Introduction to Chemical Engineering Thermodynamics
8th Edition
ISBN: 9781259696527
Author: J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Publisher: McGraw-Hill Education
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- Consider the following reaction: 10 KNO3(s) +8 C(s) +3 S(s) 2 K2CO3(s) + 3 K,SO,(s) + 6 CO2(g) + 5 N2(g) you mix 0.75 kg of KNO3 with 0.75 kg of sulfur in the presence of excess carbon and the reaction proceeds with 55% yield, what mass of gas-phase products (i.e., CO2 plus N2) will leave the reaction mixture? Show complete work including all calculations, units, appropriate significant figures, and 1-5 key words of explanation at each step of your calculation. Ifarrow_forwardSolubility (g solute/100ml solvent) 90 80 70 60 50 40 30 20 10 0 1Graph 1: Solubility Curves for KCI and KNO3 0 20 40 60 Temperature (°C) 80 Table 1: Solubility data for KCl and KNO3 at 75°C to 35°C? 100 Solubility at 75°C (g/100 g of H₂O) Solubility at 35°C (g/100 g of H₂O) Mass that will precipitate when temperature is reduced from 75°C to 35°C? (g) KCI solubility (gsolute/100g H2O) KNO3 Expon.(KNO3) 1. Use Graph 1 above to answer the following questions and fill in the Table 1. 120 KNO, KCI a) Approximately how many grams of KNO3 will dissolve in 100 g water at 10 °C? b) How many grams of KCI will dissolve in 1 liter of H₂O at 50 °C? c) 500 g of water are used to make a saturated solution of KC at 15 °C. How many more grams of KCI could be dissolved if the temperature were raised to 78 °C? d) A saturated solution of KNO3 in 200 g of H₂O at 51 °C is cooled to 28 °C. How much KNO, will precipitate out of solution?arrow_forward26.20 The data provided in Figure 26.7 are based on the diffusion of O₂ into SiO₂ formed from the oxidation of (100) crystalline silicon at 1000°C. Estimate the diffusion coefficient of O₂ in SiO₂ formed from the oxidation of (111) crystalline silicon at 1000 °C, using the data in the table below, provided by Hess (1990).* Time 1.0 2.0 4.0 7.0 16.0 Measured SiO₂ Film Thickness (um) 0.049 0.078 0.124 0.180 0.298 0.070 0.105 0.154 0.212 0.339 The maximum solubility of O₂ in the SiO₂ is 9.6-10-8 mole 0₂/cm³ solid at 1000°C and 1.0 atm O₂ gas partial pressure. *D.W. Hess, Chem. Eng. Education, 24, 34 (1990).arrow_forward
- As reported in US Patent 4203923, cyclohexanone is an important chemical raw material in the production of nylon intermediates. The separation and purification section for cyclohexanone production usually done through a series of distillation units. Liquid mixture of cyclohexanone (1) and phenol (2) was reported to exist in equilibrium with its vapor at 144 °C (417.15K). The system conforms closely to Modified Raoult’s Law. The mixture forms azeotrope at composition of 0.695. (Refer Table) (a) Provide a sketch that clearly shows that the system exhibits azeotrope(α12)x1=0 = P1sat eA / P2sat and (α12)x1=1 = P1sat / P2sat eA (b) State Paz and sketch a P-xy diagram of the systemarrow_forward1. An impure sample of compound A is contaminated with two impurities B and C. The sample is to be purified by recrystallization using ethanol as the solvent. The solubility properties of the three components are summarized below. Solubility in Solubility in ethanol Solubility in 50 mL Solubility in 50 mL ethanol at -78 °C at - 0°C ethanol at -78 °C ethanol at - 0°C (g) (g) Compound A 0.12 g/mL 0.02 g/mL Impurity B 0.58 g/mL 0.04 g/mL Impurity C 0.005 g/mL 0.0003 g/mL The impure (7.5 g) sample contains 5.0 g of compound A, 1.5 g of B and 1.0 g of C and is recrystallized using 50 mL of ethanol. The sample is boiled with 50 mL of ethanol, filtered by gravity and then cooled in ice and filtered by suction. a) How much compound A should be obtained as the final product? Will the sample be contaminated with any of the impurities? Explain (using calculations to support your answer-fill in the missing masses in the table above). Hint: For this question you should calculate the mass of each…arrow_forwardConsider the following reaction in a sealed vessel kept at constant temperature: A(g) ⇌ 2B(g) If the reaction is started with 2.0 mol of A and no B, the amount of B at equilibrium is 3.0 mol. How many moles of A should one start with to obtain 6.0 mol of B at equilibrium under the same conditions (same vessel, same temperature, no gas B present initially)? A. 5.6 mol B. 5.0 mol C. 4.0 mol D. 6.0 mol E. 6.5 molarrow_forward
- Consider the dissociation of methane to graphite (C) and hydrogen gas. For the methane at 298K, the data available are: k] -74.85- mol = -80.67- mol · K A,GEgraphite = A,G Calculate the equilibrium constant (K) of the dissociation of methane a. at 298 K with the appropriate units. b Assuming that A,H is independent of temperature, calculate the equilibrium constant (K) of methane dissociation at 1000 K. Calculate the ratio between the amounts of methane and hydrogen C. gases at 298 K and 0.2 barg.arrow_forwardThe decomposition of N,0, can be described by the equation 2 N,0,(soln) → 4NO, (soln) + O,(g) Consider the data in the table for the reaction at 45 °C in carbon tetrachloride solution. 1 (s) [N,O3] (M) 2.576 215 2.250 456 1.934 755 1.602 Given the data, calculate the average rate of reaction for each successive time interval. What is the average rate of reaction for the time interval from 0 s to 215 s? average rate of reaction: M/s What is the average rate of reaction for the time interval from 215 s to 456 s? average rate of reaction: M/s What is the average rate of reaction for the time interval from 456 s to 755 s? average rate of reaction: M/sarrow_forwardNaOH (Caustic soda) may be produced in a process from the following reactions: CaCO3 = CaO + CO2 CaO+H2O = Ca(OH)2 2NaCl + CaCO3 = Na2CO3 + CaCl2 Na2CO3+ Ca(OH)2 = 2 NaOH + CaCO3 1. Write the overall reaction for NaOH production using salt (NaCl), limestone (CaCO3) and water (H2O) as raw materials 2. What are the required feed rates of salt (NaCl), limestone (CaCO3) and water (H2O) required to produce 1000 lbm/day of NaOH as a 10% wt solution.arrow_forward
- Table Q4 shows the solubility of liquid trichlorohexane in toluene (also liquid) at equilibrium at different temperatures, where species 1 is trichlorohexane and species 2 is toluene. These data are obtained at 1 atm. X1 0.037 0.050 0.085 0.135 0.199 0.288 0.364 0.482 0.500 0.585 Table Q4 Temperature (°C) 92.18 100.00 107.11 111.96 113.84 112.87 109.63 101.91 100.00 90.05 (a) Plot a properly labeled T-x₁ diagram of this binary mixture at 1 atm. (b) Estimate the composition of each phase at 110°C for this binary mixture. (c) At 110°C and 1 atm, trichlorohexane is added dropwise into an initially pure toluene until the mole fraction of trichlorohexane reaches 0.5. Assuming equilibrium is preserved during every addition of trichlorohexane, describe what you would see if the whole process is conducted in a transparent beaker. (d) At 100°C, determine the A12 and A21 in the two-constant Margules equation. Justify any assumptions that you make.arrow_forwardStandard Gibbs energy of formation, in kJ mol, at 25°C + 124.5 Benzene, C6H6(1) Carbon dioxide, CO2(g) Carbon monoxide, CO(g) - 394.4 – 137.2 Cyclohexane, C6H12(1) + 26.7 Ethanoic acid, CH3COOH (1) - 299.8 - 174.8 Ethanol, C2H$OH(1) Water, H20(1) - 237.1 1. Calculate the standard Gibbs energy change for the following reactions at 25°C: (а) С>H:ОН() + O2(g) > CH-СООН() -+ H2O(1) (b) 2 CO2(g) → 2 CO(g) + O2(g) Which of the above reactions, as written, is spontaneous at the standard state? [- 362.1; +514.4]arrow_forward(a) Consider the following chemical reaction: 3FE203(s) + CO(g) → 2Fe304(s) + CO2(g) AH° = ? Use the following thermochemical data to determine the enthalpy change of this reaction. (6) 2FE2O3 (s) AH° = -1652 kJ 4Fe(s) + 302(g) C(s,graphite) + ½O2(g) → CO(g) 3Fe(s) + 202 (g) → CO2(g) AH° = -110.5 kJ Fe304(s) C(s,graphite) + O2(g) AH° = -1117 kJ AH° = +395.5 kJ (b) What is the standard enthalpy of formation of carbon dioxide? (2)arrow_forward
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