Interpretation:
The total vapor pressure of the mixture at
Concept Introduction:
The equilibrium between a liquid and its vapor produces a characteristic vapor pressure for each substance that depends on the temperature. The lowering of the vapor pressure is caused by a lesser ability of the solvent to evaporate, so equilibrium is reached with a smaller concentration of the solvent in the gas phase. The vapor pressure of a solution is expressed using Raoult’s law:
The vapor pressure of the solvent
Mole fraction: Mole fraction of a substance in a solution is the number of moles of that substance divided by the total number of moles of all substances present. The formula is,
Dalton’s Law:
The total pressure of a gas mixture is the sum of the partial pressures of its component gases.
Where
The partial pressure of the gas can be obtained by multiplying the total pressure of the mixture with the percent of the gases present in the mixture.
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Chapter 5 Solutions
CHEMICAL PRINCIPLES (LL) W/ACCESS
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- For the reaction 2 NH3(g) ⇋ N2(g) + 3H2(g), Kc= 0.395 at 350 degrees Celsius. A sample of NH3 of mass 25.6 g is laced in a reaction vessel of volume 5.00 L and heated to 350 degrees Celsius. What are the equilibrium concentrations of NH3, N2, and H2?arrow_forwardThe vapor pressure of water at 30 °C is 4.24 kPa. Calculate the vapor pressure if 95.0 g of glycerol, C₃H₈O₃(l), is added to 100.0 mL of water. The density of water at 30 °C is 0.996 g・mL⁻¹.arrow_forwardCamphor (C10H16O) melts at 179.8 °C, and it has aparticularly large freezing-point-depression constant,Kf = 40.0 °C/m. When 0.186 g of an organic substance of unknownmolar mass is dissolved in 22.01 g of liquid camphor,the freezing point of the mixture is found to be 176.7 °C.What is the molar mass of the solute?arrow_forward
- The sealed containers of fizzy drinks contain dissolved CO2. This dissolved CO2 is in equilibrium with a small quantity of gaseous CO2 at the top of the container. (a) The partial pressure of CO2 gas in a 250 cm3 can of fizzy drink is 3.0 atm at 25 0C. What is the concentration of CO2 in the fizzy drink? (b) If the can contain only the mass of CO2 1.09g as a gas, calculate the pressure in the can when it is stored at 25 0C. (c) The maximum pressure that a can of fizzy drink can withstand is 7 atm. Using the graph below, determine the maximum temperature at which a can, can be stored safely. (concentration=0.093Marrow_forward3) Camphor (CoH160) melts at 179.8 °C, and it has a particularly large freezing point depression constant of 40.0 "C/m. When 0.186 g of an organic substance of unknown molar mass is dissolved in 22.10 g of liquid camphor, the freezing point of the mixture is found to be 176.7 C. What is the molar mass of the organic substance?arrow_forwardWhat is the solubility of carbon dioxide (in units of grams per liter) in water at 25 °C, when the CO2 gas over the solution has a partial pressure of 208 mm Hg? kH for CO2 at 25 °C is 3.36×10-2 mol/L·atm.arrow_forward
- The sealed containers of fizzy drinks contain dissolved CO2. This dissolved CO2 is in equilibrium with a small quantity of gaseous CO2 at the top of the container. (a) The partial pressure of CO2 gas in a 250 cm3 can of fizzy drink is 3.0 atm at 25 0C. What is the concentration of CO2 in the fizzy drink? (b) If the can contain only the mass of CO2 calculated in part (ii) as a gas, calculate the pressure in the can when it is stored at 25 0C. (c) The maximum pressure that a can of fizzy drink can withstand is 7 atm. Using the graph below, determine the maximum temperature at which a can, can be stored safely. (concentration=0.093M)arrow_forwardThe vapor pressure of benzene, C6H6, is 94.6 Torr at 25 °C. A nonvolatile compound was added to 0.300 mol C6H6(l) at 25 °C and the vapor pressure of the benzene in solution decreased to 75.0 Torr. What amount of (in moles) of solute molecules was added to the benzene?arrow_forwardA mixture consiting of 1.000 mol H2O(g) and 1.000 mol CO(g) is placed ina reaction vessel of volume 10.00 L at 800. K. At equilibrium, 0.665 mol CO2(g) is present as a result of the reaction CO (g) + H2O (g)⇋ CO2(g)+H2(g). What are the equilibrium concentrations for all substances?arrow_forward
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