We can use the Ideal Gas Law to determine the pressure exerted by 0.44 moles of CO2 in a 2.6 L container at 25 degrees celsius. The Ideal Gas Law is expressed as:

PV = nRT

Where:

P = Pressure in atmospheres (atm)

V = Volume in liters (L)

n = Number of moles of gas (mol)

R = Universal gas constant (0.08206 L * atm / mol * K)

T = Temperature in Kelvin (K)

First, we need to convert the temperature from degrees Celsius to Kelvin:

T (K) = T (°C) + 273.15

T (K) = 25°C + 273.15

T (K) = 298.15 K

Now, we can plug the values into the Ideal Gas Law and solve for P:

PV = nRT

P = nRT/V

P = (0.44 mol)(0.08206 L * atm / mol * K)(298.15 K) / 2.6 L

P = 4.56 atm

Therefore, the pressure exerted by 0.44 moles of CO2 in a 2.6 L container at 25 degrees Celsius is 4.56 atm.