Concept explainers
(a)
Interpretation:
Calculate the daily rate which octane is used.
Concept introduction:
The
Where, the volume (V) occupied by ‘n’ moles of any gas has a pressure (P) at temperature (T) in Kelvin and ‘R’ = Gas constant
(b)
Interpretation:
Calculate the variation in absolute pressure at the bottom of tank
Concept introduction:
The Ideal Gas Law is defined as,
Where, the volume (V) occupied by ‘n’ moles of any gas has a pressure (P) at temperature (T) in Kelvin and ‘R’ = Gas constant
(c)
Interpretation:
Calculate the amount of octane lost to the atmosphere.
Concept introduction:
The Ideal Gas Law is defined as,
Where, the volume (V) occupied by ‘n’ moles of any gas has a pressure (P) at temperature (T) in Kelvin and ‘R’ = Gas constant
(d)
Interpretation:
Why is nitrogen used in the vapor space instead of air?
Concept introduction:
The Ideal Gas Law is defined as,
Where, the volume (V) occupied by ‘n’ moles of any gas has a pressure (P) at temperature (T) in Kelvin and ‘R’ = Gas constant
(e)
Interpretation:
Suggest a method to recover octane from the gas stream.
Concept introduction:
The Ideal Gas Law is defined as,
Where, the volume (V) occupied by ‘n’ moles of any gas has a pressure (P) at temperature (T) in Kelvin and ‘R’ = Gas constant
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Chapter 6 Solutions
EBK ELEMENTARY PRINCIPLES OF CHEMICAL P
- In the gas phase reaction 2 A(g) + B(g) = 3 C (g) + 2 D (g) it was found that when 1.00 mol A, 2.00 mol B and 1.00 mol D were mixed and allowed to come to equilibrium at 25oC, the resulting mixture contained 0.9 mol C at a total pressure of 1.00 bar. Calculate (a) the mole fractions of each species, (b) KX, (c) KP and (d) △Go . Answer: [0.087 (A); 0.370 (B); 0.196 (C); 0.348 (D); 0.326; 0.325; 2.76 kJ]arrow_forwardThe following reaction is carried out under standard conditions (25°C and 1 bar): 2CH3OH(1) + 302(g) → 2CO2(g) + 4H₂O(1) AH₁° kJ mol-1 Sᵒ J K-¹ mol-1 C6H12O6 (1) -238.4 212.0 O₂ (g) 0.0 205.1 CO₂(g) -393.5 213.7 H₂O (1) -285.8 69.95 Using the data in the table above: a) Calculate the enthalpy of reaction, ArH, for the reaction: kJ mol-¹ b) Calculate the entropy change, AS, for the reaction: 1 c) Calculate AG for the reaction: kJ mol-¹ d) Is the reaction spontaneous? Put any calculations in here: J mol-1arrow_forwardCa(OH)2(aq) + 2HCl(aq) → CaCl2(8) + 2H2O(1) 2. Standar... 1req For the reaction 3. AS surrou... 1req 4. AG° = A... 1req 5. AG: Pre... 1req 6. AG: Enthal... M 7. AG fro... 1req 8. Calculat... 1req 9. Calculat... 1req Question Question Question 10. Calcul... 1req AH° 30.2 kJ and AS° = 206 J/K The equilibrium constant for this reaction at 280.0 K is Assume that AH° and As are independent of temperature. Submit Answer Retry Entire Group 3 more group attempts remainingarrow_forward
- 2 When 50 cm' of hydrochloric acid of concentration 2.0 mol dm is added to 50 cm' of sodium hydroxide solution of concentration 2.0mol dm, the temperature increase is 13.0°C HCl(aq) + NAOH(aq) + NaCl(aq) + H,O(1) The experiment is repeated using 25 cm of the same hydrochloric acid and 50 cm' of the same sodium hydroxide solution. What is the temperature increase? O A 4.9°C I B 6.5°C I C 8.7°C D 13.0°Carrow_forwardA chemical engineer must calculate the maximum safe operating temperature of a high-pressure gas reaction vessel. The vessel is a stainless-steel cylinder that measures 24.0cm wide and 28.8cm high. The maximum safe pressure inside the vessel has been measured to be 8.30MPa. For a certain reaction the vessel may contain up to 1.35kg of boron trifluoride gas. Calculate the maximum safe operating temperature the engineer should recommend for this reaction. Write your answer in degrees Celsius. Round your answer to 3 significant digits.arrow_forward5:27 PM Mon Mar 6 In a 1.0 L container at high temperature, 0.20 mol N₂ and 0.15 mol O₂ are allowed to react. Set up the expression for Qc. Each reaction participant must be represented by one tile. Do not combine terms. Once the expression is constructed, solve for Qc to determine the direction of the reaction. [0] # 3 [0.050] 0.030 E D Predict the equilibrium concentration of O₂ in the reaction described below by constructing an equilibrium expression for Qc, constructing an ICE table, writing an equilibrium expression for Kc, and solving for the equilibrium concentration. Complete Parts 1-4 before submitting your answer. N₂(g) + O₂(g) 2 NO(g) C $ [1.0] 9.0 x 104 4 [0.201² R F Qc = % 5 [0]³ [0.15]¹ 1.1 x 10* V T G 2 Question 4 of 7 6 [1.0]² [0.40]³ ... B Y [0.20] [0.30]¹ & 7 H U N [0.15] [0.050]³ 8 J 4 I [0.40] 9 M 0 K O RESET [0.30] 33 O V L cmd P V { at Su 7 optionarrow_forward
- GMT-7) Example Application of an Energy Balance to a Closed, Unsteady-State System without Reaction Alkaloids are chemical compounds containing nitrogen that can be produced by plant cells. In an experiment, an insulated closed vessel 1.673 m in volume was injected with a dilute water solution containing two alkaloids: ajmalicine and serpentine. The temperature of the solution was 10 C. To obtain an essentially dry residue of alkaloids, all of the water in the vessel was vaporized. Assume that the properties of water can be used in lieu of the properties of the solution. How much heat had to be transferred to the vessel if 1 kg of saturated liquid water initially at 10 C was completely vaporized to a final condition of 100°C and 1 atm T 100°C final H20 Figure E22.1arrow_forwardConsider the following reactions, write the expressions for Kc and Kp and determine their units. Unit for concentration should be mol/dm3 and for pressure kPa. d) Ca3(PO4)2 (s) = 3 Ca²*(aq) + 2 PO4³ (aq) e) 2C2H6(g) + 7O2(g) = 4CO2(g) + 6H2O (g)arrow_forwardIn biological cells that have a plentiful supply of oxygen, glucose is oxidized completely to CO2 and H2O by a process called aerobic oxidation. Muscle cells may be deprived of O2 during vigorous exercise and, in that case, one molecule of glucose is converted to two molecules of lactic acid (CH3CH(OH)COOH) by a process called anaerobic glycolysis. (a) When 0.3212 g of glucose was burned at 298 K in a bomb calorimeter of calorimeter constant 641 J K−1 the temperature rose by 7.793 K. Calculate (i) the standard molar enthalpy of combustion, (ii) the standard internal energy of combustion, and (iii) the standard enthalpy of formation of glucose. (b) What is the biological advantage (in kilojoules per mole of energy released as heat) of complete aerobic oxidation compared with anaerobic glycolysis to lactic acid?arrow_forward
- Excess A(g) is placed in a vacuum vessel with a certain volume at 298 K and pa = 53.33 kPa. A does not react at this temperature. A dissociates as the following reaction when the temperature of system increases to 573 K: A (g) B (g) + C (g) The pressure of system at equilibrium is 186.7 kPa. Calculate A,Gand K of the reaction at 573 K. Assume that the gases are ideal gases.arrow_forwardThe reactionSO2(g) + 2 H2S(g) ⇌ 3 S(s) + 2 H2O(g)is the basis of a suggested method for removal of SO2 frompower-plant stack gases. (a) What is the equilibriumconstant for the reaction at 298 K? (b) In principle,is this reaction a feasible method of removing SO2?(c) If PSO2 = PH2S and the vapor pressure of water is 25 torr,calculate the equilibrium SO2 pressure in the system at298 K. (d) Would you expect the process to be more orless effective at higher temperatures?arrow_forwardAt room temperature when HI (aq) is added to potassium bisulfite, KHSO3(s), sulfur dioxide is formed and the reaction vessel becomes cold. HI (aq) + KHSO3(s)→ SO2(g) + H2O(l) + K+(aq) + I-(aq). Fill in the blank: A.) If the temp of the reaction vessel is increased then Ea,rev will... (decrease, stay the same, increase, or need more info). B.) If the temp of the reaction vessel is increased then Kc will... (decrease, stay the same, increase, or need more info).arrow_forward
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