A student adds 4.00 g of dry ice to an empty balloon. What will be the volume of the balloon at
25°C and 1 atm of pressure after all of the dry ice sublimes?

V= 2.45 L

Explanation:

Given data:

Volume of balloon = ?

Temperature = 25 °C (25+273 = 298 K)

Pressure of gas = 1 atm

Mass of ice = 4.00 g

Solution:

Formula:

PV = nRT

P = Pressure

V = volume

n = number of moles

R = ideal gas constant

T = temperature

Number of moles:

Number of moles = mass/molar mass

Number of moles = 4.00 g/ 44 g/mol

Number of moles = 0.1 mol

Now we will put the values:

Ideal gas constant = R = 0.0821 atm.L/mol.K

PV = nRT

V = nRT/P

V = 0.1 mol × 0.0821 atm.L/mol.K × 298 K / 1 atm

V = 2.45 L

mark him as !

fe 55.85 g/mol and h2o 18.02 g/mol.