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(C) The total pressure is calculated using the ideal gas equation: $PV = n_{total}RT$.First,calculate the number of moles of each gas:$n_{O_2} = \frac

Vedclass · Accepted Answer

$25.18$

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(C) The total pressure is calculated using the ideal gas equation: $PV = n_{total}RT$.First,calculate the number of moles of each gas:$n_{O_2} = \frac{4 \ g}{32 \ g/mol} = 0.125 \ mol$$n_{H_2} = \frac{2 \ g}{2 \ g/mol} = 1.0 \ mol$Total moles $n_{total} = 0.125 + 1.0 = 1.125 \ mol$.Using $PV = nRT$ with $V = 1 \ L$,$R = 0.082 \ L \ atm \ mol^{-1} \ K^{-1}$,and $T = 273 \ K$:$P 	imes 1 = 1.125 	imes 0.082 	imes 273$$P = 25.18 \ atm$.

Choose the correct option for the total pressure (in $atm$) in a mixture of $4 \ g$ $O_2$ and $2 \ g$ $H_2$ confined in a total volume of $1 \ L$ at $0^{\circ} C$ is :
$\left[ \text{Given } R = 0.082 \ L \ atm \ mol^{-1} \ K^{-1}, T = 273 \ K \right]$

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Choose the correct option for the total pressure (in $atm$) in a mixture of $4 \ g$ $O_2$ and $2 \ g$ $H_2$ confined in a total volume of $1 \ L$ at $0^{\circ} C$ is :$\left[ \text{Given } R = 0.082 \ L \ atm \ mol^{-1} \ K^{-1}, T = 273 \ K \right]$