A piece of solid carbon dioxide with a mass of 5.60 g is placed in a 10.0-L vessel that already contains air at 715 torr and 23 C
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After CO2 vaporizes what is the partial press of CO2 and total pressure?
To determine what happens when the solid carbon dioxide is placed in the vessel, we need to consider the conditions of the initial air and the physical properties of carbon dioxide.
First, we need to convert the initial pressure from torr to atm. We know that 1 atm is equal to 760 torr, so the initial pressure is:
715 torr / 760 torr/atm = 0.94 atm
Next, we need to calculate the number of moles of carbon dioxide in the 5.60 g sample. To do this, we need to use the molar mass of carbon dioxide, which is 44.01 g/mol.
Number of moles = mass / molar mass
Number of moles = 5.60 g / 44.01 g/mol
Number of moles = 0.127 moles
Now, using the ideal gas law equation (PV = nRT), we can calculate the final pressure when the solid carbon dioxide sublimates and fills the 10.0-L vessel at 23°C.
P1V1 = P2V2
P1 = initial pressure = 0.94 atm
V1 = initial volume = 10.0 L
P2 = final pressure (what we're trying to find)
V2 = final volume = V1 (since the vessel is already at the same volume)
Now, we need to consider the temperature. The temperature is given as 23°C, but the ideal gas law requires temperatures to be in Kelvin. So, we need to convert the temperature from °C to Kelvin.
Temperature (K) = 273.15 + Temperature (°C)
Temperature (K) = 273.15 + 23
Temperature (K) = 296.15 K
Now we can rearrange the equation and solve for P2:
P2 = (P1 × V1) / V2
P2 = (0.94 atm × 10.0 L) / 10.0 L
P2 = 0.94 atm
Therefore, the final pressure when the solid carbon dioxide sublimates and fills the 10.0-L vessel is also 0.94 atm.