Q2:
A sample of carbon dioxide(CO2) has a mass of 55g and occupies 3.3L at 100C. What pressure does the gas exert (in kPa)?
Use PV = nRT with R 8.314 and P comes out directly in kPa OR use R = 0.08206 in L*atm/mol*K and find P in atm, then atm x 101.325 = kPa.
To determine the pressure the gas exerts, we can use the ideal gas law, which states that the pressure of a gas is equal to the product of its molar amount, its molar gas constant (R), and its temperature, divided by its volume:
PV = nRT
Where:
P = Pressure of the gas
V = Volume of the gas
n = Number of moles of the gas
R = Molar gas constant (8.314 J/(mol·K))
T = Temperature in Kelvin
First, let's convert the given temperature from Celsius to Kelvin:
T(K) = T(C) + 273.15
So, T(K) = 100 + 273.15 = 373.15 K
Next, we need to calculate the number of moles of carbon dioxide. We can do this by dividing the given mass of carbon dioxide by its molar mass.
The molar mass of carbon dioxide (CO2) is calculated by adding the atomic masses of one carbon atom (12.01 g/mol) and two oxygen atoms (16.00 g/mol each).
Molar mass of CO2 = 12.01 g/mol + 2 * 16.00 g/mol = 44.01 g/mol
Now, we can calculate the number of moles:
n = Mass / Molar mass = 55 g / 44.01 g/mol
Finally, we can substitute the values into the ideal gas law equation to find the pressure:
P = (nRT) / V
Remember to convert the volume from liters to m^3, as the ideal gas constant (R) has units in J/(mol·K).
1 L = 0.001 m^3
Let's do the calculations now.