Dry ice (CO2) 1.28 g was emptied into a 10 L container. The temperature of the container was maintained at 35.1oC.Calculate the pressure of the container when the dry has converted to a gaseou sform? (R= 0.08206 L.atm/mol.K).
First, we need to determine the number of moles of CO2 in the container:
n = m/M
n = 1.28 g / 44.01 g/mol
n = 0.0291 mol
Next, we need to use the ideal gas law to calculate the pressure:
PV = nRT
where P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is the temperature in Kelvin.
We can rearrange this equation to solve for P:
P = nRT/V
P = (0.0291 mol)(0.08206 L.atm/mol.K)(308.1 K) / 10 L
P = 0.073 atm
Therefore, the pressure in the container after the dry ice has converted to a gaseous form is 0.073 atm.
To calculate the pressure of the container when the dry ice has converted to a gaseous form, we can use the ideal gas law equation:
PV = nRT
Where:
P = pressure
V = volume
n = number of moles
R = ideal gas constant
T = temperature
First, we need to calculate the number of moles of CO2 using the given mass of dry ice:
Given mass of CO2 = 1.28 g
Molar mass of CO2 = 44.01 g/mol
Number of moles (n) = mass / molar mass
n = 1.28 g / 44.01 g/mol ≈ 0.029 moles
Now we can substitute the values into the ideal gas law equation:
P * 10 L = 0.029 moles * 0.08206 L.atm/mol.K * (35.1 + 273.15) K
Simplifying the equation:
P = (0.029 * 0.08206 * 308.25) / 10
P ≈ 0.0722 atm
Therefore, the pressure of the container when the dry ice has converted to a gaseous form is approximately 0.0722 atm.