how much faster does krypton diffuse than bromine under the same conditions of temperature and pressure?
What's your problem with using the diffusion rate law?
To determine how much faster krypton diffuses than bromine under the same conditions of temperature and pressure, you'll need to compare their rates of diffusion using Graham's Law of Effusion. Graham's Law states that the rate of effusion or diffusion of a gas is inversely proportional to the square root of its molar mass.
Here's how you can calculate the relative rate of diffusion between krypton and bromine:
1. Find the molar mass of krypton (Kr) and bromine (Br).
The molar mass of krypton is approximately 83.8 g/mol.
The molar mass of bromine is approximately 79.9 g/mol.
2. Calculate the square root of the molar masses.
Square root of krypton's molar mass: √83.8 g/mol = 9.15 g/mol
Square root of bromine's molar mass: √79.9 g/mol = 8.93 g/mol
3. Calculate the relative rate of diffusion.
The relative rate of diffusion is the ratio of the square roots of the molar masses:
Relative rate of diffusion = √(Molar mass of Krypton) / √(Molar mass of Bromine)
= 9.15 g/mol / 8.93 g/mol
= 1.025
Therefore, krypton diffuses approximately 1.025 times faster than bromine under the same conditions of temperature and pressure.