The heat of combustion of ethene (C_2H_4) is | vedclass

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(B) The combustion reaction for ethene is: $C_2H_4(g) + 3O_2(g) \rightarrow 2CO_2(g) + 2H_2O(l)$; $\Delta H = -1411 \, kJ \, mol^{-1}$.From the stoich

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$296.5 \, L$

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(B) The combustion reaction for ethene is: $C_2H_4(g) + 3O_2(g) ightarrow 2CO_2(g) + 2H_2O(l)$; $\Delta H = -1411 \, kJ \, mol^{-1}$.From the stoichiometry,$1 \, mol$ of $C_2H_4$ requires $3 \, mol$ of $O_2$ for combustion,releasing $1411 \, kJ$ of heat.To produce $6226 \, kJ$ of heat,the number of moles of $C_2H_4$ burned is $n = \frac{6226}{1411} \approx 4.4125 \, mol$.The moles of $O_2$ required = $3 	imes n = 3 	imes 4.4125 = 13.2375 \, mol$.At $S.T.P.$,the volume of $1 \, mol$ of gas is $22.4 \, L$.Volume of $O_2 = 13.2375 	imes 22.4 \approx 296.5 \, L$.

The heat of combustion of ethene $(C_2H_4)$ is $1411 \, kJ$. If a certain amount of ethene is burned to produce $6226 \, kJ$ of heat,what is the volume of $O_2$ (at $S.T.P.$) consumed in the process?

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