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Using the Raoult's law standard state, estimate the activity coefficient of CHCl3 in a solution with χ(CHCl3) = 0.8.
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- 1-Pentanol to 1-bromopentane Chemicals: - 60ml Conc. Sulfuric Acid - 100ml Saturated Sodium bicarbonate - 65ml 1-Pentanol - 78g sodium bromide - Distilled water - 58.42g 1-Bromopentane 1-Pentanol Sodium Bromide Sulfuric Acid 1-Bromopentane Formula C5H12O NaBr H2SO4 C5H11Br MW (g/mol) 88.15 102.894 98.078 151.04 Density (g/mL) 0.811 3.21 1.84 1.218 Boiling point (*C) 138 1,396 337 130 NaBr(aq) + H2SO4(aq) -> NaHSO4(aq) + HBr(aq) CH3(CH2)4OH(aq) + H+ Br- (aq) CH3(CH2)4OH2 (aq) + Br-(aq) CH3(CH2)4OH2 (aq) + Br-(aq) CH3(CH2)4Br(aq) + H2O(aq) How do I calculate the percent yield and identify the limiting reagent?Calculate the missing data in the following table. Compound ΔHvap (kJ/mol) ΔSvap [J/(mol·K)] Boiling Point (°C) hexanoic acid 71.1 105.7 hexane 28.9 85.5 69 or 68.73 formic acid 60.7 100.8 1-hexanol 44.5 157.5 The text states that the magnitude of ΔSvap tends to be similar for a wide variety of compounds. Based on the values in the table, do you agree?Extintion coeficient for Y is 1280
- Use the molar DHf° under the formulas to calculate DH°rxn for the equations as balanced: 1. 2B2H6(g) + 3CO2(g) --> 2B2O3(s) + 3CH4(g) ΔH°rxn = _______ kJ ΔH°f = +36 –394 –1274 –75 kJ/mol exo ? endo_thermic 2. 2P2O5 + 2CaC2 -->P4 + 2CaCO3 + 2CO2 ΔH°rxn = _______ kJ ΔH°f = –1505 –59 ___ –1207 –394 kJ/mol exo ? endo_thermic 3. 2Na2CrO4(s) + 10HCl(g) --> 4NaCl(s) + 3Cl2(g) + Cr2O3(s) + 5H2O(l) ΔH°f = –1342 –92 –411 ___ –1140 –286 kJ/mol ΔH°rxn = _______ kJ exo ? endo_thermicThe normal freezing point of n-octane 1C8H182 is -57 °C. In what temperature range is it a nonspontaneous process?A solution of chloroform (CHCl3) and acetone((CH3)2CO) exhibits a negative deviation from Raoult's law.This result implies that:W. chloroform-chloroform and acetone-acetone interactions are stronger than chloroform-acetone interactions.X. chloroform-chloroformand acetone-acetone interactions are weaker than chloroform-acetone interactions.Y. acetone-acetone interactions are stronger than chloroform-chloroform interactions.Z. acetone-acetone interactions are weaker than chloroform-chloroform interactions. only X is true W and Y are true only W is true X and Z are true only Y is true
- In a beaker, I mix 100 ml of 4 M HCl with 100 ml of distilled water. Both fluids are at 25 C initially. (Cp mix = 0.985 cal/g-C) a. What is the Q required if we want to keep the temperature at 25 C? b. What is the T if its adiabatic? c. What is the molarity of the final mixture?A 1-kg iron bar (c=0.11 kcal/kgC) at 100C is placed in 3.0 kg water at 15C. The temperature of the water increases by A. 0.7C B. 3C C. 5C D. 18CGive the solution with proper sig figs. 4.523 g O2 x ( 1 mol O2 / 32.00 g O2) x (– 533.7 kJ/ 3 mol O2) = – 25.14505313 kJ a. – 25.145 kJ b. – 25.14505313 kJ c. – 25 kJ d. – 25.1 kJ e. none of these f. – 25.15 kJ g. – 2 x 10^1 kJ h. – 3 x 10^1 kJ i. – 25.14 kJ
- Consider the following reaction: NH4Cl--->NH3(g)+HCl(g). The vapor pressure after dissasociation of a certain amount of NH4Cl is 608 kPa at 427 Celsius, but rises to 1115 kPa at 459 Celsius. Calclate Keq, deltarGstandard, and deltarHstandard, all at 427 Celsius. Assume that the vapor is an idela gas and that the enthalpy is indepednet of temperature in the range given.During an experiment to determine the value of R a student collected the following data:Molarity of HCl 3.00MVolume of HCl 20.3mlMass of Mg 0.0411gVolume before equalization chamber 43.1mlVolume after equalization chamber 42.7mlBarometric pressure 759.1mmHgTemperature 21.9Calculate the following information and show all work.Moles of Mg reacted ____Moles of H2 formed ____Vapor pressure of water 19.8mmHgPressure of H2 from dalton’s law ____Volume of H2 ____Temperature(k) ____Calculated R value _______Boiling Point Elevation/Freezing Point Depression T = m K where, for freezing point depression: T = T(pure solvent) - T(solution) and for boiling point elevation: T = T(solution) - T(pure solvent) m = (# moles solute / Kg solvent) Kb = boiling point elevation constant. Kf = freezing point depression constant. Kb and Kf depend only on the SOLVENT. Below are some common values. Use these values for the calculations that follow. Solvent Formula Kb(°C / m) Kf(°C / m) Water H2O 0.512 1.86 Ethanol CH3CH2OH 1.22 1.99 Chloroform CHCl3 3.67 Benzene C6H6 2.53 5.12 Diethyl ether CH3CH2OCH2CH3 2.02