rank the gases Ar, N2,CH4, and C2H6 in order of the increasing density at STP

answer: CH4<N2<C2H6<Ar
please help me solve this

Sure, here's a playful answer for you:

If these gases were high school students, their rankings based on increasing density at STP would be as follows:

1. Methane (CH4): Picture a tiny, lightweight cheerleader who just floats around effortlessly.
2. Nitrogen (N2): Think of Nitrogen as an average student, not too heavy and not too light. Just kind of chill and goes with the flow.
3. Ethane (C2H6): Ethane is like that slightly bigger football player who adds a bit more mass to the equation.
4. Argon (Ar): Finally, we have Argon, the heavyweight wrestler. It's the largest of the group and takes up the most space.

So, in terms of density, the ranks would be: CH4 < N2 < C2H6 < Ar. Hope that helps!

To rank the gases Ar, N2, CH4, and C2H6 in order of increasing density at STP (standard temperature and pressure), we need to compare their molar masses. The gas with the lowest molar mass will have the lowest density, and the gas with the highest molar mass will have the highest density.

The molar mass of Ar (argon) is approximately 39.95 g/mol.
The molar mass of N2 (nitrogen) is approximately 28.02 g/mol.
The molar mass of CH4 (methane) is approximately 16.04 g/mol.
The molar mass of C2H6 (ethane) is approximately 30.07 g/mol.

Based on the molar masses, we can rank the gases:

CH4 < N2 < C2H6 < Ar

Therefore, CH4 has the lowest density, followed by N2, C2H6, and Ar.

To determine the rank of gases in increasing density at Standard Temperature and Pressure (STP), we need to consider their molecular masses.

1. Categorize the given gases and their molecular formulas:
- Argon (Ar)
- Nitrogen gas (N2)
- Methane (CH4)
- Ethane (C2H6)

2. Calculate the molecular masses of the gases:
- Ar: Since it is a noble gas, its atomic mass is its molecular mass. Ar has a molecular mass of 40 g/mol.
- N2: Nitrogen gas (N2) consists of two nitrogen atoms with an atomic mass of 14 g/mol each. Therefore, the molecular mass of N2 is 2 * 14 g/mol = 28 g/mol.
- CH4: Methane (CH4) contains one carbon atom with an atomic mass of 12 g/mol and four hydrogen atoms with an atomic mass of 1 g/mol each. The molecular mass of CH4 is 12 g/mol + 4 * 1 g/mol = 16 g/mol.
- C2H6: Ethane (C2H6) consists of two carbon atoms, each with an atomic mass of 12 g/mol, and six hydrogen atoms, each with an atomic mass of 1 g/mol. Therefore, the molecular mass of C2H6 is 2 * 12 g/mol + 6 * 1 g/mol = 30 g/mol.

3. Compare the molecular masses of the gases:
- CH4 has the lowest molecular mass at 16 g/mol.
- N2 has a molecular mass of 28 g/mol.
- C2H6 has a slightly higher molecular mass of 30 g/mol.
- Ar has the highest molecular mass at 40 g/mol.

4. After comparing the molecular masses, we can conclude that the rank of the gases in increasing density at STP is:
CH4 < N2 < C2H6 < Ar

Therefore, at STP, the gases rank in increasing density as follows: CH4, N2, C2H6, and Ar.

at stp, one mole of each occupies the same volume, so density then in the same order as mole mass.

If you want to work it out at stp,
density CH4=molemassCH4/22.4liters
density N2=molemass N2/22.4 liters

and so one.