As discussed in the “Chemistry Put to Work” box in  enriched uranium can be produced by effusion ofgaseous UF6 across a porous membrane. Suppose a processwere developed to allow effusion of gaseous uranium atoms,U(g). Calculate the ratio of effusion rates for 235U and 238U,and compare it to the ratio for UF6 given in the essay.

Given the following data from the experiment, calculate the molar volume of hydrogen gas at STP. Be sure to show all of your calculations. Note: You can assume the solution level was the same inside and outside of the tube at the end of the experiment.  Mass of metal used : 0.0862 g Temperature of the gas collected : 24.0 °C Vapor pressure of water at 24 °C : 22.4 torr Volume of gas collected : 89.4 mL Room atmospheric pressure : 757 torr Gas constant : 0.0821 L • atm / K • mol

Ozone molecules in the stratosphere absorb much of the harmful radiation from the sun. How many ozone molecules are present in 4.00 L of air under the stratospheric ozone conditions of 249 K temperature and 1.67 × 10−3 atm pressure?

What is the experimental molar mass (that is, calculated from the data given and not taken from the periodic table) of magnesium if 0.0204 grams of magnesium generates 20.54 mL of hydrogen at 24.6 °C with a hydrogen partial pressure of 761.7 torr? Note that the partial pressure of water vapor has already been subtracted from the total pressure. O25.9 g/mol O26.0 g/mol O 24.2 g/mol 23.8 g/mol O 20.9 g/mol

If I react 20.0 grams of hydrogen with 200. grams of oxygen in the formation of water, what volume of water vapor is produced at 500.K and 1.00 atm?

Suppose 125 g of NO3- flows into a swamp each day. What volume of N2 would be produced each day at 17.0°C and 1.00 atm if the denitrification process were complete?

In an experiment, 175 mL of nitrogen gas was collected over water at 23.5 oC and 757 mmHg. What mass of nitrogen gas was obtained? At the temperature of the gas (23.5 oC), the vapor pressure of water is 21.8 mmHg.