Balloon- CO2
Balloon- O2
Balloon- He
Balloon- N2
Balloon- CH4
Represented above are five identical balloons, each filled to the same volume at 25 degrees Celcius and 1.0 atmosohere pressure with the pure gases indicated.
A) which balloon contains the greatest mass of gas? explain
B) Compare the average kinetic engeries of the gas molecules in the balloons. explain.
C)Which balloon contains the gas that would be expected to deviate mose from the behavior of an ideal gas? explain.
D)12 hours after being filled, all the balloons have decreased in size. Predict which balloon will be the smallest
Balloon- CO2
Balloon- O2
Balloon- He
Balloon- N2
Balloon- CH4
Represented above are five identical balloons, each filled to the same volume at 25 degrees Celcius and 1.0 atmosohere pressure with the pure gases indicated.
A) which balloon contains the greatest mass of gas? explain
Look at PV=nRT. If P is the same, V is the same, R and T are constants (and therefore the same), then n must be the same for each gas. So calculate for a number of mols (just pick a number, such as 1) the molar mass.
B) Compare the average kinetic engeries of the gas molecules in the balloons. explain.
KE = 1/2 mv2
C)Which balloon contains the gas that would be expected to deviate mose from the behavior of an ideal gas? explain.
Deviations from ideal behavior are a function of size and attraction to other molecules. Look for the molecule that is the largest and might have some attractions to each other.
D)12 hours after being filled, all the balloons have decreased in size. Predict which balloon will be the smallest
I would look for the molecule that I thought might have the best chance of getting through the pores of the balloon walls.
For A)
wat do i plug in if they don't give me a volume.and will i get the number of moles from the PV=nRT, or is there another step?
For B)
what do i do if they don't give me a volume?
Assume any volume you wish. It doesn't matter as long as you use the same number for all of them. And there is no other step. Just use 1 for P, 22.4 for V, (although you can pick any number), use 0.08206 for R and use 273 for T. But I had envisioned you doing it simpler than that. Since the problem says the same conditions, then we know P is the same, we know V is the same, we know R is the same and we know T is the same;therefore, n (the number of mols) MUST be the same. So make it easy on yourself and pick 1 mol for n to start with. NOW, calculate the mass of 1 mol of CO2, O2, N2, He, etc etc. That will be 44 g for CO2, 32 g for O2, 28 g for N2, etc. You get the idea? Then you just compare to see which balloon has the highest mass and which the lowest mass.
I gave you the formula for KE which is 1/2*mass*velocity2. But the average KE is proportional to the temperature; that is, at the same temperature, all gases have the same average KE. The masses will be different and the speeds of the small molecules will be greater than those of larger molecules but the average KE will be the same.
e
a)CO2- has highest molecular weight
b) all of them same because kinetic energy is determined by temperature, and that's the same
c)CO2- has most electrons
d) He-smallest size
Sorry, I didn't quite understand your question. Could you please rephrase it?
For B), if they don't give you a volume, you can still compare the average kinetic energies of the gas molecules using the formula KE = 1/2 * mv^2. The mass (m) and velocity (v) of the gas molecules are independent of volume. Only the number of gas molecules (n) would be affected by the volume, but since we are comparing the average kinetic energies, the individual masses of the gas molecules and their velocities are what matter. So you can still compare the average kinetic energies without needing the volume information.
In general, the average kinetic energy of gas molecules is directly proportional to the temperature. So at the same temperature (which is given as 25 degrees Celsius), all the gas molecules in the balloons will have the same average kinetic energy, regardless of their mass or volume.
For C), deviations from ideal gas behavior are typically due to intermolecular forces and the size of the gas molecules. Larger molecules or molecules with stronger intermolecular forces tend to deviate more from ideal gas behavior. From the given options, you can consider the molecule that is the largest or has the potential for stronger intermolecular attractions. In this case, CH4 (methane) might exhibit the most deviation from ideal gas behavior due to its larger size compared to the other gases and the possibility of some intermolecular attractions between methane molecules.
For D), in general, the gas molecules in the balloon that will decrease in size the most are those that can easily escape through the pores of the balloon material. Typically, smaller molecules and molecules that are more easily compressed will escape more easily and cause the balloon to shrink. So, from the given options, helium (He) is the lightest gas and also has smaller atomic/molecular size, making it more likely to escape through the balloon pores compared to the other gases. Therefore, the helium-filled balloon is likely to be the smallest after 12 hours.