Answer:
12.93 atm.
Explanation:
Given,
mass of nitrogen gas, m = 1.78 g
Volume, V = 0.118 L
Temperature, T = 25° C = 273 +25 = 298 K
Atomic mass of N₂ = 28
[tex]n= \dfrac{1.78}{28}[/tex]
[tex]n = 0.0635[/tex]
Using ideal gas equation
[tex]PV = n RT[/tex]
[tex]P\times 0.118 = 0.0635 \times 0.0806 \times 298 [/tex]
[tex] P = 12.93\ atm[/tex]
Hence, the pressure is equal to 12.93 atm.
The pressure of the nitrogen gas confined to a volume of 0.118 L is 13.16 atm.
The pressure of nitrogen gas can be calculated by using the ideal gas equation.
PV =nRT
P = pressure
V = volume = 0.118 L
n = moles of nitrogen gas
moles = [tex]\rm\dfrac{weight}{molecular\;weight}[/tex]
moles of nitrogen gas = [tex]\rm \dfrac{1.78}{28}[/tex]
Moles of nitrogen gas = 0.0635 moles
R = constant = 0.0821
T = temperature = 25[tex]\rm ^\circ C[/tex] = 298 K
Substituting the values:
P [tex]\times[/tex] 0.118 = 0.0635 [tex]\times[/tex] 0.0821 [tex]\times[/tex] 298
P [tex]\times[/tex] 0.118 = 1.5535
P = 13.16 atm.
The pressure of the nitrogen gas confined to a volume of 0.118 L is 13.16 atm.
For more information about the volume of gas, refer to the link:
https://brainly.com/question/12357202
