T$
$58000 = 1 \times (7 / 2) \times 2 \times (T_{2} - 298)$
$∴ T_{2} = 8583.71 K$

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The correct option is A 8583.71KH2(g)+(1/2)O2(g)⟶H2O(g);ΔH∘=−58kcalThe heat produced during combustion is used to heat the product H2O(g) of heat capacity 7/2R.Thus, ΔH=n.Cp.ΔT 58000=1×(7/2)×2×(T2−298)∴T2=8583.71K