Respuesta :
Answer: 0.24 moles
Explanation: Using IDEAL GAS LAW
[tex]PV=nRT[/tex]
where,
P = pressure of the gas= 2.0 atm
V = volume of the gas= 3.00L
T =Temperature of gas=[tex]25^0C=(25+273)K=298K[/tex]
n = number of moles of gas=?
R = Gas constant = 0.0821 Latm/moleK
[tex]n=\frac {PV}{RT}=\frac {2.0\times 3.0}{0.0821\times 298}=0.24moles[/tex]
In a hypothetical gas condition, the molecules do not show any attraction and repulsion towards each other and show elastic collision generally are said to follow the ideal gas equation.
0.24 moles of the oxygen must be placed.
How to calculate the moles?
Given,
- The pressure of the gas (P) = 2.0 atm
- The volume of the gas (V) = 3.0 L
- Gas constant (R) = [tex]\rm 0.0821 L\;atm/mol\;K[/tex]
- The number of moles of oxygen (n) = ?
- The temperature of the gas (T) = [tex]\rm 25.0\°C[/tex]
Temperature is converted as:
[tex]\begin{aligned}\rm T &= 25 + 273\\\\&= 298 \;\rm K\end{aligned}[/tex]
Ideal gas law is given by:
[tex]\rm PV = nRT[/tex]
Substituting the values in the above equation:
[tex]\begin{aligned}\rm n &=\dfrac{\rm PV}{\rm RT}\\\\\\\rm n &= \dfrac{2.00 \times 3.00}{0.0821 \times 298}\\\\\\\rm n &= 0.28\;\rm moles\end{aligned}[/tex]
Therefore, 0.24 moles of oxygen is needed.
Learn more about ideal gas law here:
https://brainly.com/question/9424438
