Concept explainers
(a)
Interpretation:
Estimate the volume of HCl.
Concept introduction:
The ideal gas equation can be written as,
Where, P = pressure, V = volume, n = moles, R =
(b)
Interpretation:
Calculate the heat that must be transferred from the absorber.
Concept introduction:
The ideal gas equation can be written as,
Where, P = pressure, V = volume, n = moles, R = ideal gas law and T = temperature
(c)
Interpretation:
Estimate the solution temperature.
Concept introduction:
The ideal gas equation can be written as,
Where, P = pressure, V = volume, n = moles, R = ideal gas law and T = temperature
(d)
Interpretation:
Explain how you use this experimental system to estimate the change of enthalpy for the given case.
Concept introduction:
The ideal gas equation can be written as,
Where, P = pressure, V = volume, n = moles, R = ideal gas law and T = temperature
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ELEMENTARY PRINCIPLES OF CHEM. PROCESS.
- A polymer of large molar mass is dissolved in the organic solvent tetrahydrofuran (C4H8O) at 25 °C, and the resulting solution rises to a final height of 12.7 cm above the level of the pure solvent, as solvent molecules pass through a semipermeable membrane into the solution. If the solution contains 3.61 g polymer per liter, calculate the molar mass of the polymer. Take the density of the solution to be 0.886 g cm³³. g mol-1 Molar mass polymer =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_forwardHenry s law is important in environmental chemistry, where it predicts the distribution of pollutants between water and the atmosphere. The hydrocarbon methylacetylene (C3H4) emitted in wastewater streams, for example, can pass into the air, where it is degraded by processes induced by light from the sun. The Henry s law constant for methylacetylene in water at 25 °C is 601 atm, when the following form of the law is used: = k methylacetylene Calculate the partial pressure of methylacetylene vapor in equilibrium with a solution of 1.47 g of methylacetylene per 1060 L of water. How many methylacetylene molecules are present in each cubic centimeter of vapor? P methylacetylene methylacetylene methylacetylene X = atm molecules per cubic centimeterarrow_forward
- 0.376 grams of KHP are placed in an Erlenmeyer flask and some water and a drop of phenolphthalein is added to the flask. The buret is filled with an NaOH (aq) solution of unknown concentration. The NaOH solution is added dropwise to the flask containing KHP (aq). After 12.78 mLs of the NaOH(aq) solution is added, the color of the solution is found to be faintly pink. What is the concentration (M) of the unknown NaOH solution based on this data alone?arrow_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_forwardMethanol (CH3OH) is produced in the reaction of carbon dioxide and hydrogen via the reaction and process given below: CO2+3H2→CH3OH+H2O The fresh feed to the process contains hydrogen, carbon dioxide, and 0.400 mol% inerts (I). The reactor effluent passes through a condenser that removes essentially all of the methanol and water formed and none of the reactants or inerts. The unreacted reactants and inerts are recycled to the reactor. To avoid buildup of the inerts in the system, a purge stream is withdrawn from the recycle. 100 mol/h of feed to the reactor (not the fresh feed to the process) contains 29.5 mol% CO2, 68.0 mol% H2, and 2.50 mol% inerts. The single-pass conversion of hydrogen is 46.71%. What is the recycle-to-fresh feed ratio?arrow_forward
- 7. 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_forwardA geochemist in the field takes a 9.0 mL sample of water from a rock pool lined with crystals of a certain mineral compound X. He notes the temperature of the pool, 15. C, and caps the sample carefully. Back in the lab, the geochemist first dilutes the sample with distilled water to 400. mL.. Then he filters and evaporates all the water under vacuum. Crystals of X are left behind. The researcher washes, dries and weighs the crystals. They weigh 0.045 g. Using only the information above, can you calculate the solubility of Xin water at 15.° C7 If you said yes, calculate it. Be sure your answer has a unit symbol and 2 significant digits. yes O no 0 0.9 H ロ・ロ X 0 Garrow_forwardA student determined the molar mass of an unknown ionic solid by the method used in this experiment. She found the equilibrium temperature of the ice water mixture (THE FREEZING POINT) to be 0.50°C on her thermometer. When she added 3.10 g of her solid to the mixture, the temperature fell to -4.30°C. She then poured off the solution into a beaker. The mass of the solution was 34.59 g. Kf = 1.86°C/m What was the freezing point depression ∆Tf (celsius) What was the molality of the unknown solution? How much water was in the solution? What did she find to be the observed molar mass of the ionic solid, assuming she made the calculation properly?arrow_forward
- C1. Subject :- CHemistry At 25C, the partial molar volumes of ethanol and water in a mixture 12 per cent by mass ethanol are 54.23 cm^3 mol and 17.93 cm^3 mol'. Calculate the total volume and density of the mixture. M(H20)=18.02 g/mol', M(EtOH)=46.07 g/molarrow_forwardcoompute with full solutionarrow_forwardAt 25 °C the solubility of lead(Il) bromide is 2.70 x 10 mol/L. Calculate the value of Kgp at this temperature. Enter your answer in exponential format using a capital "E (example 1.23E-4) and no units (value 2%).arrow_forward
- Chemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning