Answer:
The pressure of the resulting mixture of gases will be 4.89 atm.
Explanation:
An ideal gas is a theoretical gas that is considered to be composed of randomly moving point particles that do not interact with each other. Gases in general are ideal when they are at high temperatures and low pressures.
The pressure, P, the temperature, T, and the volume, V, of an ideal gas, are related by a simple formula called the ideal gas law:
P*V = n*R*T
where P is the gas pressure, V is the volume that occupies, T is its temperature, R is the ideal gas constant, and n is the number of moles of the gas. The universal constant of ideal gases R has the same value for all gaseous substances. The numerical value of R will depend on the units in which the other properties are worked.
In this case:
Replacing:
P* 35 L= 7 moles* 0.082 [tex]\frac{atm*L}{mol*K}[/tex] * 298 K
Solving:
[tex]P=\frac{ 7 moles* 0.082 \frac{atm*L}{mol*K} * 298 K}{35 L}[/tex]
P= 4.89 atm
The pressure of the resulting mixture of gases will be 4.89 atm.
The pressure (in atm) of the resulting mixture of the gases is 4.89 atm
From the question given above, the following data were obtained:
Mole of N₂ = 3 moles
Mole of O₂ = 4 moles
Total mole = 3 + 4 = 7 moles
Volume (V) = 35 L
Temperature (T) = 25 °C = 25 + 273 = 298 K
Gas constant (R) = 0.0821 atm.L/Kmol
The pressure of the resulting mixture of the gases can be obtained by using the ideal gas equation as illustrated below:
PV = nRT
P × 35 = 7 × 0.0821 × 298
P × 35 = 171.2606
Divide both side by 35
P = 171.2606 / 35
Therefore, the pressure of the resulting mixture of the gases 4.89 atm
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