Answer: 339.84 K
Explanation:
[tex]$We are given: \\$\mathrm{n}=0.46$ moles \\$V=13.3 \mathrm{~L}$\\$\mathrm{P}=734 \mathrm{~mm} \mathrm{Hg}=0.965 \mathrm{~atm}$\\Putting these values in ideal gas equation we get:\\$0.965$ batm * $13.3 \mathrm{~L}=0.46 \mathrm{~mol} * 0.0821 \frac{\mathrm{atmL}}{\mathrm{molK}} * \mathrm{~T}$\\$\mathrm{T}=\frac{0.965 * 13.3}{0.46 * 0.0821} \mathrm{~K}$$\mathrm{T}=339.84 \mathrm{~K}$[/tex]
