Estimate the number of moles of gas (and mass of gas assuming that it is all N2) inside your family car (or a friends if you don't have one). If the amount of gas was compressed at constant temperature to fit inside a coke can what would the pressure inside the coke can be?
Did i solve this correctly,
28.317 l x 115ft^3 = 3256 l at a standard temperature (0 C, 40 F)
3256 l x 1mole N2/22.44 l = 145.4 moles N2
Number of moles = 145.4 moles N2
145.4 moles N2/22.4 l = 6.49
28/6.49=4.3
Im kind of stuck right here, what do i need to do next?
Also, are the units correct here, what are the units that should be on 6.49 ex.?
I assume 28.317 is the conversion factor for cubic feet to L and I assume 115 ft^3 is the volume of the inside of the car.
28.317 l x 115ft^3 = 3256 l at a standard temperature (0 C, 40 F)
3256 l x 1mole N2/22.44 l = 145.4 moles N2
Number of moles = 145.4 moles N2
You are ok to here although I didn't check the math. I don't get what follows.
145.4 moles N2/22.4 l = 6.49
28/6.49=4.3
You have mols (assuming the math is right) at 145.4. Convert to mass by
145.5mol x (28 g/1 mol) = ?
Then to convert to pressure inside a coke can, it will be
PV = nRT. You know n,R, T and you will need the volume of the empty coke can. Solve for pressure in atm.
To estimate the number of moles of gas and the mass of gas in your car, you have correctly calculated that there are 145.4 moles of N2 gas.
To find the mass of the gas, you can use the molar mass of N2, which is approximately 28 g/mol. So, the mass of the N2 gas is:
145.4 moles N2 * 28 g/mol = 4071.2 grams or 4.0712 kg (rounded to four decimal places).
Now, let's move on to the second part of the question, which asks about the pressure inside the coke can if the gas was compressed at constant temperature.
To solve this, we can use the ideal gas law equation:
PV = nRT
Where:
P is the pressure
V is the volume
n is the number of moles
R is the ideal gas constant (approximately 8.314 J/(mol*K))
T is the temperature (in Kelvin)
We will assume that the temperature remains constant during the compression, so the initial and final temperatures are the same.
Let's convert the volume of the car to liters (note that 1 ft^3 = 0.0283168466 m^3 = 28.3168466 liters):
V = 3256 liters
Using the ideal gas law equation, rearrange it to solve for P:
P = (nRT)/V
Substituting the values:
P = (145.4 moles * 8.314 J/(mol*K) * T) / 3256 liters
Since you haven't provided the temperature, we cannot calculate the exact pressure. However, this equation can be used to find the pressure given the temperature. Plug in the temperature value in Kelvin and perform the calculation to find the pressure.
I hope this explanation helps you solve the problem!