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Calculate the ratio of the diffusion rates and arrange the gases in order of their speed of diffusion: HBr, Cl2, Kr
Consider the following experiment:
A Kr gas was allowed effuse through a small hole under constant pressure. The 2 L sample of Kr took 96.0 s to effuse. Another gas of unknown identity went through the same conditions. It took a 2 L sample of the unknown gas 55.5 s to effuse. Calculate the molar mass of the unknown gas.
Under the same conditions of temperature and pressure, molecules of an acid in the gas phase effuse through a small hole at 0.702 times the rate of effusion of Ar gas. Calculate the molecular formula of the acid if it only has one hydrogen atom and one other atom.
It takes 54 seconds for N2O gas to effuse from a container. How much time it would take for the same amount of I2 gas to effuse from the same conditions?
A sample of CO2 effuses from a container in 57.0 seconds. How long will it take the same amount of gaseous Br2 to effuse from the same container under identical conditions?