In the manufacture of nitric acid, ammonia and preheated air are mixed to form a gas containing 10.0 mole% NH3 at 600°C. The ammonia is then catalytically oxidized to form NO2 , which is absorbed in water to form HNO3 . If ammonia enters the gas blending unit at 25°C at a rate of 520 kg/h and heat is lost from the mixer to its surroundings at a rate of 7.00 kW, determine the temperature to which the air must be preheated. The constant pressure heat capacities of air and ammonia are given by the equations (in units of J/mol · K): Air: Cp(T)= 28.94+0.004147T Ammonia: Cp(T)= 35.15+0.02954T. Enthalpy is a function of temperature and pressure in general, but it is a stronger function of temperature. For this problem, we will assume that the enthalpy is only a function of temperature (a reasonable assumption under many circumstances). In this case, a change in enthalpy can be calculated as follows: Intensive: •T2 L Cp(T)dT |T1 AH = Extensive: •T2 Cp(T)dT JT1 ΔΗ - = n where T1 and T2 are initial and final temperature, respectively and n is the number of moles. Mass can be used as well, but it is dependent on the units of the heat capacity.
In the manufacture of nitric acid, ammonia and preheated air are mixed to form a gas containing 10.0 mole% NH3 at 600°C. The ammonia is then catalytically oxidized to form NO2 , which is absorbed in water to form HNO3 . If ammonia enters the gas blending unit at 25°C at a rate of 520 kg/h and heat is lost from the mixer to its surroundings at a rate of 7.00 kW, determine the temperature to which the air must be preheated. The constant pressure heat capacities of air and ammonia are given by the equations (in units of J/mol · K): Air: Cp(T)= 28.94+0.004147T Ammonia: Cp(T)= 35.15+0.02954T. Enthalpy is a function of temperature and pressure in general, but it is a stronger function of temperature. For this problem, we will assume that the enthalpy is only a function of temperature (a reasonable assumption under many circumstances). In this case, a change in enthalpy can be calculated as follows: Intensive: •T2 L Cp(T)dT |T1 AH = Extensive: •T2 Cp(T)dT JT1 ΔΗ - = n where T1 and T2 are initial and final temperature, respectively and n is the number of moles. Mass can be used as well, but it is dependent on the units of the heat capacity.
Introduction to Chemical Engineering Thermodynamics
8th Edition
ISBN:9781259696527
Author:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Publisher:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Chapter1: Introduction
Section: Chapter Questions
Problem 1.1P
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![In the manufacture of nitric acid, ammonia and preheated air are mixed to form a gas containing 10.0 mole% \( NH_3 \) at 600°C. The ammonia is then catalytically oxidized to form \( NO_2 \), which is absorbed in water to form \( HNO_3 \). If ammonia enters the gas blending unit at 25°C at a rate of 520 kg/h and heat is lost from the mixer to its surroundings at a rate of 7.00 kW, determine the temperature to which the air must be preheated. The constant pressure heat capacities of air and ammonia are given by the equations (in units of \( J/mol \cdot K \)):
**Air:**
\[ C_p(T) = 28.94 + 0.004147T \]
**Ammonia:**
\[ C_p(T) = 35.15 + 0.02954T \]
Enthalpy is a function of temperature and pressure in general, but it is a stronger function of temperature. For this problem, we will assume that the enthalpy is only a function of temperature (a reasonable assumption under many circumstances). In this case, a change in enthalpy can be calculated as follows:
**Intensive:**
\[ \Delta H = \int_{T_1}^{T_2} C_p(T)dT \]
**Extensive:**
\[ \Delta H = n \int_{T_1}^{T_2} C_p(T)dT \]
where \( T_1 \) and \( T_2 \) are initial and final temperature, respectively and \( n \) is the number of moles. Mass can be used as well, but it is dependent on the units of the heat capacity.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F8dbff956-e43c-48ff-b648-b98fd3ab1747%2Fbe7d5c43-cf4c-4d49-a2b8-9f88c581e993%2Fsf8xg0k_processed.png&w=3840&q=75)
Transcribed Image Text:In the manufacture of nitric acid, ammonia and preheated air are mixed to form a gas containing 10.0 mole% \( NH_3 \) at 600°C. The ammonia is then catalytically oxidized to form \( NO_2 \), which is absorbed in water to form \( HNO_3 \). If ammonia enters the gas blending unit at 25°C at a rate of 520 kg/h and heat is lost from the mixer to its surroundings at a rate of 7.00 kW, determine the temperature to which the air must be preheated. The constant pressure heat capacities of air and ammonia are given by the equations (in units of \( J/mol \cdot K \)):
**Air:**
\[ C_p(T) = 28.94 + 0.004147T \]
**Ammonia:**
\[ C_p(T) = 35.15 + 0.02954T \]
Enthalpy is a function of temperature and pressure in general, but it is a stronger function of temperature. For this problem, we will assume that the enthalpy is only a function of temperature (a reasonable assumption under many circumstances). In this case, a change in enthalpy can be calculated as follows:
**Intensive:**
\[ \Delta H = \int_{T_1}^{T_2} C_p(T)dT \]
**Extensive:**
\[ \Delta H = n \int_{T_1}^{T_2} C_p(T)dT \]
where \( T_1 \) and \( T_2 \) are initial and final temperature, respectively and \( n \) is the number of moles. Mass can be used as well, but it is dependent on the units of the heat capacity.
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