When 1.0 g of solid oxalic acid (H_2C_2O_4) | vedclass

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(D) The combustion reaction is: $H_2C_2O_{4(s)} + \frac{1}{2} O_{2(g)} \rightarrow H_2O_{(\ell)} + 2CO_{2(g)}$The change in the number of gaseous mole

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$-241.96 \ kJ/mol$

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(D) The combustion reaction is: $H_2C_2O_{4(s)} + \frac{1}{2} O_{2(g)} ightarrow H_2O_{(\ell)} + 2CO_{2(g)}$The change in the number of gaseous moles is $\Delta n_g = 2 - 0.5 = 1.5$.The internal energy of combustion $(\Delta U_c)$ is calculated as: $\Delta U_c = -\frac{q}{n} = -\frac{C 	imes \Delta T}{n}$.Given $C = 8.75 \ kJ/K$,$\Delta T = 0.312 \ K$,and molar mass of $H_2C_2O_4 = 90 \ g/mol$,the moles $n = \frac{1.0 \ g}{90 \ g/mol} = \frac{1}{90} \ mol$.$\Delta U_c = -\frac{8.75 	imes 0.312}{1/90} = -245.7 \ kJ/mol$.Using the relation $\Delta H = \Delta U + \Delta n_g RT$ at $T = 300 \ K$:$\Delta H = -245.7 + (1.5 	imes 8.314 	imes 10^{-3} 	imes 300) = -245.7 + 3.7413 = -241.9587 \ kJ/mol \approx -241.96 \ kJ/mol$.

Column $I$	Column $II$
$A$. Freezing of water at $273 \ K$ and $1 \ atm$	$P$. $q=0$
$B$. Expansion of $1 \ mol$ of an ideal gas into a vacuum under isolated conditions	$Q$. $w=0$
$C$. Mixing of equal volumes of two ideal gases at constant temperature and pressure in an isolated container	$R$. $\Delta S_{sys} < 0$
$D$. Reversible heating of $H_{2(g)}$ at $1 \ atm$ from $300 \ K$ to $600 \ K$,followed by reversible cooling to $300 \ K$ at $1 \ atm$	$S$. $\Delta U=0$
	$T$. $\Delta G=0$

When $1.0 \ g$ of solid oxalic acid $(H_2C_2O_4)$ is burned in a bomb calorimeter whose heat capacity is $8.75 \ kJ/K$,the temperature increases by $0.312 \ K$. The enthalpy of combustion of oxalic acid at $27 \ ^oC$ is

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