Concept explainers
(a)
Interpretation:
A flowchart of process along with degree of freedom analysis needs to be prepared and molar amounts of all species in product to be calculated.
Concept introduction:
Flow chart is diagrammatic representation of the reaction taking place in the reactor:
The calculation of flowchart is based on the relation
It helps us to determine the amount of product formed with respect to the amount of reactant fed to the reactor.
Mole fraction
Here,
(b)
Interpretation:
The amount of heat added or removed from the reactor is to be calculated
Concept introduction:
The amount of heat transferred is calculated as follows:
Based on energy conservation
Here,
Enthalpy of reactant and product depends upon the specific heat and the temperature difference.
(c)
Interpretation:
If the process is considered for biodiesel formation, whether biodiesel is economically viable as compared to petroleum diesel or not needs to be determined.
Concept introduction:
Energy transfer equation,
This equation helps to determine the amount of energy generated in product stream with respect to the energy given to the reactor.
(d)
Interpretation:
For atomic species, the degree of freedomneeds to be calculated.
Concept introduction:
Degree of freedom helps to determine the feasibility of reaction and tells about the number of unknowns in a reaction.
The formula for degree of freedom is given as
Degree of freedom = no. of unknown + no. of chemical reaction − no of independent molecular species − no of independent non-reactive molecular species − no. of equation relating unknown
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Chapter 9 Solutions
EBK ELEMENTARY PRINCIPLES OF CHEMICAL P
- (a) The atomic weight of carbon is 12, hydrogen is 1 and oxygen is 16, and the formula for the combustion of methane (CH4) is given by : CH4 + 2 O2 –→ CO2 + 2 H2O + energy A mole of methane releases 810 KJ of energy on burning. Calculate the weight of carbon dioxide produced by burning 5kg of methane. Identify an alternative gas for combustion that produces less carbon dioxide than methane and state how it is generated.arrow_forwardFrom the discussion question from Module 5, recall the chemical equation for the combustion of gasoline (iso-octane, C8H18) is: 2C8H18 + 25O2 ---> 16CO2 + 18H2O This means that 2 moles of iso-octane combine with 25 moles of CO2 to produce 16 moles of CO2 and 18 moles of water. This is important for understanding the impact of fossil fuel use on the atmosphere because burning one mole of fuel adds a lot of CO2. Thinking about this in terms of the stoichiometry, and change in concentration, suppose we had 1.0 mole of iso-octane dissolved in 1.0 m3 of atmosphere. That means the concentration of carbon-containing molecules would be 1 mole per cubic meter. However, ff we burned all that iso-octane and convert the C8H18 into CO2 the concentration of carbon-containing molecules increases. How much does the concentration of carbon-containing molecules increase if 1.0 mole of C8H18 in 1.0 m3 of air is converted into CO2 as shown in the chemical equation above?arrow_forwardSucrose, C12 H22011, is common table sugar. The enthalpy change at 25°C and 1 atm for the complete burning of 2 mol of sucrose in oxygen to give CO2(9) and H2O(1) is - 1.128 x 10* k. From this and from data given below: AH (H2O(1) = -285.8 kJ/mol AH (CO2(9)) = -393.5 kJ/mol AH (O2(9) = 0 kJ/mol Calculate the standard enthalpy of formation of sucrose. AH; =| K/molarrow_forward
- One of the best-selling light, or low-calorie, beers is 4.2%alcohol by volume and a 12-oz serving contains 110 Calories;remember: 1 Calorie = 1000 cal = 1 kcal. To estimatethe percentage of Calories that comes from thealcohol, consider the following questions. (a) Write abalanced chemical equation for the reaction of ethanol,C2H5OH, with oxygen to make carbon dioxide andwater. (b) Use enthalpies of formation in Appendix Cto determine ΔH for this reaction. (c) If 4.2% of the totalvolume is ethanol and the density of ethanol is0.789 g/mL, what mass of ethanol does a 12-oz servingof light beer contain? (d) How many Calories arereleased by the metabolism of ethanol, the reaction frompart (a)? (e) What percentage of the 110 Calories comesfrom the ethanol?arrow_forwardWhich type of flame: a. undergoes complete combustion of fuel (propane) used? Why? Write the reaction involved by predicting the product/s of the reaction. Reaction: CsHe() + O2(g) → b. undergoes incomplete combustion of fuel used? Why? Write the reaction involved. Reaction: C3Heg) + O2(9)· c. Is good for heating/cooking? Why?arrow_forwardThe following reaction using hydrogen and oxygen is carried out in a bomb calorimeter: 2H2(g) + O2(g) → → 2H20(1) The specific heat of the reaction vessel is 0.200 kcal/°C-kg and the specific heat of water is 1.00 kcal/°C-kg. Assuming that m is 0.2 mole of water was formed in the experiment and Q is 3.7 kcal, calculate the heat of the reaction per mole of liquid water.arrow_forward
- Whenever organic matter is decomposed under oxygen-free(anaerobic) conditions, methane is one of the products. Thus,enormous deposits of natural gas, which is almost entirely methane, serve as a major source of fuel for home and industry.(a) Known sources of natural gas can produce 5600 EJ of energy(1 EJ 10^18J). Current total global energy usage is 4.0X10^2 EJper year. Find the mass (in kg) of known sources of natural gas(Hrxnfor the combustion of CH₄=802 kJ/mol).(b) For how many years could these sources supply the world’stotal energy needs?(c) What volume (in ft³) of natural gas, measured at STP, isrequired to heat 1.00 qt of water from 25.0C to 100.0C (d of H₂O= 1.00 g/mL; d of CH₄ at STP =0.72 g/L)?(d) The fission of 1 mol of uranium (about 4X10^4 ft³) in a nu-clear reactor produces 2X10^13 J. What volume (in ft3) of naturalgas would produce the same amount of energy?arrow_forwardComplete combustion of 5.50 g of a hydrocarbon produced 17.7 g of CO, and 6.03 g of H, O. What is the empirical formula for the hydrocarbon? Insert subscripts as necessary. empirical formula: CH SPECIAL ΔΣΩ λμπ (s) (1) (aq) -> (g) () [ ] -> 1. CLR 3,438 19 SA stv W MacBook Airarrow_forwardWrite and balance the reaction for the complete combustion of butane, C4H10.arrow_forward
- Q 8. Premier Periclase in Drogheda produces Magnesium Oxide which can be used in bricks for use in furnaces Write balanced equations to show how the raw material limestone (CaCO3) is converted to the feedstock Hydroxide (Ca(OH)2) The manufacture of MgO is carried out by a continuous process. Give one advantage and one disadvantage of continuous processes in manufacture.arrow_forward||| ANAN Microsoft O V The extraction of aluminum metal from the aluminum hydroxide found in bauxite by the Hall-Héroult process is one of the most remarkable success stories of 19th century chemistry, turning aluminum from a rare and precious metal into the cheap commodity it is today. In the first step, aluminum hydroxide reacts to form alumina (Al₂O3) and water: 2Al(OH)3(s) → Al₂O3(s) + 3H₂O(g) W Microsoft CHEMICAL REACTIONS Reaction sequence stoichiometry Microsoft 6.52.210... esc In the second step, alumina (Al2O3) and carbon react to form aluminum and carbon dioxide: 2Al₂O3(s) + 3C(s) → 4Al(s) + 3 CO₂ (8) Suppose the yield of the first step is 91.% and the yield of the second step is 85.%. Calculate the mass of aluminum hydroxide required to make 6.0 kg of aluminum. Be sure your answer has a unit symbol, if needed, and is rounded to the correct number of significant digits. Explanation Check 9,269 Q x10 HH 103 X OCT 24 ロ・ロ S OOO tv NONZA © 2022 McGraw Hill LLC. All Rights…arrow_forwardHydrogen gas has the potential for use as a clean fuel inreaction with oxygen. The relevant reaction is2 H2(g) + O2(g) ---->2 H2O(l)Consider two possible ways of utilizing this reaction asan electrical energy source: (i) Hydrogen and oxygengases are combusted and used to drive a generator, muchas coal is currently used in the electric power industry;(ii) hydrogen and oxygen gases are used to generate electricitydirectly by using fuel cells that operate at 85 °C.(a) Calculate ΔH° and ΔS° forthe reaction. We will assume that these values do notchange appreciably with temperature. (b) Based on thevalues from part (a), what trend would you expect forthe magnitude of ΔG for the reaction as the temperatureincreases? (c) What is the significance of the change inthe magnitude of ΔG with temperature with respect to the utility of hydrogen as a fuel? (d) Based on the analysishere, would it be more efficient to use the combustionmethod or the fuel-cell method to generate electricalenergy from…arrow_forward
- Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning
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