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Ideal Gas Law
A certain amount of helium gas occupies a volume of $\mathrm{0.04 \mathrm{~m}^3}$ at a temperature of $\mathrm{300 \mathrm{~K}}$ and a pressure of $\mathrm{3 \mathrm{~atm}}$ . Calculate the number of moles of helium gas present.

Option: 1
$0.005 \: \mathrm{moles}$

Option: 2
$1.000 \: \mathrm{moles}$

Option: 3
$5.00 \: \mathrm{moles}$

Option: 4
$21.00 \: \mathrm{moles}$

Answers (1)

best_answer

Given data:

Volume, $\mathrm{V=0.04 \mathrm{~m}^3}$

Temperature, $\mathrm{T=300 \mathrm{~K}}$

Pressure, $\mathrm{P=3 \mathrm{~atm}}$

The ideal gas law equation is:

$\mathrm{ P V=\eta R T }$

Solving for the number of moles, $\eta$ :

$\mathrm{ \eta =\frac{P V}{R T} }$

Plugging in the values and the ideal gas constant $\mathrm{ R=8.314 \mathrm{~J} / \mathrm{mol} \mathrm{K}: }$

$\mathrm{ \eta =\frac{(3 \mathrm{~atm}) \cdot\left(0.04 \mathrm{~m}^3\right)}{(8.314 \mathrm{~J} / \mathrm{mol} \mathrm{K}) \cdot(300 \mathrm{~K})} }$

$\mathrm{\eta \approx 0.005 \mathrm{moles}}$

Therefore ,the correct option is 1

Posted by

Rakesh

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