Final answer:
The pressure of CO₂ in a 49 L cylinder at 22°C, containing 179 g of CO₂, is approximately 0.527 atmospheres, calculated using the ideal gas law.
Step-by-step explanation:
To calculate the pressure of CO₂ inside the cylinder, we can use the ideal gas law, which is PV = nRT. Given that the mass of CO₂ is 179 g and the molar mass of CO₂ is approximately 44.01 g/mol, we can find the number of moles (n) of CO₂. First, divide the mass by the molar mass:
n = 179 g / 44.01 g/mol = 4.07 mol
Next, convert the temperature to Kelvin:
T = 22°C + 273.15 = 295.15 K
The volume (V) is 49 L, and the ideal gas constant (R) is 0.0821 L·atm/mol·K. Now we can solve for pressure (P):
P = (nRT) / V = (4.07 mol)(0.0821 L·atm/mol·K)(295.15 K) / 49 L = 0.527 atm
Therefore, the pressure of CO₂ in the cylinder at 22°C is approximately 0.527 atmospheres.