Question

A gas mixture contains hbr, no2, and c2h6 at stp. if a tiny hole is made in the container, which gas will effuse fastest?

Answer 1

Using Graham's law of effusion, C2H6 (ethane) will effuse the fastest from a mixture of HBr, NO2, and C2H6 due to its lowest molar mass.

Step-by-step explanation:

When a gas mixture containing HBr, NO2, and C2H6 is contained and a small hole is made in the container, the gas that will effuse fastest can be determined using Graham's law of effusion. This law states that the rate of effusion for a gas is inversely proportional to the square root of its molar mass. Therefore, the lighter a gas molecule, the faster it will effuse. Considering the molar masses of HBr (approximately 81 g/mol), NO2 (approximately 46 g/mol), and C2H6 (approximately 30 g/mol), C2H6 (ethane) has the lowest molar mass and will effuse the fastest at STP (Standard Temperature and Pressure).

Answer 2

This problem is solved by the law of effusion, which states that the rate of effusion is ~ 1/sqrt(molecular weight). Calculate the molecular weights of the different gases: HBr = 80.91 g/mol NO2 = 46.0055 g/mol C2H6 = 30.07 g/mol Thus, the approximate relative rates are HBr ~ 0.112, NO2 = 0.1474 and C2H6 = 0.1824. Answer: C2H6 effuses fastest.