(a)
Interpretation:
A labeled flow chart should be drawn taking a basis of 1 mol of heptanes feed.
Concept Introduction
The flow chart will be drawn on the basis of given information of reaction:
(b)
Interpretation:
Taking elemental species [C (s) and H2 (g)] at 25? as references, an inlet-outlet enthalpy table should be prepared and filled in.
Concept introduction:
The standard heat of formation will be helpful to solve the problem as:
(c)
Interpretation:
The required heat transfer to or from the reactor should be obtained in kJ.
Concept introduction:
Heat transferred is determined by the formula:
(d)
Interpretation:
The heat of the heptanes dehydorcyclization reaction should be calculated at 400? and 1atm.
Concept Introduction
The heat of the heptanes dehydorcyclization reaction is determined using the formula:
(e)
Interpretation:
It should be explained that why the calculation is done in part (c) instead of directly looking up the heat of reaction at 400 o C.
Concept Introduction
In this particular case, the heat of reaction at 400°C is the heat required (given to the reactor) for the reaction to be carried out. It is equal to the heat provided for the reactor and can be calculated either the way.
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Chapter 9 Solutions
EBK ELEMENTARY PRINCIPLES OF CHEMICAL P
- Benzoic acid, C6H5COOH, is a common standard used in bomb calorimeters, which maintain a constant volume. If 1.20 g of benzoic acid gives off 31, 723 J of energy when burned in the presence of excess oxygen and in a water bath having a temperature of 24.6 C, calculate q, w, H, and U for the reaction.arrow_forwardWhat are the two ways that a final chemical state of a system can be more probable than its initial state?arrow_forwardExplain why the high-temperature reservoir of a heat engine must, indeed, be higher in temperature than the low-temperature reservoir. Can it ever be the other way around?arrow_forward
- In the 1880s, Frederick Trouton noted that the enthalpy of vaporization of 1 mol pure liquid is approximately 88 times the boiling point, Tb, of the liquid on the Kelvin scale. This relationship is called Troutons rule and is represented by the thermochemical equation liquid gas H = 88 Tb, joules Combined with an empirical formula from chemical analysis, Troutons rule can be used to find the molecular formula of a compound, as illustrated here. A compound that contains only carbon and hydrogen is 85.6% C and 14.4% H. Its enthalpy of vaporization is 389 J/g, and it boils at a temperature of 322 K. (a) What is the empirical formula of this compound? (b) Use Troutons rule to calculate the approximate enthalpy or vaporization or one mole of the compound. Combine the enthalpy of vaporization per mole with that same quantity per gram to obtain an approximate molar mass of the compound. (c) Use the results of parts (a) and (b) to find the molecular formula of this compound. Remember that the molecular mass must be exactly a whole-number multiple of the empirical formula mass, so considerable rounding may be needed.arrow_forwardEsc ||| = OTHERMOCHEMISTRY A student runs two experiments with a constant-volume "bomb" calorimeter containing 1200. g of water (see sketch at right). Calculating heat of reaction from bomb calorimetry data First, a 5.000 g tablet of benzoic acid (C6H,CO₂H) is put into the "bomb" and burned completely in an excess of oxygen. (Benzoic acid is known to have a heat of combustion of 26.454 kJ/g.) The temperature of the water is observed to rise from 16.00 °C to 38.96 °C over a time of 9.2 minutes. 2 4. Next, 5.730 g of acetaldehyde (C₂H₂O) are put into the "bomb" and similarly completely burned in an excess of oxygen. This time the temperature of the water rises from 16.00 °C to 42.19 °C. 84°F Sunny Use this information, and any other information you need from the ALEKS Data resource, to answer the questions below about this reaction: FI Explanation Is this reaction exothermic, endothermic, or neither? 4- F₂ Check 2C₂H4O(g) + 50₂(g) 4CO₂(g) + 4H₂O(g) Be sure any of your answers that are…arrow_forwardFrom the enthalpies of reaction 2C(s) + O2 (9) → 2C0(g) 2C(s) + O2 (9) + 4H2 (g) → 2CH3 OH(g) AH ΔΗ :-221.0kJ %3| :-402.4kJ calculate AH for the reaction CO(g) + 2H2 (g) → CH3 OH(g) Express your answer to three significant figures with the appropriate units.arrow_forward
- What is the molar energy of combustion (in kJ/mol) of C7HO2 when 2.50 g of C7H6O2 burns completely in excess O2 gas at constant pressure, temperature 298 K and releases -30.9 kJ of energy? 2 C7H6O2 + 15 02 - 14 CO2 + 6 H20 1.59 x 105 kJmol-1 1.59 x 10 kJmol-1 O 1.59 x 103 kJmol¯1 1590 kJmol-1arrow_forwardUsing the following data, determine the heat of reaction for the combustion of 1 mol of ethylene, C,H4. CH.(g) + 302(g) → 2CO2(g) + 2H2O(1) Compound СН.(8) CO2(g) H2O(1) +731.4 kJ +1411.1 kJ -1411.1 kJ -1306.5kJ +1306.5kJ AH°: ( kJ/mol) +52.3 -393.5 -285.9 A) B) C) According to the quantum theory, what is the energy contained in a single quantum of orange light with a frequency of 5.00 x 1014 ? (Planck's constant is 6.63 x 10J. s.) A) B) 34 1.25 x 10 J 3.32 x 10 J 1.88 x 10 J 3.13 x 103 J 6.02 x 10 J D) E) 3. Which quantum number describes the orientation in space of an orbital? A) B) C) Dy E) 1 ml any of thesearrow_forwarda) Calculate the enthalpy variation produced in the butane combustion reaction under standard conditions.b) what amount of heat will be released in the complete combustion of the 12kg of butane contained in a cylinder dH standard CO2 (g) = -393kJ / mol, H2O (l) = -286kJ / mol, C4H10 (g) = -125kJ / molarrow_forward
- Given the following heats of formation, calculate the temperature change in 500 g of water starting at 25°C (make note of any phase changes if applicable) if 50 g of ethane is combusted. (hint: heat summation) |C2H6(g) H2O) |-285.5 Substance CO2(g) AH; (kJ / mol) |-393 |-83.6arrow_forwardUsing molar enthalpies of formation, determine the heat of reaction (KJ) for the combustion of 1.0000 mole of methanol. 2CH30H() + 302(g) -› 2C02 (g) + 4H20(1) Heat f° (kJ/mol) CH3OH(1) = -238 7 C02(g) = -393 5 H20(1) = -285.8arrow_forwardGiven the following reactions A (g) +B (g) – 2 C (g) AH = +810.7 kJ 2 C (g) + B (g) → 2 D (g) AH =- 321.1 kJ the enthalpy for the decomposition of D into A and B 2D (g) → A (g) + 2B (g) is kJ. 1131.8 OA. 45.5 В. 489.6 OC. O D.-1131.8 O E. Е. – 489.6arrow_forward
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