Butane reacts with oxygen to produce carbon d | vedclass

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(C) The balanced chemical equation is: $C_4H_{10} + \frac{13}{2} O_2 ightarrow 4 CO_2 + 5 H_2O$. Molar mass of $C_4H_{10} = 4 	imes 12 + 10 	imes

Vedclass · Accepted Answer

$138$

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(C) The balanced chemical equation is: $C_4H_{10} + \frac{13}{2} O_2 ightarrow 4 CO_2 + 5 H_2O$. Molar mass of $C_4H_{10} = 4 	imes 12 + 10 	imes 1 = 58 \ g \ mol^{-1}$. Molar mass of $O_2 = 2 	imes 16 = 32 \ g \ mol^{-1}$. Moles of $C_4H_{10} = \frac{174 	imes 10^3 \ g}{58 \ g \ mol^{-1}} = 3000 \ mol$. Moles of $O_2 = \frac{320 	imes 10^3 \ g}{32 \ g \ mol^{-1}} = 10000 \ mol$. According to the stoichiometry,$1 \ mol$ of $C_4H_{10}$ requires $6.5 \ mol$ of $O_2$. For $3000 \ mol$ of $C_4H_{10}$,$O_2$ required $= 3000 	imes 6.5 = 19500 \ mol$. Since only $10000 \ mol$ of $O_2$ is available,$O_2$ is the limiting reagent. Moles of $H_2O$ formed $= 5 	imes (\frac{10000}{6.5}) = 7692.3 \ mol$. Mass of $H_2O = 7692.3 \ mol 	imes 18 \ g \ mol^{-1} = 138461.5 \ g$. Since density $= 1 \ g \ mL^{-1}$,volume $= 138461.5 \ mL = 138.46 \ L$. The nearest integer is $138$.

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