The Kelvin temperature required for 0.0470 mol of helium gas to fill a balloon to 1.20 L under 0.878 atm is: a. 0.679 K b. 14.4 K c.273 K d. 298 K e. 307 K

Answer 1

To find the Kelvin temperature, we can use the ideal gas law equation:

PV = nRT

Where:
P = pressure (0.878 atm)
V = volume (1.20 L)
n = number of moles (0.0470 mol)
R = gas constant (0.0821 L∙atm/mol∙K)

First, let's convert the pressure to atm:

0.878 atm

Now we can plug in the values and solve for T (temperature):

(0.878 atm)(1.20 L) = (0.0470 mol)(0.0821 L∙atm/mol∙K)(T)

1.0536 = 0.0038687T

T ≈ 271.8 K

Rounded to three significant figures, the Kelvin temperature required for 0.0470 mol of helium gas to fill a balloon to 1.20 L under 0.878 atm is 272 K.

The closest option is c. 273 K.