-1 Henry's -law constants km of the relation m= km"P for nitrogen and oxygen in water at 0 °C are 0.00102 and 0.0022 mol L bar", respectively. What will be the difference in freezing point between pure water and water in equilibrium, i.e., saturated, with air?
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A: Draw Vapour pressure vs composition (in terms of mole fraction) diagram for an ideal solution.
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Q: 4- Henry's -law constants km' of the relation m= km'P for nitrogen and oxygen in water at 0 °C are…
A: Given: Henry Law Constant for Nitrogen in water =0.00102 mol L-1 bar-1 Henry Law Constant for…
Q: Henry's Law constants for oxygen and nitrogen in water at 0 °C are 2.54 x 10^4 bar and 5.45 x 10^4…
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- The Henry's law constant for CO2(g)CO2(g) in water at 25 ∘C25 ∘C is 29.4 bar·M−129.4 bar·M−1. Estimate the concentration of dissolved CO2(g)CO2(g) in a carbonated soft drink pressurized with 1.801.80 bar of CO2(g)CO2(g).At 20 oC, the vapour pressure of pentane is 58kPa and the vapor pressure of hexane is 16 kPa. a) Estimate the pressure at which solution containing 258 g of hexane and 144 g of pentane will boil at 20 oC. b) Estimate the molar ratio of hexane to pentane in the vapor phase above this solution.Henry's Law constants for oxygen and nitrogen in water at 0 °C are 2.54 x 10^4 bar and 5.45 x 10^4 bar, respectively. Calculate the lowering of the freezing point of water by dissolved air with 80% N2 and 20% O2 by volume at 1 bar pressure. Assume ideal behavior.
- Calculate the solubility of 1,4-dibromobenzene in benzene at 25.000C and at 45.000 assuming that these two compounds form ideal mixtures. The enthalpy of fusion of 1,4-dibromo benzene is 20.39 kJ mol-1 and its melting point is 87.400C. Report the solubility of 1,4-dibromo benzene in benzene as (a) its mole fraction, and (b) grams of 1,4-dibromo benzene in 1000 grams of benzene.The vapor pressure of pure dichloromethane at 298 K is 57.3 kPa. What is its vaporpressure above its mixture with chloroform with 8:2 molar ratios of dichloromethane to chloroform (consider their mixture an ideal solution).Assuming benzene and toluene form ideal solution, what is the mole fraction of toluene in a solution that has a total vapor pressure of 88.98 torr at 20.0oC and 1.0 bar? The vapor pressures of toluene and benzene at 20.0oC and 1.0 bar are 22.14 torr and 75.01 torr, respctively.
- Methanol and Ethanol form an Ideal solution. The vapour pressure of pure Ethanol and pure Methanol at 200C is 44mmHg and 94mmHg respectively. A mixture of 30g of methanol (CH3OH) and 45g of ethanol (CH3CH2OH) is prepared. (RAM: C= 12, O=16, H=1). Calculate: the mole fraction of methanol in the solution the total pressure of the vapour above the solution at 200C the mole fraction of methanol in the vapour above the solution.At 300 K, the vapour pressures of dilute solutions of HCI in liquid GeCI4 are as follows: x(HCI) 0.005 0.012 0.019p/kPa 320 76.9 121 .8 Show that the solution obeys Henry's law in th is range of mole fractions and calculate Henry's law constant at 300 K.The weight fraction of methanol in an aqueous solution is 0.64. The mole fraction of methanol (x) satisfies a. X < 0.5 b. 0.5 < XM < 0.64 c. xu = 0.5 d. Xu ~ 0.5
- The osmotic pressu re of an aqueous solution of urea at 300 K is 150 kPa. Calculate the freezing point of the same solution.The following information pertains to nitrobenzene: Normal melting point = 5.7°C Kf = 7.00°C/m, Normal boiling point = 210.8°C Kb = 5.24°C/m. If 0.100 mol of a non-volatile non-electrolyte is dissolved in 100 g of nitrobenzene, what will be the boiling point of the resulting solution?Assume you are interested in exploring the use of ammonium nitrate (NH4NO3) as the active ingredient in an inexpensive home-made cold pack. You decide that a practical cold pack should be able to depress the temperature of 1 kg of human muscle tissue by 5 oC. Now you need to know the amount of NH4NO3 required to achieve this. Ammonium nitrate is a highly water soluble solid. You believe the enthalpy of dissolution for NH4NO3 must be determined. To this end, you add 2.339 g of NH4NO3 to 99.7 mL of water at 23.7 °C in a constant-pressure calorimeter and close the calorimeter. The temperature of the water decreases to a minimum of 21.9 °C. 1a. Assume the density and specific heat of water is 1.00 g/mL and 4.184 J/g °C, respectively. Using the data above, determine the for ammonium nitrate in water. Assume the heat capacity of the calorimeter is negligible.