The molar heat of formation of NH_4NO_{3(s)} | vedclass

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(B) The reaction is: $NH_4NO_{3(s)} \rightarrow N_2O_{(g)} + 2H_2O_{(l)}$First,calculate the enthalpy change of the reaction $(\Delta H)$:$\Delta H =

Vedclass · Accepted Answer

$-125.04$

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(B) The reaction is: $NH_4NO_{3(s)} ightarrow N_2O_{(g)} + 2H_2O_{(l)}$First,calculate the enthalpy change of the reaction $(\Delta H)$:$\Delta H = [\Delta H_f(N_2O) + 2 	imes \Delta H_f(H_2O)] - [\Delta H_f(NH_4NO_3)]$$\Delta H = [81.46 + 2 	imes (-285.78)] - (-367.54)$$\Delta H = [81.46 - 571.56] + 367.54 = -122.56 \ kJ \ mol^{-1}$Next,calculate the change in the number of moles of gaseous species $(\Delta n_g)$:$\Delta n_g = n_{g, 	ext{products}} - n_{g, 	ext{reactants}} = 1 - 0 = 1$Using the relation $\Delta H = \Delta U + \Delta n_g RT$:$-122.56 = \Delta U + (1 	imes 8.314 	imes 10^{-3} 	imes 298)$$-122.56 = \Delta U + 2.477$$\Delta U = -122.56 - 2.477 = -125.037 \approx -125.04 \ kJ \ mol^{-1}$

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For the following combustion reaction occurring in an automobile: $2C_{8}H_{18(g)} + 25O_{2(g)} \to 16CO_{2(g)} + 18H_{2}O_{(g)}$,what are the signs of $\Delta H$,$\Delta S$,and $\Delta G$?

For the process $H_2O_{(l)} (1 \ bar, 373 \ K) \rightarrow H_2O_{(g)} (1 \ bar, 373 \ K)$,the correct set of thermodynamic parameters is:

Identify the correct statements from the following.
$I$. At $0 \ K$,the entropy of pure crystalline materials approaches zero.
$II$. Entropy for the process,$H_2O_{(l)} \longrightarrow H_2O_{(g)}$ decreases.
$III$. Gibbs' energy is a state function.

For the process $H_2O_{(l)} \rightarrow H_2O_{(g)}$ at $100^{\circ}C$ and $1 \ atm$ pressure,which of the following is true?

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