(a)
Interpretation:
The rate
Concept introduction:
The energy balance is the first law of
(b)
Interpretation:
The volumetric flowrate of the steam produced by using steam tables needs to be determined.
Concept introduction:
The volumetric flowrate
(c)
Interpretation:
The volumetric flowrate by assuming the ideal gas behaviour needs to be determined and compared with volumetric flowrate calculated using steam tables.
Concept introduction:
The ideal gas equation is given as follows;
The molar mass of water is 18 g/mol thus,
(d)
Interpretation:
The effect on the 35% of the thermal energy released due to the combustion process that does not produces steam needs to be explained.
Concept introduction:
Thermal energy is defined as energy coming from heat. The heat is produced due to the movement of tiny particles in an object. Amount of geat generated depends on the speed of the particles.
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- A sample of solid benzoic acid (C,H;COOH) that weighs 800 g is burned in an excess of oxygen to CO,(g) and H,O(€) in a constant-volume calorimeter at 25°C. The temperature increase is observed to be 2.15°C. The heat capacity of the calorimeter and its contents is known to be 9382 J K-1. (a) Write and balance the equation for the combustion of benzoic acid. (b) Calculate the standard change in internal energy (AU°) for the combustion of 1.000 mol benzoic acid to CO2(g) and H,O(€) at 25°C. lc) Calculate the standard enthalpy change (AH°) for the same reaction as in part (b). (d) Calculate the standard enthalpy of formation per mole of benzoic acid, using data for the standard enthalpies of formation of CO2(g) and H,O(() from Appendix D.arrow_forwardThe specific heat of compound AB(s) was determined using coffee-cup calorimeter. When 1.750 g of AB(s) was mixed with 15.00 mL deionized distilled water at room temperature, only 0.850 grams of the compound was dissolved. The temperature of the heterogenous mixture was decreased by 1.70K.Prior to this, the calorimeter was calibrated using a 15mL aqueous reaction mixture that initially contains 0.070 moles each of HBr and KOH. The recorded ΔT is +5.75K. Note: H+(aq) + OH -(aq) → H2O(l) ΔH = -55.85 kJ/molAB(s) ⇌ A+(aq) + B-(aq) ΔH = 88.75 kJ/molspecific heat (H2O) = 4.184 J/g°CMM of AB = 65 g/mol What is the specific heat of solid AB compound (in J/g°C)?arrow_forwardWhen the oxide of generic metal M is heated at 25.0 C, a negligible amount of M is produced. MO,(s) = M(s) + 0,(g) AG = 291.0 mol When this reaction is coupled to the conversion of graphite to carbon dioxide, it becomes spontancous. What is the chemical equation of this coupled process? Show that the reaction is in equilibrium. Include physical states and represent graphite as C(s). chemical equation: What is the thermodynamic equilbrium constant for the coupled reaction? K =arrow_forward
- Construct enthalpy cycles; use Hess's law and the following data to calculate the enthalpy of formation of ethane (from carbon and hydrogen gas). Cis) + Ozig) + CO2(g) AHa = -394kJmol H2g) + %02(a) – H20 m AH°. = -286kJmol1 + 3%O2(g) → 2002(9) + 3H20 m AH = -1560kJmol1arrow_forwardA gas in the initial state of p1 = 75 psia and V1 = 5 ft.3 undergoes a process to p2 = 25 psia and V2 = 9.68 ft., during which the enthalpy decreases 62 BTU. The %3D specific heat at constant volume is c, = 0.754 BTU/lb.°R. Determine (a) the change of internal energy, (b) the specific heat at constant pressure, (c) the gas constant R.°arrow_forwardIn a generic chemical reaction involving reactants and B and products C and D, aA + bB cC + dD, the standard enthalpy AHin of the reaction is given by AHixn = CAH; (C) + dAH; (D) —aAH (A) – bAH (B) Notice that the stoichiometric coefficients, a, b, c, d, are an important part of this equation. This formula is often generalized as follows, where the first sum on the right-hand side of the equation is a sum over the products and the second sum is over the reactants: where m and n represent the appropriate stoichiometric coefficients for each substance. Part A What is AHxn for the following chemical reaction? CS2(g) + 2H₂O(1)→CO2(g) + 2H₂S(g) You can use the following table of standard heats of formation (AH) to calculate the enthalpy of the given reaction. ■ μÅ Value AHrxn=products H - Σreactants mΔΗ Element/ Compound H(g) H₂(g) H₂O(1) CS2 (g) C(g) C(s) Units ? Standard Heat of Formation (kJ/mol) Express the standard enthalpy of reaction to three significant figures and include the…arrow_forward
- Nitroglycerin (C3H5N3O9), a liquid at room temperature (25 oC) and atmospheric pressure (1.01325 x 105 Pa) is used to relieve angina. It may undergo decomposition under these same conditions to form nitrogen, carbon dioxide, oxygen and water, with an enthalpy of decomposition of -1541 kJ mol-1.The standard enthalpies of formation of water and carbon dioxide are -285.9 kJ mol-1 and -393.5 kJ mol-1 respectively. Determine the standard enthalpy of formation of 1.0 mole of nitroglycerin.arrow_forwardCarbon dioxide from the atmosphere "weathers," or dissolves, limestone (CaCO3) by the reaction CACO3(8) + CO2(9) + H2O(1) → Ca²+ (aq) + 2HCO3¯(aq) Obtain AH° for this reaction using the following data: AH;(CaCO3(8)) = –1206.9 kJ/mol AH;(CO2(9)) = -393.5 kJ/mol AH;(H2O(1)) = –285.8 kJ/mol AH;(Ca²+ (ag) -542.8 kJ/mol AH;(HCO3¯(aq)) = -692.0 kJ/mol ΔΗ kJ %3Darrow_forwardA bomb calorimeter was calibrated by burning 0.610g benzoic acid. The temperature of calorimeter was found to increase by 0.178°C. the standard enthalpy of combustion of benzoic acid is known to be -3230kJmol' and the relative molecular mass of benzoic acid is 122. Calculate the heat capacity, C of the calorimeter. (c)arrow_forward
- Ethane is flamed off in abundance from oil wells, because it is unreactive and difficult to use commercially, but would it make a good fuel? The standard enthalpy of reaction for 2 C2H6(g) + 7 O2(g) → 4 CO2(g) + 6 H2O(1) is-3120 kJ mol-1. (a) What is the standard enthalpy of combustion of ethane? (b) What is the specific enthalpy of combustion of ethane? (c) Is ethane a more or less efficient fuel than methane?arrow_forwardThe enthalpy of combustion and the standard enthalpy of formation of a fuel can be determined by measuring the temperature change in a calorimeter when a weighed amount of the fuel is burned in oxygen. (a) Write a balanced chemical equation for the combus- tion of isooctane, C3H18(€), to CO2(g) and H2O(€). Isooctane is a component of gasoline and is used as a reference standard in determining the “octane rating" of a fuel mixture. (b) Suppose 0.542 g isooctane is placed in a fixed-volume (bomb) calorimeter, which contains 750 g water, ini- tially at 20.450°C, surrounding the reaction compart- ment. The heat capacity of the calorimeter itself (excluding the water) has been measured to be 48 J K-1 in a separate calibration. After the combustion of the isooctane is complete, the water temperature is mea- sured to be 28.670°C. Taking the specific he: to be 4.184 J K-1g¬!, calculate AU for the combustion of 0.542 g isooctane. (c) Calculate AU for the combustion of 1 mol isooctane. (d)…arrow_forwardThe standard enthalpy change of combustion [to CO,(g) and H,O(€)] at 25°C of the organic liquid cyclohexane, CH10(€), is –3731.7 kJ mol-1. Determine the AH of CH10(€).arrow_forward
- Physical ChemistryChemistryISBN:9781133958437Author:Ball, David W. (david Warren), BAER, TomasPublisher:Wadsworth Cengage Learning,