The heat of reaction $C (s) + \frac{1}{2} O_{2} (g) ⟶ C O (g)$ at $17^{o} C$ and at constant volume is $- 29.29 k c a l$ . Calculate the heat of reaction at constant pressure.

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Solution

Solution:- (A) $- 68.0 K c a l$
Heat change at constant volume for the combustion of carbon $= - 29.29 K c a l$
$C_{(s)} + \frac{1}{2} {O_{2}}_{(g)} ⟶ {C O}_{(g)}$
From the above reaction,
$Δ n_{g} = n_{P} - n_{R} = 1 - \frac{1}{2} = \frac{1}{2}$
Temperature $(T) = 17 ℃ = (17 + 273) K = 290 K (Given)$
Now from first law of thermodynamics,
$Δ H = Δ E + Δ n_{g} R T$
$Δ H = - 29.29 + (\frac{1}{2}) \times 2 \times 10^{- 3} \times 290$
$\Rightarrow Δ H = - 29.29 + 0.29 = - 29 K c a l$
Hence the heat of reaction at constant pressure will be $- 29 K c a l$ .

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The heat of reaction C(s)+12O2(g)⟶CO(g) at 17oC and at constant volume is −29.29 kcal. Calculate the heat of reaction at constant pressure.

The heat of reaction $C (s) + \frac{1}{2} O_{2} (g) ⟶ C O (g)$ at $17^{o} C$ and at constant volume is $- 29.29 k c a l$ . Calculate the heat of reaction at constant pressure.