Question

An empty water bottle is full of air at 15°C and standard pressure. The volume of the bottle is 0. 500 liter. How many moles of air are in the bottle? The water bottle contains mole of air.

Answer 1

The moles of gas in the bottle has been 0.021 mol.

The ideal gas has been given as the gas where there has been negligible amount of interatomic collisions. The ideal gas equation has been given as:

$PV=nRT$

Computation for the moles of gas

The given gas has standard pressure, $P=1\rm atm$

The volume of the gas has been, $V= 0. 500 \;\rm L$

The temperature of the gas has been, $T=15^\circ \text C\\ T=288\;\rm K$

Substituting the values for the moles of gas, n:

$\rm 1\;\times\; 0. 500 =\textit n\;\times\;0.08214\;atm.L/mol.K\;\times\;288\;K\\\\ \textit n=\dfrac{0. 500}{0.08214\;\times\;288} \;mol\\\\ \textit n=0.021\;mol$

The moles of gas in the bottle has been 0.021 mol.

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