A liquefied mixture of n-butane, n-pentane, and n-hexane has the following composi- tion in percent: n-C,H10 50 n-C,H12 30 n-C,H14 20 For this mixture, calculate: (a) The weight fraction (b) The mole fraction (c) The mole percent of each component (d) The average molecular weight
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- Prove that M = (mole IL) %3D is % x 10 x d M. M.wtQ/ Prepare 0.1 N and 0.1 M of 98% H,SO4 in 250 ml. M.wt of H,SO4 = 98 g/mol, and its Specific density (SP.gr.) =1.09 . tousityxioA mixture containing acetone (C3H6O) and chloroform (CHCI3) is prepared in which the mole fraction of chloroform is 0.4297. The partial molar volumes of acetone (A) and chloroform (C) for this mixture are VA = 74.166 mL mol mL Vc = 80.235 mol (a) What is the number of moles of each component and the volume (in mL) of the mixture if it has a total mass of 278.0 g? (b) What is the volume of the unmixed components of this mixture (in mL) if their individual molar volumes (in pure form) are mL V (acetone) = 73.993 mol mL V (chloroform) = 85.665 mol Does the total volume of the materials expand or contract upon mixing?
- At an air-water interface, fatty acids such as oleic acid liein a one-molecule-thick layer (monolayer), with the heads in thewater and the tails perpendicular in the air. When 2.50 mg of oleic acid is placed on a water surface, it forms a circular mono-layer 38.6 cm in diameter. Find the surface area (in cm²) occu-pied by one molecule (of oleic acid M=283 g/mol).= STATES OF MATTER Applying like dissolves like For each solute, click the button under the better solvent. H H HO U C solute H I 2 CIH Η 2=0 CaC1₂ H H CH₂ - CH₂-OH Which is the better solvent? CH₂(CH₂) CH3 H₂O CH₂ CH₂OH :0: || CH₂- - CH3 I CH CC14 CH₂OH - CH3 0/5A mixture has 5g of NaCl, 500mg of NH4Cl and 8g of SiO2 What is thepercentage composition of the mixture ?
- One mole of pure hydrochloric acid, HCl, requires 100 g of 80% pure NaOH to neutralize. The mass of sodium chloride or salt that forms is: (masses: Cl 35.5g; H 1.0g; O 16.0g; N 23.0g) Keep in mind the equation: NaOH + HCl -> NaCl + H2O Select one:a. 36.5gB. 80gC. 58.5gD. 117gQ1: calculate the density of solute (10 ml benzene) in liquid mixture if the mole fraction of solvent ( 20 ml carbon tetrachloride and ) 0.342 and the density of solvent (1590 Kg/m) at 30 °C ? Atwt(C=12,Cl=35.5,H=1) g/ mol Q2: When adding( 5 g) of salt to( 0.23 L) of hot water(40 °C) inside the calorimeter, the density of the solution is 2.56 g / ml and the temperature of the solution decreased by( 5 K). Calculate the molecular weight of the salt? Knowing that the calorimeter constant is 2.98 kJ / mol at 20° C, the heat of solubility the solution is (123 J / mol) and ( specific heat of the salt ( 0.774 J/g.°C). Q3 : When nitric acid is added to the water, the temperature of the solution increases, while adding potassium chloride to the water, the temperature of the solution decreases. Why? What is the scientific name for these two cases. Q4: The excess molar volume of liquid mixtures in some solutions appears negative, while in others it appears positive. Why?(D) A sample of gas at 1.08 atm and 25°C has a SO₂ concentration of 1.55 µg/m³ and is in equilibrium with water. The Henry's Law constant for SO2 in water is 2.00 M atm¹ at 25°C. Ideal gas volume = 22.4 dm³ at 1 atm pressure and 0°C. i) Calculate the SO₂ concentration in the sample in ppm. ii) Calculate the SO2 concentration in water at 25°C. (
- I (lec) (CHEM-1305-7Z3), Topic: Unit 6:. w McGraw-Hill Education Campus ork i Saved c. Ex. 6- Molarity - calculate from mole and volume (mL) values (Pool Calculate the molarity, M, of KCl when 2.65 g KCl are dissolved in 2.50 × 10´ mL of solution. Enter your answer in scientific notation. Be sure to answer all parts. x 10 (select) E M KCI < Prev 4 of 11 Next MAR tv1. Given the following mixture of two compounds 45.00 g of X (MW =78.00 g/mol)(density 1.128 g/mL) and 610.00 mL of Y (62.00 g/mol))(density 0.872 g/mL), calculate the mole fraction of X. 2. Given the following mixture of two compounds 25.00 mL of X (MW =87.00 g/mol)(density 1.077 g/mL) and 620.00 mL of Y (90.00 g/mol))(density 1.229 g/mL). The boiling point of pure Y is -3.00 degrees C. The molal boiling constant is 3.276 degrees C/m. What is the boiling point of the solution. 3. Given the following mixture of two compounds 35.00 mL of X (MW =75.00 g/mol)(density 0.879 g/mL) and 765.00 mL of Y (74.00 g/mol))(density 1.161 g/mL). The vapor pressure of pure Y is 24.00. Calculate the vapor pressure of the solution. 4. 3.82 grams of a water soluble ionic compound with the formula of A1X4 (Molar mass of 125.00 grams/mol) is dissolved in 64 grams of water. Calculate the expected boiling point of the solution. The boiling point elevation constant for water is 0.512 degrees C/molal. The…Use the T-xy diagram for mixtures of benzene (Mbenzene-78.11 kg/kmol) and toluene (Mtoluene-92.13 kg/mol) at 1 atm to answer the following question. Temperature (°C) 20 15 10 115 110 105 5 85858KOS 100 95 90 80 75 70 65 Vapor A mixture consisting of 15 moles of 60 mol% benzene and 40 mol% toluene at 90 °C, how much benzene (in moles) would need to be added to make the mixture all vapor? Liquid 0.6 0.8 1.0 0.2 0.4 Mole fraction benzene P = 1 atm