Concept explainers
(a)
Interpretation:
To explain if the use of the container at given temperature is safe using the given values in the question and based on Raoult’s Law.
Concept introduction:
Raoult’s Law can be used to find the molecular mass of an unknown solute like in this question we need to find the partial pressure of water.
Antoine equation is an empirical equation
Where A, B, C are the coefficients and T is the temperature.
Mole fraction can be defined as the ratio of one of the components to the total mixture of the substances given by:
(b)
Interpretation:
To explain the assumption regarding no change in liquid composition is reasonable.
Concept introduction:
Raoult’s can be used to find the molecular mass of an unknown solute like in this question we need to find the partial pressure of water.
Let us assume, the vapor to be an ideal gas. So, the pressure is directly proportional to the temperature given by:
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Chapter 6 Solutions
ELEMENTARY PRINCIPLES OF CHEM. PROCESS.
- What is AG for the decomposition of CaCO3 at 298 K and a partial pressure of CO2 of 4.00x10-4 bar? CaCO3(s) → CaO(s) + CO2(g) AGrxn (298 K, Pco2 = 0.400 mbar) = ??? CO2(g) Compound AG°; (kJ mol·1) CACO3(s) СаО(s) -1129 -604 -394arrow_forwardA mixture of isobutylene ((CH3)2CCH2, 0.400 bar partial pressure) and HCI (0.600 bar partial pressure) is heated at 500.0 K. The equilibrium constant K for the gas- phase thermal decomposition of tert- butyl chloride ((CH3)3CCI) is 3.45 at 500.0 K. bar (CH3);CCI(g) = (CH3)2CCH2(g) + HCI(g) 1 3 You have calculated the equilibrium partial pressures to be: 4 C tert-butyl chloride,CH3);CCI = (x) hydrochloric acid, HCI = (0.600 - x) isobutylene, (CH3)2CCH2 = (0.400 - x) What is the partial pressure of tert- butyl chloride ((CH3)3CCI) at equilibrium? 8. 9. +/- х 100arrow_forwardA mixture of isobutylene ((CH3)2CCH2, 0.400 bar partial pressure) and HCI (0.600 bar partial pressure) is heated at 500.0 K. The equilibrium constant K for the gas- phase thermal decomposition of tert- butyl chloride ((CH3)3CCI) is 3.45 at 500.0 K. bar (CH3);CCI(g) = (CH3)2CCH2(g) + HCI(g) 1 3 What is the partial pressure of isobutylene ((CH3)2CCH2) at equilibrium? 4 C 8. 9. +/- х 100arrow_forward
- (A) It is required to separate 1 mole of ethanol from ethanol-water mixture by using distillation Column at standard conditions. After 1 hour, it is found that the volume was double and the pressure increased to 152 kpa. Find the Temperature after 1 hour by using the ideal gas law: PV = nRT Given : R = 0.082 L.atm/mole.K (B) Calculate the capacity of a Base added to a solution contains 10 mole of ammonia (k, = 1.8x105) and 6 mole of ammonium chloride in 120 ml? Note: Atomic weight: H = 1, 0 = 16, C = 12, Ba = 137, Cl= 35 , N=14arrow_forward7. The solubility, C, of sucrose in water, expressed as grams of sucrose per 100 g of solvent, is given as below t/°C C/g 0 179.2 10 20 203.9 190.5 30 219.5 [ΔΗ (a) Draw an appropriate graph to determine the molar enthalpy of solution of sucrose in the temperature range 0 to 40°C. (b) 50mL of saturated solution of benzoic acid at 25°C requires 12.8 mL of 0.05 M NaOH to completely neutralize. What is the solubility of benzoic acid in g/L water at 25°C. so ln,m 40 238.1 = 4.96 kJ/mol, Cbenzoic acid = 1.56g/L]arrow_forwardUse only the first decimal points (X.X) for atomic masses. R = 8.314 L*kPa/mole*K. In a reactor at 350.0 kPA and 95 °C, HCl adds to acetylene by the following reaction:2HCl(g) + C2H2(g) --> C2Cl2H4(g)39.1 g of HCl and 39.1 g of acetylene are placed into the reactor. What is the limiting reagent? What is the final volume of the system?arrow_forward
- Water and acetonitrile, CH3CN, are miscible (can be mixed in any proportions). However, whenwater and acetonitrile are mixed, the volumes are not additive (the total volume of the resultingsolution is not equal to the sum of the pure liquid volumes). For example, when 100.0 mL ofwater and 100.0 mL of CH3CN(l), are mixed at 20 °C, the total volume of the solution is 192.0mL,not 200.0 mL.a. Provide an explanation for this phenomenon.b. Calculate the molarity, molality and mol fraction of CH3CN in a solution preparedby mixing 100.0 mL of water and 100.0 mL of CH3CN(l) at 20 °C. The total volume of themixture is 192.0 mL and the densities of water and acetonitrile are 0.998 g/mL and 0.782g/mL, respectively, at this temperature.c. When 70.0 g H2O and 190.0 g CH3CN(l) are mixed, to resulting solution has adensity of 0.860 g/mL at 20 °C. Calculate the volumes of the pure liquid samples and thesolution, and show that the pure liquid volumes are not additive.arrow_forwardA quantity of methyl acetate is placed in an open, transparent, three-liter flask and boiled long enough to purge all air from the vapor space. The flask is then sealed and allowed to equilibrate at 30°C, at which temperature methyl acetate has a vapor pressure of 269 mm Hg. Visual inspection shows 10 mL of liquid methyl acetate present.(a) What is the pressure in the flask at equilibrium? Explain your reasoning.(b) What is the total mass (grams) of methyl acetate in the flask? What fraction is in the vapor phase atequilibrium?(c) The above answers would be different if the species in the vessel were ethyl acetate because methyl acetate and ethyl acetate have different vapor pressures. Give a rationale for that difference.arrow_forwardA mixture combining 60 mL ethanol (C₂H6O) with 75 mL water (H₂O) is prepared at 280 K. The partial molar volumes of ethanol (E) and water (W) when mixed in these proportions (right column below) and in pure form (left column below) are ethanol water pure substance molar volume 58.2 mL/mol 18.00 mL/mol partial molar volume 55.3 mL/mol 17.7 mL/mol Determine the volume of the ethanol-water mixture. [Hint: You will need to determine the moles of each component.]arrow_forward
- A student investigates the enthalpy of solution, ΔHsoln, for two alkali metal halides, KCl and RbCl. Inaddition to the salts, the students has access to a calorimeter, a balance with a precision of ±0.1 g,and a thermometer with a precision of ±0.1°C.a. To measure ΔHsoln for KCl, the student adds 100.0 g of water initially at 25.0°C to acalorimeter and adds 20.0 g of KCl(s), stirring to dissolve. After the KCl dissolvescompletely, the maximum temperature reached by the solution is 55.4°C. Question : Determine the value of ΔHsoln for KCl in kJ/molrxnarrow_forwardA mixture of isobutylene ((CH3)2CCH2, 0.400 bar partial pressure) and HCI (0.600 bar partial pressure) is heated at 500.0 K. The equilibrium constant K for the gas-phase thermal decomposition of tert-butyl chloride ((CH3)3CCI) is 3.45 at 500.0 K. (CH3);CCI(g) = (CH3),CCH2(g) + HCI(g) Based on your ICE table, set up the expression for K for the decomposition of (CH3);CCI. (CH3);CCI(g) = (CH3)2CCH2(g) + HCI(g) 1 Do not combine or simplify terms. K = 3.45 5 RESET (P(CH);CCH;) (P(CH,);CCH,)? (PHCI) (Рнс) (P(CH,),cCi) (P(CH,),CCI)? 2(Рнс) 2(P(CH3),CCH;) 2(P(CH,),CCI) 2(P(CH,),CCI)? 2(Рнс)? 2(P(CH3),C=CH,)?arrow_forwardA student investigates the enthalpy of solution, ΔHsoln, for two alkali metal halides, KCl and RbCl. Inaddition to the salts, the students has access to a calorimeter, a balance with a precision of ±0.1 g,and a thermometer with a precision of ±0.1°C.a. To measure ΔHsoln for KCl, the student adds 100.0 g of water initially at 25.0°C to acalorimeter and adds 20.0 g of KCl(s), stirring to dissolve. After the KCl dissolvescompletely, the maximum temperature reached by the solution is 55.4°C.i. Calculate the magnitude of the heat absorbed by the solution during the dissolutionprocess, assuming that the specific heat capacity of the solution is 4.18 J/(g*°C).Include units with your answer.arrow_forward
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