How many moles of CO2 would be contained in a cylinder the size of a pop can (355 ml) at a temperature of 300K and 10 atm? How much would that weigh?
To find the number of moles of CO2 in the given cylinder size, we'll be using the ideal gas law equation:
PV = nRT
Where:
P = Pressure (in atm)
V = Volume (in liters)
n = Number of moles
R = Ideal gas constant (0.0821 L·atm/(mol·K))
T = Temperature (in Kelvin)
First, we need to convert the volume of the pop can from milliliters to liters:
355 ml = 0.355 L
Next, we substitute the given values into the equation and solve for the number of moles (n):
PV = nRT
(10 atm) * (0.355 L) = n * (0.0821 L·atm/(mol·K)) * (300K)
3.55 = 0.0821n
Now, we solve for n:
n = 3.55 / 0.0821
n ≈ 43.32 moles
Therefore, the pop can-sized cylinder would contain approximately 43.32 moles of CO2.
To find the weight, we need to know the molar mass of CO2, which is approximately 44.01 g/mol.
Finally, we can calculate the weight (mass) of the CO2:
Weight = Number of moles × Molar mass
Weight = 43.32 moles × 44.01 g/mol
Weight ≈ 1,905.79 g
Therefore, the CO2 in the given cylinder size would weigh approximately 1,905.79 grams.