The partial molar volumes of water and ethanol in a solution with xH2O = 0.45 at...
The partial molar volumes of water and ethanol in a solution with xH2O = 0.45 at 25 ∘C are 17.0 and 57.5 cm3 mol−1, respectively.
Calculate the volume change upon mixing sufficient ethanol with 6.18 mol of water to give this concentration. The densities of water and ethanol are 0.997 and 0.7893 g cm−3, respectively, at this temperature.
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The partial molar volumes of water and ethanol in a solution
with xH2O = 0.45 at...
please answer 1.) The partial molar volume of water and ethanol in a solution with Xx20=0.60...
please answer
1.) The partial molar volume of water and ethanol in a solution with Xx20=0.60 at 25°C are 17.0 and 57.0 cm mol-, respectively. Calculate the volume change upon mixing sufficient ethanol with 2.00 mol of water to give this concentration. The densities of water and ethanol are 0.997 and 0.7893 g cm , respectively, at this temperature.
An ethanol-water solution is 40.00% ethanol by mass and has a density of 0.9450 (g/cm3) at 25.00°C. The density of pure...
An ethanol-water solution is 40.00% ethanol by mass and has a density of 0.9450 (g/cm3) at 25.00°C. The density of pure ethanol is 0.7850 (g/cm3) and the density of pure water is 0.9970(g/cm3) at this temperature. At these conditions, the partial molar volume of ethanol is 55.00 (cm3/mol) and the partial molar volume of water is 17.5 (cm3/mol). a. Calculate the total volume of a 1000.0 g solution assuming both ideal and non-ideal conditions. b. What does the difference between...
9) An ethanol-water solution is 40.00% ethanol by mass and has a density of 0.9450 (g/cm3) at 25.00°C. The density...
9) An ethanol-water solution is 40.00% ethanol by mass and has a density of 0.9450 (g/cm3) at 25.00°C. The density of pure ethanol is 0.7850 (g/cms) and the density of pure water is 0.9970(g/cms) at this temperature. At these conditions, the partial molar volume of ethanol is 55.00 (cm3/mol) and the partial molar volume of water is 17.5 (cmmol). a. Calculate the total volume of a 1000.0 g solution assuming both ideal and non-ideal conditions. b. What does the difference...
9) An ethanol-water solution is 40.00% ethanol by mass and has a density of 0.9450 (g/cms)...
9) An ethanol-water solution is 40.00% ethanol by mass and has a density of 0.9450 (g/cms) at 25.00°C. The density of pure ethanol is 0.7850 (g/cms) and the density of pure water is 0.9970(g/cms) at this temperature. At these conditions, the partial molar volume of ethanol is 55.00 (cmx/mol) and the partial molar volume of water is 17.5 (cm3/mol). a. Calculate the total volume of a 1000.0 g solution assuming both ideal and non-ideal conditions. b. What does the difference...
explain step by step for each The partial molar volumes of a benzene-carbon tetrachloride solution at...
explain step by step for each The partial molar volumes of a benzene-carbon tetrachloride solution at 25 ° C at a molar fraction of 0.5 are Vb=0.106 Lmol-1 and Vc=0.100 Lmol-1 respectively, where the subindices b and c denote C6H6 and CCl4, what is the volume of the solution formed by each of them? Since the molar volumes are C6H6=0.089 Lmol-1 and CCl4=0.097 mol-1, what is the volume change when mixing one mole of each of them? What can you...
What is the partial molar volume of ethanol (in units of mL/mol) in a solution with water if 168 mL of ethanol...
What is the partial molar volume of ethanol (in units of mL/mol) in a solution with water if 168 mL of ethanol is added to 650. mL of water and the volume increases by only 153 mL ? Take the density of ethanol to be 0.789 g/mL.
An equimolar gaseous mixture of CO2 and CH4 is at 37.8 C and 8.618 MPa. The partial molar volumes...
An equimolar gaseous mixture of CO2 and CH4 is at 37.8 C and 8.618 MPa. The partial molar volumes, 7,, of the components are o.176 and 0.288 m /Ikmol, respectively. The pure component specific volumes, v, are 0.0935 and 0.2668 m3/kmol, respectively Find: (a) The mixture molar volume, v (m/kmol) (b) The percent error using the ideal gas model for the mixture (c) The compressibility factor for the mixture. (d) The volume change of mixing (m/kmol).
An equimolar gaseous mixture...
4. (10 pts.) At ambient temperature and pressure, the molar volumes of pure liquids A and...
4. (10 pts.) At ambient temperature and pressure, the molar volumes of pure liquids A and B are A 40 cm3/mole and 18 cm3/mole, respectively. Consider a liquid solution of A and B for which x 0.20. At that composition, the partial molar volumes of A and B are VA- 38 cm3/mole and Vs -15 cm3/mole, respectively. (a) (3 pts.) Calculate the mean molar volume, V, of the liquid solution. (b) (3 pts.) Calculate AVmix per mole of the liquid...
Partial-molar volume. In a binary solution the partial molar volumes of the two components can be...
Partial-molar volume. In a binary solution the partial molar volumes of the two components can be determined from the mass density N/V as a function of the mole fraction x2 of component two: V, (») = M1 [1+ (1 – x2)M1 + x2M2 22 dp(x2)] p(x2) Ñ 8(x2) dx2 ] and Team - M2 (1. (1 – x2)M1 + x2M2 1 – 22 dp(x2)] p(x2) dx2 ] (22) = (x2) M2 where Mi denotes the molar mass of component i....
Question 1: Molar volume, צ[cm3 morij, for the methanol (1) + water (2) at 298.15 K...
Question 1: Molar volume, צ[cm3 morij, for the methanol (1) + water (2) at 298.15 K and i bar is expressed as V-18.102 + 18.49 1x1 + 4.1 506xỉ [cm 3 mol-1] Show your answers in the boxes. Only numerical answers are required What is the molar volume of the mixture at xi -0.75? [10points] a) cm3 mol- b) What is the partial molar volume of methanol at x,-0.75? [10points] cm3 mol- cWhat is the partial molar volume of water...
please answer
1.) The partial molar volume of water and ethanol in a solution with Xx20=0.60 at 25°C are 17.0 and 57.0 cm mol-, respectively. Calculate the volume change upon mixing sufficient ethanol with 2.00 mol of water to give this concentration. The densities of water and ethanol are 0.997 and 0.7893 g cm , respectively, at this temperature.
9) An ethanol-water solution is 40.00% ethanol by mass and has a density of 0.9450 (g/cm3) at 25.00°C. The density of pure ethanol is 0.7850 (g/cms) and the density of pure water is 0.9970(g/cms) at this temperature. At these conditions, the partial molar volume of ethanol is 55.00 (cm3/mol) and the partial molar volume of water is 17.5 (cmmol). a. Calculate the total volume of a 1000.0 g solution assuming both ideal and non-ideal conditions. b. What does the difference...
9) An ethanol-water solution is 40.00% ethanol by mass and has a density of 0.9450 (g/cms) at 25.00°C. The density of pure ethanol is 0.7850 (g/cms) and the density of pure water is 0.9970(g/cms) at this temperature. At these conditions, the partial molar volume of ethanol is 55.00 (cmx/mol) and the partial molar volume of water is 17.5 (cm3/mol). a. Calculate the total volume of a 1000.0 g solution assuming both ideal and non-ideal conditions. b. What does the difference...
What is the partial molar volume of ethanol (in units of mL/mol) in a solution with water if 168 mL of ethanol is added to 650. mL of water and the volume increases by only 153 mL ? Take the density of ethanol to be 0.789 g/mL.
An equimolar gaseous mixture of CO2 and CH4 is at 37.8 C and 8.618 MPa. The partial molar volumes, 7,, of the components are o.176 and 0.288 m /Ikmol, respectively. The pure component specific volumes, v, are 0.0935 and 0.2668 m3/kmol, respectively Find: (a) The mixture molar volume, v (m/kmol) (b) The percent error using the ideal gas model for the mixture (c) The compressibility factor for the mixture. (d) The volume change of mixing (m/kmol).
An equimolar gaseous mixture...
4. (10 pts.) At ambient temperature and pressure, the molar volumes of pure liquids A and B are A 40 cm3/mole and 18 cm3/mole, respectively. Consider a liquid solution of A and B for which x 0.20. At that composition, the partial molar volumes of A and B are VA- 38 cm3/mole and Vs -15 cm3/mole, respectively. (a) (3 pts.) Calculate the mean molar volume, V, of the liquid solution. (b) (3 pts.) Calculate AVmix per mole of the liquid...
Partial-molar volume. In a binary solution the partial molar volumes of the two components can be determined from the mass density N/V as a function of the mole fraction x2 of component two: V, (») = M1 [1+ (1 – x2)M1 + x2M2 22 dp(x2)] p(x2) Ñ 8(x2) dx2 ] and Team - M2 (1. (1 – x2)M1 + x2M2 1 – 22 dp(x2)] p(x2) dx2 ] (22) = (x2) M2 where Mi denotes the molar mass of component i....
Question 1: Molar volume, צ[cm3 morij, for the methanol (1) + water (2) at 298.15 K and i bar is expressed as V-18.102 + 18.49 1x1 + 4.1 506xỉ [cm 3 mol-1] Show your answers in the boxes. Only numerical answers are required What is the molar volume of the mixture at xi -0.75? [10points] a) cm3 mol- b) What is the partial molar volume of methanol at x,-0.75? [10points] cm3 mol- cWhat is the partial molar volume of water...
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