A sample of carbon dioxide with a mass of
0.91 g was placed in a 335 mL container at
363 K. What is the pressure exerted by the
gas?
Answer in units of atm
Use PV = nRT
n isn't given but n = grams CO2/molar mass CO2
To determine the pressure exerted by the gas, we can use the ideal gas law equation:
PV = nRT
Where:
P = Pressure (in units of atm)
V = Volume (in units of L)
n = Number of moles of the gas
R = Ideal gas constant (0.0821 L·atm/(mol·K))
T = Temperature (in units of Kelvin)
First, we need to calculate the number of moles (n) of carbon dioxide using its mass.
The molar mass of carbon dioxide (CO2) is:
C = 12.01 g/mol
O = 16.00 g/mol (there are 2 oxygen atoms)
So, the molar mass of CO2 is:
Molar mass (CO2) = 12.01 g/mol + 2(16.00 g/mol) = 44.01 g/mol
Now, we can calculate the number of moles (n) of carbon dioxide:
n = mass/molar mass = 0.91 g / 44.01 g/mol
Next, convert the volume from milliliters (mL) to liters (L):
335 mL * 1 L/1000 mL = 0.335 L
Finally, we can substitute the known values into the ideal gas law equation and solve for pressure (P):
P * 0.335 L = (0.91 g / 44.01 g/mol) * (0.0821 L·atm/(mol·K)) * 363 K
Simplifying the equation:
P = (0.91 g / 44.01 g/mol) * (0.0821 L·atm/(mol·K)) * 363 K / 0.335 L
Now, we can perform the calculation to find the pressure (P).