Answer:
[tex]\huge\boxed{V = 2.3\ dm^3}[/tex]
Explanation:
Given:
Moles = n = 0.275 moles
Temperature = T = 75 K
Pressure = P = 1.75 atm
Ideal gas constant = R = 8.314 J/mol K
Required:
Volume = V = ?
Formula:
PV = nRT
Solution:
Rearranging Formula
[tex]\sf V = \frac{nRT}{P} \\\\Putting \ values\\\\V = \frac{(0.275)(8.314)(75)}{1.75} \\\\V = \frac{4.00}{1.75} \\\\V = 2.3\ dm^3[/tex]
Hope this helped!
Taking into account the ideal gas law, the volume of the gas is 0.966 L.
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.
In this case, you know:
Replacing in the ideal gas law:
1.75 atm×V = 0.275 moles×0.082[tex]\frac{atmL}{molK}[/tex]×75 K
Solving:
V= (0.275 moles×0.082[tex]\frac{atmL}{molK}[/tex]×75 K)÷ 1.75 atm
V=0.966 L
Finally, the volume of the gas is 0.966 L.
Learn more about the ideal gas law:
