Answer:
The volume of the balloon would be (580.12m) cm^3
Explanation:
From the ideal gas equation,
PV = nRT
P is pressure in the balloon = 742 mmHg = 742/760 = 0.976 atm
V is the volume of the balloon
n is the number of moles of carbon dioxide in the balloon. Let the mass of carbon dioxide be m.
n = mass/MW = m/44 = (0.023m) mol
R is gas constant = 82.057 cm^3.atm/mol.K
T is temperature of the balloon = 27 °C = 27 + 273 = 300 K
V = 0.023m × 82.057 × 300/0.976 = (580.12m) cm^3
Answer:
Explanation:
Given:
P = 742 mmHg
= 98925.2 Pa
T = 22 °C
= 295 K
R = 8.3145 J/mol.K
Molar mass of CO2, M = 12 + (16*2)
= 44 g/mol
Number of moles = mass/molar mass
= 28.8/44
= 0.655 mol.
Using ideal gas law,
PV = nRT
V = nRT/P
= 0.655 × 8.3145 × 295/98925.2
= 0.0162 m^3
