What is the experimental molar mass (that is, calculated from the data given and not taken from the periodic table) of magnesium if 0.0228 grams of magnesium generates 22.57 mL of hydrogen at 21.2 °C with a hydrogen partial pressure of 761.5 torr? Note that the partial pressure of water vapor has already been subtracted from the total pressure. O 25.0 g/mol O 24.3 g/mol O 22.8 g/mol O 20.9 g/mol O 25.2 g/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

Give an example of oxygen use in industry and medicine.

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?

Given that the concentration of CH4 in the atmosphere is 1.8 ppm, calculate the total mass of this gas that is present in the atmosphere. Note that the total mass of the atmosphere is 5.1 x 1018 kg and that its average molar mass is 29.0 g/mol.