If 5 mol of oxygen gas effuses through an opening in 10 seconds, how long will it take for the same amount of hydrogen gas to effuse under the same conditions? 1.6 s 2.5 s 40 s D 160 s

carbon dioxide diffuses at a rate of .653 m/s. if an unknown gas diffuses at a rate of .479 m/s at the same temperature what is the molar mass of the unknown gas

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The following data describes an initial and final state for an ideal gas. Given that the amount of gas does not change in the process, what was the initial volume (L) of the gas? 5

Consider a reaction between a 3.44 L flask containing nitrogen gas and a 18 L flask of hydrogen gas. Both gases have a temperature of 296 K and the pressures inside both flasks is 1.01 bar. What mass of ammonia (in g) would you expect to be produced at temperature 296 K and a pressure of 1.01 bar?

A gas of unknown molecular mass was allowed to effuse through a small opening under constant pressure conditions. It required 72 s for 1.0 L of the gas to effuse. Under identical experimental conditions it required 27 s for 1.0 L of 02 gas to effuse. Calculate the molar mass of the unknown gas. (Remember that the faster the rate of effusion, the shorter the time required for effusion of 1.0 L; that is, rate and time are inversely proportional.) 367.1175859 X g/mol

2. Sodium sulfide (0,1159 g) and excess hydrochloric acid were reacted together to form 35.75 mL of an unknown gas. The gas was collected over water when the atmospheric pressure was measured to be 767 mmHg. The temperature of the water was 23.0°C. Determine the molar mass, as well as identity, of the gas. Hint: You will need to reference your textbook for the vapor pressure of water.