Of the following gases, will have the greatest rate of effusion at a given temperature. of the following gases, will have the greatest rate of effusion at a given temperature. nh3 hcl ch4 ar hbr

From the given gases, the greatest rate of effusion is of

Explanation:

Rate of effusion of a gas is determined by a law known as Graham's Law.

This law states that the rate of effusion or diffusion of a gas is inversely proportional to the square root of the molar mass of the gas. The equation given by this law follows:

It is visible that molar mass is inversely related to rate of effusion. So, the gas having lowest molar mass will have the highest rate of effusion.

For the given gases:

Molar mass of

Molar mass of

Molar mass of

Molar mass of

Molar mass of

The molar mass of methane gas is the lowest. Thus, it will have the greatest rate of effusion.

Hence, the greatest rate of effusion is of

1. for the first question, we must find the mass of the anhydrous salt, mgso₄. the molar mass for mgso₄·7h₂o is 246.47 g/mol, while that of mgso₄ is 120.37 g/mol.7.834 g mgso₄·7h₂o * 1 mol mgso₄·7h₂o/246.47 g * 1 mol mgso₄/1 mol mgso₄·7h₂o * 20.37 g mgso₄/mol = 0.647 g mgso₄

2. mass of water = mass of sample - mass of anhydrous salemass of water = 7.834 - 0.647 = 7.19 gpercent water in hydrate = 7.19/7.834 * 100 = 91.74%