Multiple Choice
Henry's Law Constant for nitrogen in water is 1.67 × 10-4 M • atm–1. If a closed canister contains 0.103 M nitrogen, what would be its pressure in atm?
14. Solutions
Henry's Law Calculations
Back14. Solutions
Henry's Law Calculations
- Multiple Choice
At 0°C and 1.00 atm, as much as 0.84 g of O2 can dissolve in 1.0 L of water. At 0°C and 4.00 atm, how many grams of O2 dissolve in 1.0 L of water?
- Multiple Choice
The atmospheric pressure in a lab is calculated as 1.3 atm. If oxygen gas contributes 62% of this atmospheric pressure, determine its mass (in g) dissolved at room temperature in 25 L of water. The Henry's Law Constant for oxygen in water at this temperature is 5.3 × 10–5 M/atm.
- Multiple ChoiceWhat would be the vapor pressure at 25.0 °C of a solution of 5.00 g of glucose (C6H12O6) in 100.0 g of ethanol (C2H5OH)? Pure ethanol has a vapor pressure of 54.68 mmHg at 25 °C.
- Multiple ChoiceAt 25 °C, the solubility of O2 is 4.55 × 10−3 M at 3.5 atm pressure. What is the solubility of O2 at the same temperature and at 2.0 atm pressure?
- Open Question
At 298 K, the Henry's law constant for oxygen is 0.00130 M/atm. Air is 21.0% oxygen.
- Open Question
At 298 k, the Henry's law constant for oxygen is 0.00130 m/atm. Air is 21.0% oxygen. at 298 k, what is the solubility of oxygen in water exposed to air at 1.00 atm?
- Open Question
At 298 K, the Henry's law constant for oxygen is 0.00130 M/atm. Air is 21.0% oxygen. At 298 K, what is the solubility of oxygen in water exposed to air at 1.00 atm?
- Multiple ChoiceAt 25 degrees Celsius, the Henry's Law constant for hydrogen sulfide (H2S) gas in water is 0.087 M/atm. Calculate the mass in grams of the gas that can be dissolved in 700 mL of water at 25 degrees Celsius and a partial pressure of 1.79 atm.
- Multiple ChoiceAt a certain temperature, the solubility of N2 gas in water at 1.75 atm is 41.3 mg of N2 gas per 100 g water. Calculate the solubility of N2 gas in water, at the same temperature, if the partial pressure of N2 gas over the solution is increased to 3.50 atm.
- Multiple ChoiceCalculate the mass of oxygen (in mg) dissolved in a 5.00 L bucket of water exposed to a pressure of 1.13 atm of air. Assume the mole fraction of oxygen in air to be 0.21 and the Henry's law constant for oxygen in water at this temperature to be 1.3 × 10⁻³ mol/L·atm.
- Multiple ChoiceDetermine the Henry's law constant for ammonia in water at 25°C if an ammonia pressure of 0.022 atm produces a solution with a concentration of 0.77 M. What is the Henry's law constant (k_H) in M/atm?
- Multiple ChoiceDetermine the Henry's law constant for ammonia in water at 25°C if an ammonia pressure of 0.022 atm produces a solution with a concentration of 1.3 M.
- Multiple ChoiceDetermine the solubility of N2 in water exposed to air at 25°C if the atmospheric pressure is 1.2 atm. Assume that the mole fraction of nitrogen is 0.78 in air and the Henry's law constant for nitrogen in water at this temperature is 6.1 × 10^-4 M/atm.
- Multiple ChoiceThe Henry's law constant at 25 °C for CO₂ in water is 0.035 M/atm. What is the solubility of CO₂, in molarity units, in 1.0 L of water when the partial pressure of CO₂ is 2.3 atm?