?(a) An air-conditioning unit cools \(50(ft)^{3}·s^{?1}\) of air at 94(°F) to 68(°F)

For steady flow in a heat exchanger at approximately atmospheric pressure, what is the heat transferred: (a) When 10 mol of \(SO_{2}\) is heated from 200 to 1100°C? (b) When 12 mol of propane is heated from 250 to 1200°C? (c) When 20 kg of methane is heated from 100 to 800°C? (d) When 10 mol of n-butane is heated from 150 to 1150°C? (e) When 1000 kg of air is heated from 25 to 1000°C? (f) When 20 mol of ammonia is heated from 100 to 800°C? (g) When 10 mol of water is heated from 150 to 300°C? (h) When 5 mol of chlorine is heated from 200 to 500°C? (i) When 10 kg of ethylbenzene is heated from 300 to 700°C? Text Transcription: SO_2

For a steady-flow heat exchanger with a feed temperature of 100°C, compute the outlet stream temperature when heat in the amount of \(12 kJ \cdot mol^{?1}\) is added to the following substances. (a) methane, (b) ethane, (c) propane, (d) n-butane, (e) n-hexane, (f) n-octane, (g) propylene, (h) 1-pentene, (i) 1-heptene, (j) 1-octene, (k) acetylene, (l) benzene, (m) ethanol, (n) styrene, (o) formaldehyde, (p) ammonia, (q) carbon monoxide, (r) carbon dioxide, (s) sulfur dioxide, (t) water, (u) nitrogen, (?) hydrogen cyanide Text Transcription: 12 kJ cdot mol^-1

If \(250(ft)^{3}(s)^{?1}\) of air at 122(°F) and approximately atmospheric pressure is preheated for a combustion process to 932(°F), what rate of heat transfer is required? Text Transcription: 250(ft)^3(s)^?1

How much heat is required when 10,000 kg of \(CaCO_{3}\) is heated at atmospheric pressure from 50°C to 880°C? Text Transcription: CaCO_3

If the heat capacity of a substance is correctly represented by an equation of the form, \(C_{P} = A + BT + CT^{2}\) show that the error resulting when \(?C_{P}?_{H}\) is assumed equal to \(C_{P}\) evaluated at the arithmetic mean of the initial and final temperatures is \(C(T_{2} ? T_{1})^{2}/12\). Text Transcription: C_P = A + BT + CT^2 ?C_P?_H C_P C(T_2 ? T_1)^2/12

If the heat capacity of a substance is correctly represented by an equation of the form, \(C_{P} = A + BT + DT^{?2}\) show that the error resulting when \(?C_{P}?_{H}\) is assumed equal to \(C_{P}\) evaluated at the arithmetic mean of the initial and final temperatures is: \( \frac {D}{T_{1}T_{2}} (\frac {T_{1} - T_{2}}{T_{2} + T_{1}})^{2}\) Text Transcription: C_P = A + BT + DT^?2 ?C_P?_H C_P D / T_1T_2 (T_1 - T_2 / T_2 + T_1)^2

Calculate the heat capacity of a gas sample from the following information: The sample comes to equilibrium in a flask at 25°C and 121.3 kPa. A stopcock is opened briefly, allowing the pressure to drop to 101.3 kPa. With the stopcock closed, the flask warms, returning to 25°C, and the pressure is measured as 104.0 kPa. Determine \(C_{P}|) in \(J \cdot mol^{?1} \cdot K^{?1}\) assuming the gas to be ideal and the expansion of the gas remaining in the flask to be reversible and adiabatic. Text Transcription: C_P J cdot mol ^-1 cdot K^-1

A process stream is heated as a gas from 25°C to 250°C at constant P. A quick estimate of the energy requirement is obtained from Eq. (4.3), with \(C_{P}\) taken as constant and equal to its value at 25°C. Is the estimate of Q likely to be low or high? Why? Text Transcription: C_P

(a) For one of the compounds listed in Table B.2 of App. B, evaluate the latent heat of vaporization \(?H_{n}\) by Eq. (4.13). How does this result compare with the value listed in Table B.2? (b) Handbook values for the latent heats of vaporization at 25°C of four compounds are given in the table. For one of these, calculate \(?H_{n}\) using Eq. (4.14), and compare the result with the value given in Table B.2. Text Transcription: ?H_n

Handbook values for the latent heats of vaporization in \(J \cdot g^{?1}\) are given in the table for three pure liquids at 0°C. For one of these substances, calculate: (a) The value of the latent heat at \(T_{n}\) by Eq. (4.14), given the value at 0°C. (b) The value of the latent heat at \(T_{n}\) by Eq. (4.13). By what percentages do these results differ from the value listed in Table B.2 of App. B? Text Transcription: J cdot g^-1 T_n

Table B.2 of App. B provides parameters for an equation that gives \(P^{sat}\) as a function of T for a number of pure compounds. For one of them, determine the heat of vaporization at its normal boiling point by application of Eq. (4.12), the Clapeyron equation. Evaluate \(dP^{sat}/dT\) from the given vapor-pressure equation, and use generalized correlations from Chapter 3 to estimate ?V. Compare the computed value with the value of \(?H_{n}\) listed in Table B.2. Note that normal boiling points are listed in the last column of Table B.2. Text Transcription: P^sat dP^sat / dT ?H_n

A method for determination of the second virial coefficient of a pure gas is based on the Clapeyron equation and measurements of the latent heat of vaporization \(?H^{lv}\), the molar volume of saturated liquid \(V^{l}\), and the vapor pressure \(P^{sat}\). Determine B in \(cm^{3} \cdot mol^{?1}\) for methyl ethyl ketone at 75°C from the following data at this temperature: \(? H^{l?} = 31,600 J \cdot mol^{?1}\) \(V^{l} = 96.49 cm^{3} \cdot mol^{?1}\) \(ln P^{sat} / kPa = 48.158 ? 5623 / T ? 4.705 ln T\) [T = K] Text Transcription: ?H^lv V^l P^sat cm^3 cdot mol^-1 ? H^l? = 31,600 J cdot mol^?1 V^l = 96.49 cm^3 cdot mol^?1 ln P^sat / kPa = 48.158 ? 5623 / T ? 4.705 ln T

One hundred kmol per hour of subcooled liquid at 300 K and 3 bar is superheated to 500 K in a steady-flow heat exchanger. Estimate the exchanger duty (in kW) for one of the following: (a) Methanol, for which \(T^{sat}\) = 368.0 K at 3 bar. (b) Benzene, for which \(T^{sat}\) = 392.3 K at 3 bar. (c) Toluene, for which \(T^{sat}\) = 426.9 K at 3 bar. Text Transcription: T^sat

For each of the following substances, compute the final temperature when heat in the amount of \(60 kJ \cdot mol^{?1}\) is added to the subcooled liquid at 25°C at atmospheric pressure. (a) methanol (b) ethanol (c) benzene (d) toluene (e) water Text Transcription: 60 kJ cdot mol^-1

Saturated-liquid benzene at pressure \(P_{1} = 10 bar ( T_{1}^{sat} = 451.7K )\) is throttled in a steady-flow process to a pressure \(P_{2} = 1.2 bar ( T_{2}^{sat} = 358.7K )\), where it is a liquid/ vapor mixture. Estimate the molar fraction of the exit stream that is vapor. For liquid benzene, \(C_{P} = 162 J \cdot mol^{?1} \cdot K^{?1}\). Ignore the effect of pressure on the enthalpy of liquid benzene. Text Transcription: P_1 = 10 bar ( T_1^sat = 451.7K ) P_2 = 1.2 bar ( T_2^sat = 358.7K ) C_P = 162 J cdot mol^?1 cdot K^?1

Estimate \(? H_{f_{298}}°\) for one of the following compounds as a liquid at 25°C. (a) Acetylene, (b) 1,3-Butadiene, (c) Ethylbenzene, (d) n-Hexane, (e) Styrene. Text Transcription: ? H_f_298°

Reversible compression of 1 mol of an ideal gas in a piston/cylinder device results in a pressure increase from 1 bar to \(P_{2}\) and a temperature increase from 400 K to 950 K. The path followed by the gas during compression is given by \(PV^{1.55}\) = const, and the molar heat capacity of the gas is given by: \(C_{P} / R = 3.85 + 0.57 × 10^{?3} T\) [ T = K ] Determine the heat transferred during the process and the final pressure. Text Transcription: P_2 PV^1.55 C_P/R = 3.85 + 0.57 x 10^-3T

Hydrocarbon fuels can be produced from methanol by reactions such as the following, which yields 1-hexene: \(6CH_{3}OH(g) ? C_{6} H_{12} (g) + 6H_{2}O(g)\) Compare the standard heat of combustion at 25°C of 6 \(CH_{3}OH(g)\) with the standard heat of combustion at 25°C of \(C_{6}H_{12}(g)\) for reaction products \(CO_{2}(g)\) and \(H_{2}O(g)\). Text Transcription: 6CH_3OH(g) ? C_6 H_12 (g) + 6H_2O(g) 6CH_3OH(g) C_6H_12(g) CO_2(g) H_2O(g)

What is the standard heat of combustion of each of the following gases at 25°C if the combustion products are \(H_{2}O(l)\) and \(CO_{2}(g)\)? Compute both the molar and specific heat of combustion in each case. (a) methane, (b) ethane, (c) ethylene, (d) propane, (e) propylene, (f) n-butane, (g) 1-butene, (h) ethylene oxide, (i) acetaldehyde, (j) methanol, (k) ethanol. Text Transcription: H_2O(l) CO_2(g)

Determine the standard heat of each of the following reactions at 25°C:

Compute the standard heat of reaction for each of the following reactions taking place at 298.15 K in dilute aqueous solution at zero ionic strength.

The first step in the metabolism of ethanol is dehydrogenation by reaction with nicotinamide-adenine dinucleotide (NAD): \(C_{2} H_{5} OH + NAD + ? C_{2} H_{4} O + NADH\) What is the heat effect of this reaction upon metabolizing 10 g of ethanol from a typical cocktail? What is the total heat effect for complete metabolism of the 10 g of ethanol to \(CO_{2}\) and water? How, if at all, is the perception of warmth that accompanies ethanol consumption related to these heat effects? For computing heat effects, you may neglect the temperature, pH, and ionic strength dependence of the enthalpy of reaction (i.e. apply the enthalpies of formation from Table C.5 of App. C at physiological conditions). Text Transcription: C_2 H_5 OH + NAD + ? C_2 H_4 O + NADH CO_2

Natural gases are rarely pure methane; they usually also contain other light hydrocarbons and nitrogen. Determine an expression for the standard higher heat of combustion as a function of composition for a natural gas containing methane, ethane, propane, and nitrogen. Assume liquid water as a product of combustion. Which of the following natural gases has the highest heat of combustion? (a) \(y_{C H_{4}} = 0.95, y_{C_{2}H_{6}} = 0.02, y_{C_{3}H_{8} = 0.02, y_{N_{2}} = 0.01\). (b) \(y_{C H_{4}} = 0.90, y_{C_{2}H_{6}} = 0.05, y_{C_{3}H_{8} = 0.03, y_{N_{2}} = 0.02\). (c) \(y_{C H_{4}} = 0.85, y_{C_{2}H_{6}} = 0.07, y_{C_{3}H_{8} = 0.03, y_{N_{2}} = 0.05\). Text Transcription: y_CH_4 = 0.95, y_C_2H_ 6 = 0.02, y_C_3H_ 8 = 0.02, y_N_2 = 0.01 y_CH_4 = 0.90, y_C_2H_ 6 = 0.05, y_C_3H_ 8 = 0.03, y_N_2 = 0.02 y_CH_4 = 0.85, y_C_2H_ 6 = 0.07, y_C_3H_ 8 = 0.03, y_N_2 = 0.05

If the heat of combustion of urea, \((NH_{2})_{2}CO(s)\), at 25°C is 631,660 \(J \cdot mol^{?1}\) when the products are \(CO_{2}(g)\), \(H_{2}O(l)\), and \(N_{2}(g)\), what is \(?H_{f_{298}}°\) for urea? Text Transcription: (NH_2)_2CO(s) J cdot mol^?1 CO_2(g) H_2O(l) N_2(g) ? H_f_298°

The higher heating value (HHV) of a fuel is its standard heat of combustion at 25°C with liquid water as a product; the lower heating value (LHV) is for water vapor as product. (a) Explain the origins of these terms. (b) Determine the HHV and the LHV for natural gas, modeled as pure methane. (c) Determine the HHV and the LHV for a home-heating oil, modeled as pure liquid n-decane. For n-decane as a liquid \(?H_{f_{298}}° = ? 249,700 J \cdot mol^{?1}\). Text Transcription: ?H_f_298° = ? 249,700 J cdot mol^?1

A light fuel oil with an average chemical composition of \(C_{10}H_{18}\) is burned with oxygen in a bomb calorimeter. The heat evolved is measured as 43,960 \(J \cdot g^{?1}\) for the reaction at 25°C. Calculate the standard heat of combustion of the fuel oil at 25°C with \(H_{2}O(g)\) and \(CO_{2}(g)\) as products. Note that the reaction in the bomb occurs at constant volume, produces liquid water as a product, and goes to completion. Text Transcription: C_10H_18 J cdot g^?1 H_2O(g) CO_2(g)

Ethylene gas and steam at 320°C and atmospheric pressure are fed to a reaction process as an equimolar mixture. The process produces ethanol by the reaction: \(C_{2} H_{4} (g) + H_{2} O(g) ? C_{2} H_{5} OH(l)\) The liquid ethanol exits the process at 25°C. What is the heat transfer associated with this overall process per mole of ethanol produced? Text Transcription: C_2H_4 (g) + H_2 O(g) ? C_2 H_5 OH(l)

A gas mixture of methane and steam at atmospheric pressure and 500°C is fed to a reactor, where the following reactions occur: \(CH_{4} + H_{2} O ? CO + 3H_{2}\) and \(CO + H_{2} O ? CO_{2} + H_{2}\) The product stream leaves the reactor at 850°C. Its composition (mole fractions) is: \(y_{CO_{2}} = 0.0275\) \(y_{CO} = 0.1725\) \(y_{H_{2}O} = 0.1725 \(y_{H_{2}} = 0.6275\) Determine the quantity of heat added to the reactor per mole of product gas. Text Transcription: CH_4 + H_2O ? CO + 3 H_2 CO + H_2 O ? CO_2 + H_2 y_CO_2 = 0.0275 y_CO = 0.1725 y_H_2O = 0.1725 y_H_2 = 0.6275

A fuel consisting of 75 mol-% methane and 25 mol-% ethane enters a furnace with 80% excess air at 30°C. If \(8 × 10^{5} kJ \cdot kmol^{?1}\) fuel is transferred as heat to boiler tubes, at what temperature does the flue gas leave the furnace? Assume complete combustion of the fuel. Text Transcription: 8 × 10^5 kJ cdot kmol^?1

The gas stream from a sulfur burner consists of 15 mol-% \(SO_{2}\), 20 mol-% \(O_{2}\), and 65 mol-% \(N_{2}\). The gas stream at atmospheric pressure and 400°C enters a catalytic converter where 86% of the \(SO_{2}\) is further oxidized to \(SO_{3}\). On the basis of 1 mol of gas entering, how much heat must be added to or removed from the converter so that the product gases leave at 500°C? Text Transcription: SO_2 O_2 N_2 SO_3

For steady flow through a heat exchanger at approximately atmospheric pressure, what is the final temperature, (a) When heat in the amount of 800 kJ is added to 10 mol of ethylene initially at 200°C? (b) When heat in the amount of 2500 kJ is added to 15 mol of 1-butene initially at 260°C? (c) When heat in the amount of 106(Btu) is added to 40(lb mol) of ethylene initially at 500(°F)?

Table 9.1 lists the thermodynamic properties of saturated liquid and vapor tetrafluoroethane. Making use of the vapor pressures as a function of temperature and of the saturated-liquid and saturated-vapor volumes, calculate the latent heat of vaporization by Eq. (4.12) at one of the following temperatures and compare the result with the latent heat of vaporization calculated from the enthalpy values given in the table. (a) ?16°C, (b) 0°C, (c) 12°C, (d) 26°C, (e) 40°C.

Calculate the theoretical flame temperature when ethylene at 25°C is burned with: (a) The theoretical amount of air at 25°C. (b) 25% excess air at 25°C. (c) 50% excess air at 25°C. (d) 100% excess air at 25°C. (e) 50% excess air preheated to 500°C. (f) The theoretical amount of pure oxygen.

Determine the standard heat for one of the reactions of Prob. 4.23: part (a) at 600°C, part (b) at 50°C, part (f) at 650°C, part (i) at 700°C, part (j) at 590(°F), part (l) at 770(°F), part (m) at 850 K, part (n) at 1300 K, part (o) at 800°C, part (r) at 450°C, part (t) at 860(°F), part (u) at 750 K, part (v) at 900 K, part (w) at 400°C, part (x) at 375°C, part (y) at 1490(°F).

Develop a general equation for the standard heat of reaction as a function of temperature for one of the reactions given in parts (a), (b), (e), (f), (g), (h), (j), (k), (l), (m), (n), (o), (r), (t), (u), (v), (w), (x), (y), and (z) of Prob. 4.23.

Natural gas (assume pure methane) is delivered to a city via pipeline at a volumetric rate of 150 million standard cubic feet per day. If the selling price of the gas is $5.00 per GJ of higher heating value, what is the expected revenue in dollars per day? Standard conditions are 60(°F) and 1(atm).

Methane gas is burned completely with 30% excess air at approximately atmospheric pressure. Both the methane and the air enter the furnace at 30°C saturated with water vapor, and the flue gases leave the furnace at 1500°C. The flue gases then pass through a heat exchanger from which they emerge at 50°C. Per mole of methane, how much heat is lost from the furnace, and how much heat is transferred in the heat exchanger?

Ammonia gas enters the reactor of a nitric acid plant mixed with 30% more dry air than is required for the complete conversion of the ammonia to nitric oxide and water vapor. If the gases enter the reactor at 75°C, if conversion is 80%, if no side reactions occur, and if the reactor operates adiabatically, what is the temperature of the gases leaving the reactor? Assume ideal gases.

Saturated steam at 1(atm) and 100°C is continuously generated from liquid water at 1(atm) and 25°C by thermal contact with hot air in a counterflow heat exchanger. The air flows steadily at 1(atm). Determine values for m ? (steam)/ n ? (air) for two cases: (a) Air enters the exchanger at 1000°C. (b) Air enters the exchanger at 500°C. For both cases, assume a minimum approach ?T for heat exchange of 10°C.

Saturated water vapor, i.e., steam, is commonly used as a heat source in heat-exchanger applications. Why saturated vapor? Why saturated water vapor? In a plant of any reasonable size, several varieties of saturated steam are commonly available; for example, saturated steam at 4.5, 9, 17, and 33 bar. But the higher the pressure the lower the useful energy content (why?), and the greater the unit cost. Why then is higher-pressure steam used?

Hydrogen is produced by the reaction: \(CO(g) + H_{2} O(g) ? CO_{2} (g) + H_{2} (g)\). The feed stream to the reactor is an equimolar mixture of carbon monoxide and steam, and it enters the reactor at 125°C and atmospheric pressure. If 60% of the \(H_{2}O\) is converted to \(H_{2}\) and if the product stream leaves the reactor at 425°C, how much heat must be transferred to or from the reactor? Text Transcription: CO(g) + H_2 O(g) ? CO_2 (g) + H_2 (g)

A direct-fired dryer burns a fuel oil with a lower heating value of 19,000(Btu) \((lb_{m})^{?1}\). [Products of combustion are \(CO_{2}(g)\) and \(H_{2}O(g)\).] The composition of the oil is 85% carbon, 12% hydrogen, 2% nitrogen, and 1% water by weight. The flue gases leave the dryer at 400(°F), and a partial analysis shows that they contain 3 mol-% \(CO_{2}\) and 11.8 mol-% CO on a dry basis. The fuel, air, and material being dried enter the dryer at 77(°F). If the entering air is saturated with water and if 30% of the net heating value of the oil is allowed for heat losses (including the sensible heat carried out with the dried product), how much water is evaporated in the dryer per \((lb_{m})\) of oil burned? Text Transcription: (lb_m)^?1 CO_2(g) H_2O(g) CO_2 (lb_m)

An equimolar mixture of nitrogen and acetylene enters a steady-flow reactor at 25°C and atmospheric pressure. The only reaction occurring is: \(N_{2} ( g ) + C_{2} H_{2} ( g ) ? 2HCN ( g )\). The product gases leave the reactor at 600°C and contain 24.2 mol-% HCN. How much heat is supplied to the reactor per mole of product gas? Text Transcription: N_2 ( g ) + C_2 H_2 ( g ) ? 2HCN( g )

Chlorine is produced by the reaction: \(4HCl ( g ) + O_{2} ( g ) ? 2 H_{2} O ( g ) + 2 Cl_{2} ( g )\). The feed stream to the reactor consists of 60 mol-% HCl, 36 mol-% O2, and 4 mol-% N2, and it enters the reactor at 550°C. If the conversion of HCl is 75% and if the process is isothermal, how much heat must be transferred to or from the reactor per mole of the entering gas mixture? Text Transcription: 4HCl ( g ) + O_2 ( g ) ? 2 H_2O ( g ) + 2 Cl_2 ( g )

A gas consisting only of CO and \(N_{2}\) is made by passing a mixture of flue gas and air through a bed of incandescent coke (assume pure carbon). The two reactions that occur both go to completion: \(CO_{2} + C ? 2CO and 2C + O_{2} ? 2CO\) The flue gas composition is 12.8 mol-% CO, 3.7 mol-% CO2, 5.4 mol-% \(O_{2}\), and 78.1 mol-% N2. The flue gas/air mixture is so proportioned that the heats of the two reactions cancel, and the temperature of the coke bed is therefore constant. If this temperature is 875°C, if the feed stream is preheated to 875°C, and if the process is adiabatic, what ratio of moles of flue gas to moles of air is required, and what is the composition of the gas produced? Text Transcription: N_2 CO_2 + C ? 2CO and 2C + O_2 ? 2CO O_2

A fuel gas consisting of 94 mol-% methane and 6 mol-% nitrogen is burned with 35% excess air in a continuous water heater. Both fuel gas and air enter dry at 77(°F). Water is heated at a rate of \(75(lb_{m})(s)^{?1}\) from 77(°F) to 203(°F). The flue gases leave the heater at 410(°F). Of the entering methane, 70% burns to carbon dioxide and 30% burns to carbon monoxide. What volumetric flow rate of fuel gas is required if there are no heat losses to the surroundings? Text Transcription: 75(lb_m)(s)^?1

A process for the production of 1,3-butadiene results from the catalytic dehydrogenation at atmospheric pressure of 1-butene according to the reaction: \(C_{4} H_{8} (g) ? C_{4} H_{6} (g) + H_{2} (g)\) To suppress side reactions, the 1-butene feed stream is diluted with steam in the ratio of 10 moles of steam per mole of 1-butene. The reaction is carried out isothermally at 525°C, and at this temperature 33% of the 1-butene is converted to 1,3-butadiene. How much heat is transferred to or from the reactor per mole of entering 1-butene? Text Transcription: C_4 H_8 (g) ? C_4 H_6 (g) + H_2 (g)

(a) An air-cooled condenser transfers heat at a rate of \(12(Btu) \cdot s^{?1}\) to ambient air at 70(°F). If the air temperature is raised 20(°F), what is the required volumetric flow rate of the air? (b) Rework part (a) for a heat-transfer rate of \(12 kJ \cdot s^{?1}\), ambient air at 24°C, and a temperature rise of 13°C. Text Transcription: 12(Btu) cdot s^-1 12 kJ cdot s^-1

(a) An air-conditioning unit cools \(50(ft)^{3}·s^{?1}\) of air at 94(°F) to 68(°F). What is the required heat-transfer rate in \((Btu) \cdot s^{?1}\)? (b) Rework part (a) for a flow rate of \(1.5 m^{3} \cdot s^{?1}\), a temperature change from 35°C to 25°C, and units of \(kJ \cdot s^{?1}\). Text Transcription: 50(ft)^3 cdot s^?1 (Btu) cdot s^?1 1.5 m^3 cdot s^?1 kJ cdot s^?1

A propane-fired water heater delivers 80% of the standard heat of combustion of the propane [at 25°C with \(CO_{2}(g)\) and \(H_{2}O(g)\) as products] to the water. If the price of propane is $2.20 per gallon as measured at 25°C, what is the heating cost in $ per million (Btu)? In $ per MJ? Text Transcription: CO_2 H_2O

Determine the heat transfer \((J \cdot mol^{?1})\) when one of the gases identified below is heated in a steady-flow process from 25°C to 500°C at atmospheric pressure. (a) Acetylene; (b) Ammonia; (c) n-Butane; (d) Carbon dioxide; (e) Carbon monoxide; (f) Ethane; (g) Hydrogen; (h) Hydrogen chloride; (i) Methane; (j) Nitric oxide; (k) Nitrogen; (l) Nitrogen dioxide; (m) Nitrous oxide; (n) Oxygen; (o) Propylene Text Transcription: (J cdot mol^?1)

Determine the final temperature for one of the gases of the preceding problem if heat in the amount of \(30,000 J \cdot mol^{?1}\) is transferred to the gas, initially at 25°C, in a steadyflow process at atmospheric pressure. Text Transcription: 30,000 J cdot mol^?1

Quantitative thermal analysis has been suggested as a technique for monitoring the composition of a binary gas stream. To illustrate the principle, do one of the following problems. (a) A methane/ethane gas mixture is heated from 25°C to 250°C at 1(atm) in a steadyflow process. If \(Q = 11,500 J \cdot mol^{?1}\), what is the composition of the mixture? (b) A benzene/cyclohexane gas mixture is heated from 100°C to 400°C at 1(atm) in a steady-flow process. If \(Q = 54,000 J \cdot mol^{?1}\), what is the composition of the mixture? (c) A toluene/ethylbenzene gas mixture is heated from 150°C to 250°C at 1(atm) in a steady-flow process. If \(Q = 17,500 J \cdot mol^{?1}\), what is the composition of the mixture? Text Transcription: Q = 11,500 J cdot mol^?1 Q = 54,000 J cdot mol^?1 Q = 17,500 J cdot mol^?1

The oxidation of glucose provides the principal source of energy for animal cells. Assume the reactants are glucose \([C_{6}H_{12}O_{6}(s)]\) and oxygen \([O_{2}(g)]\). The products are \(CO_{2}(g)\) and \(H_{2}O(l)\). (a) Write a balanced equation for glucose oxidation, and determine the standard heat of reaction at 298 K. (b) During a day an average person consumes about 150 kJ of energy per kg of body mass. Assuming glucose the sole source of energy, estimate the mass (grams) of glucose required daily to sustain a person of 57 kg. (c) For a population of 275 million persons, what mass of \(CO_{2}\) (a greenhouse gas) is produced daily by mere respiration. Data: For glucose, \(?H_{f_{298}}° = ? 1274.4 kJ \cdot mol ^{?1}\). Ignore the effect of temperature on the heat of reaction. Text Transcription: [C_6H_12O_6(s)] [O_2(g)] CO_2(g) H_2O(l) ?H_f_298° = ? 1274.4 kJ cdot mol^?1

A natural-gas fuel contains 85 mol-% methane, 10 mol-% ethane, and 5 mol-% nitrogen. (a) What is the standard heat of combustion \((kJ \cdot mol^{?1})\) of the fuel at 25°C with \(H_{2}O(g)\) as a product? (b) The fuel is supplied to a furnace with 50% excess air, both entering at 25°C. The products leave at 600°C. If combustion is complete and if no side reactions occur, how much heat (kJ per mol of fuel) is transferred in the furnace? Text Transcription: (kJ cdot mo^l?1) H_2O(g)