A balloon has been fillled to a volume of 1.90L with 0.09Omal of helium gas. If 0.0210mol of additional helium is added to the balloon with the temperature and pressure are held constant, what is the new volume of the balloom

2.34 L

Explanation:

Step 1:

Data obtained from the question. This includes:

Initial volume (V1) = 1.90L

Initial mole (n1) = 0.090 mol

Final mole (n1) = 0.090 + 0.0210 = 0.111 mole

Final volume (V2)

Step 2:

Determination of the final volume.

From the ideal gas equation:

PV = nRT

Divide both side by n

PV /n = RT

Divide both side by P

V/n = RT/P

Since the pressure and temperature are constant, then

V/n = constant.

V1/n1 = V2/n2

V1 is the initial volume

V2 is the final volume

n1 is the initial mole

n2 is the final mole.

V1/n1 = V2/n2

1.9 / 0.09 = V2 / 0.111

Cross multiply to express in linear form

V2 x 0.09 = 1.9 x 0.111

Divide both side by 0.09

V2 = (1.9 x 0.111) / 0.09

V2 = 2.34 L

Therefore, the new volume of the balloon is 2.34 L

explanation:

i think option no d is the correct answer