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
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).
To determine the order of increasing rate of effusion for these gases at constant temperature, you need to compare their molar masses. The lighter the gas, the faster it will effuse. Here is the order from slowest to fastest effusion rate:
1. Argon (Ar): Molar mass of 39.95 g/mol
2. Nitrogen (N): Molar mass of 14.0 g/mol
3. Oxygen (O): Molar mass of 16.0 g/mol
4. Carbon (C): Molar mass of 12.0 g/mol
5. Helium (He): Molar mass of 4.0 g/mol
Therefore, the order of increasing rate of effusion is:
Argon (Ar) > Nitrogen (N) > Oxygen (O) > Carbon (C) > Helium (He)