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Hydrogen gas has a Henry's law constant of 7.8 × 10-4 mol/kg · bar at 25°C when dissolving in water. If the total pressure of gas (H2 gas plus water vapor) over water is 1.00 bar, what is the concentration of H2 in the water in grams per milliliter? (See Appendix G in your textbook for the vapor pressure of water.)
A sample containing 2.40 moles neon gas has a volume of 8.00 L. Assume that the pressure and the temperature remain constant.What is the new volume of gas in liters when a leak allows one-half of the neon atoms to escape?
calculate the mass of sodium nitrate, NaNO3, required to produce 7.00g of oxygen according to the following reaction:
Calculate the concentration of all ionic species at equilibrium after adding 1 g sodium acetate to 0.1 L of a 0.1 M solution of acetic acid. Assume volume stays constant and conditions are at standard state
Gas x effuses 0.629 times as far as oxygen under the same conditions. what is the molar mass of gas x.
If 0.80 g of sulfur dioxide at 10.00 atm pressure (P) dissolves in 5.00 L of water at 25.0°C, how much of it will dissolve in 1 L of water at 9.00 atm pressure (P) and the same temperature?
calculate the colume of a .200 M NaOH solution needed to neutralize 40.0 mL of .600 M H2SO4 solution.
If another sample of the same compound is decomposed and found to contain 8.46 g of oxygen, how many g of carbon must it contain?
use standard reduction potentials to find the equilibrium constant for the following reaction at 25 degrees C.
A gas in a sealed container has a pressure of 125 kPa at a tempurature of 30.0 degrees celcius. If the pressure in the container is increased to 201 k Pa, what is the new tempurature?
Sulfuric acid (H2SO4) is a very strong diprotic acid. If 0.022 moles of sulfuric acid is mixed with water to make 607 mililiter of solution, what is the molarity of H+.
The amount of boiling water required to raise the temperature of 25 kg of water in the bath to body temperature is 4.8 kg. In this process, the heat lost by the boiling water is equal to the heat gained by the room-temperature water.
Determine the partial pressure of each gas in a mixture of gases using Dalton's law of partial pressures
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