To solve this problem, we assume ideal gas so that we can use the formula:
PV = nRT
since the volume of the flask is constant and R is universal gas constant, so we can say:
n1 T1 / P1 = n2 T2 / P2
1.9 mol * (21 + 273 K) / 697 mm Hg = n2 * (26 + 273 K) / 841 mm Hg
n2 = 2.25 moles
The moles of gas after the addition of more gas have been 2.25 mol.
To calculate moles of the gas:
We assume ideal gas in order to utilize the formula,
The volume of the flask is constant, and
R is the universal gas constant,
According to the ideal gas,
PV = nRT
Since V and R are constant,
[tex]\rm \dfrac{n_1T_1}{P_1}\;=\;\dfrac{n_2T_2}{P_2}[/tex]
T1 = 21 [tex]\rm ^\circ C[/tex] = 294 K
n1 = 1.9 mol
P1 = 697 mm Hg
T2 = 26 [tex]\rm ^\circ C[/tex] = 299 K
P2 = 841 mm Hg
Substituting the values:
[tex]\rm \dfrac{1.9\;\times\;294}{697}\;=\;\dfrac{n_2\;\times\;299}{841}[/tex]
n2 = 2.25 mol.
The moles of gas after the addition of more gas have been 2.25 mol.
To learn more about ideal gas equation, refer to the link:
https://brainly.com/question/21912477
