The enthalpies of combustion of S_{(s)} and H | vedclass

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(C) The formation reaction of $H_2SO_{4(l)}$ is: $S_{(s)} + H_{2(g)} + 2O_{2(g)} \rightarrow H_2SO_{4(l)}$.We are given:$1) S_{(s)} + O_{2(g)} \righta

Vedclass · Accepted Answer

$-820$

Vedclass · Answer

(C) The formation reaction of $H_2SO_{4(l)}$ is: $S_{(s)} + H_{2(g)} + 2O_{2(g)} \rightarrow H_2SO_{4(l)}$.We are given:$1) S_{(s)} + O_{2(g)} \rightarrow SO_{2(g)}$; $\Delta H_1 = -300 \ kcal \ mol^{-1}$$2) H_{2(g)} + 1/2 O_{2(g)} \rightarrow H_2O_{(l)}$; $\Delta H_2 = -290 \ kcal \ mol^{-1}$$3) SO_{2(g)} + 1/2 O_{2(g)} \rightarrow SO_{3(g)}$; $\Delta H_3 = -100 \ kcal \ mol^{-1}$$4) SO_{3(g)} + H_2O_{(l)} \rightarrow H_2SO_{4(l)}$; $\Delta H_4 = -130 \ kcal \ mol^{-1}$Adding equations $(1) + (2) + (3) + (4)$:$S_{(s)} + O_{2(g)} + H_{2(g)} + 1/2 O_{2(g)} + SO_{2(g)} + 1/2 O_{2(g)} + SO_{3(g)} + H_2O_{(l)}$ $\rightarrow SO_{2(g)} + H_2O_{(l)} + SO_{3(g)} + H_2SO_{4(l)}$Canceling common species on both sides:$S_{(s)} + H_{2(g)} + 2O_{2(g)} \rightarrow H_2SO_{4(l)}$$\Delta H_f = \Delta H_1 + \Delta H_2 + \Delta H_3 + \Delta H_4 = (-300) + (-290) + (-100) + (-130) = -820 \ kcal \ mol^{-1}$.

Similar Questions

The difference between the reaction enthalpy change $(\Delta _r H)$ and reaction internal energy change $(\Delta _r U)$ for the reaction $2C_6H_{6(l)} + 15O_{2(g)} \longrightarrow 12CO_{2(g)} + 6H_2O_{(l)}$ at $300 \ K$ is $....$ $J \ mol^{-1}$ $(R = 8.314 \ J \ mol^{-1} \ K^{-1})$

For a spontaneous process, the correct statement$(s)$ is (are):

$5 \, mol$ of an ideal gas at $100 \, K$ are allowed to undergo reversible compression till its temperature becomes $200 \, K$. If $C_v = 28 \, J \, K^{-1} \, mol^{-1}$,calculate $\Delta U$ and $\Delta pV$ for this process. $(R = 8.0 \, J \, K^{-1} \, mol^{-1})$

At the temperature $T$ $(K)$ for the reaction: $X_2O_{4(l)} \rightarrow 2XO_{2(g)}$,given $\Delta U = x \ kJ \ mol^{-1}$ and $\Delta S = y \ J \ K^{-1} \ mol^{-1}$. The Gibbs energy change for the reaction is: (Assume $X_2O_4$ and $XO_2$ are ideal gases)

Assertion $(A)$: If heat of combustion of $C_2H_6$ is $X \ kJ \ mol^{-1}$,heat liberated on combustion of $150 \ g$ of $C_2H_6$ is $5X \ kJ$.
Reason $(R)$: Enthalpy is an extensive property.

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