What is the order of increasing rate of effusion for the following gases at constant temperature? Put the slowest at the top, or first, and the fastest at the bottom, or last. Mwts: He = 4.0 g; C= 12.0 g; N = 14.0 g; O = 16.0 g; Ar = 39.95 g

Answer 1

The rate of effusion is inversely proportional to the square root of the molar mass of the gas.

Rate of effusion ∝ 1/√(molar mass of the gas)

So, the order of increasing rate of effusion will be as follows:

1. Ar (39.95 g)
2. C (12.0 g)
3. N (14.0 g)
4. O (16.0 g)
5. He (4.0 g)

Therefore, the slowest (or first) gas will be Argon (Ar) and the fastest (or last) gas will be Helium (He).