Answer :
n = 0.100 moles
At STP (standard temperature pressure), where gas is collected, the temperature is 0°C and the pressure is 1 atm.
[tex]\\$\therefore$ Temperature $(T)=0^{\circ} \mathrm{C}=0^{\circ}+273[/tex]
[tex]=273K[/tex]
[tex]Pressure $(P)=1$ atm.[/tex]
The ideal gas equation indicates that
[tex]\begin{aligned}& P V=n R T \Rightarrow V=\frac{n R T}{P} \\\therefore & R=\text { gas constant }=0.0821 \mathrm{~L} \cdot \mathrm{cetm} / \mathrm{mo} / \cdot K\end{aligned}[/tex]
[tex]\begin{aligned}&V=\frac{0.100 \mathrm{~mol} \cdot \times 0.0821 \mathrm{~L} \cdot \mathrm{atm} / \mathrm{mol} . \mathrm{K} \times 273 \mathrm{~K}}{1 \mathrm{~atm}} \\&V=\frac{2.24 L}{1}\end{aligned}\\[/tex]
[tex]V=2.24L[/tex]
Group of answer choices [tex]2.44L[/tex] .The volume occupied by mole of a given gas at a given temperature and pressure is expressed as the gas's molar volume.
The most typical illustration is the molar volume of a gas at STP, which is equal to [tex]2.44L[/tex] for [tex]1[/tex] mole of any ideal gas at a temperature of [tex]273.15[/tex] Kand a pressure of [tex]1[/tex] atm.
Hence, the volume of the gas is [tex]2.24L[/tex].
What is the STP?
A unit is stated to have a temperature of absolute zero [tex](273 Kelvins)[/tex] and an atmospheric pressure of one atmosphere, or [tex]1[/tex] atm, at standard temperature and pressure. Additionally, at STP, a mole of any gas takes up [tex]22.414 L[/tex] of space. Keep in mind that this idea only applies to gases.
For experimental measurements to be established under standard conditions that allow for comparisons between various sets of data, standard temperature and pressure must be met.
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