Q1) The heat capacity at constant volume of hydrogen sulfide at low pressures is given by Eq. Ql-1: C[kJ/(mol*C)] = 0.0252 + 1.547 × 10-$T – 3.012 × 10-°T² .. Eq. QI-1 Where, Tis temperature in °C. A quantity of H;S is kept in a piston-fitted cylinder with initial temperature, pressure, and volume equal to 25°C, 2.0 atm, and 3.0 liters, respectively. i- Calculate the heat (kJ) required to raise the gas temperature from 25°C to 1000°C, if the heating takes place at constant volume (i.e., if the piston does not move).
Q1) The heat capacity at constant volume of hydrogen sulfide at low pressures is given by Eq. Ql-1: C[kJ/(mol*C)] = 0.0252 + 1.547 × 10-$T – 3.012 × 10-°T² .. Eq. QI-1 Where, Tis temperature in °C. A quantity of H;S is kept in a piston-fitted cylinder with initial temperature, pressure, and volume equal to 25°C, 2.0 atm, and 3.0 liters, respectively. i- Calculate the heat (kJ) required to raise the gas temperature from 25°C to 1000°C, if the heating takes place at constant volume (i.e., if the piston does not move).
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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![Q1)
The heat capacity at constant volume of hydrogen sulfide at low pressures is given by Eq. Q1-1:
C[kJ/(mol*C)] = 0.0252 + 1.547 × 10-$T – 3.012 × 10-°7²
- Eq. Ql-1
Where, Tis temperature in °C.
A quantity of H;S is kept in a piston-fitted cylinder with initial temperature, pressure, and
volume equal to 25°C, 2.0 atm, and 3.0 liters, respectively.
i- Calculate the heat (kJ) required to raise the gas temperature from 25°C to 1000°C, if the
heating takes place at constant volume (i.e., if the piston does not move).
ii- For a closed system at constant pressure with negligible kinetic and potential energy changes,
the specific heat is determined by Eq. Q1-2:
Cp = C, + 0 008314
Eq. Q1-2
calculate the heat (J) required to raise the gas from 25°C to 1000°C at constant pressure. What
would the piston do during this process?
Given the gas constant = 0 08206 atm. Lit/ (mol. K)](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Ffadbcb41-efad-4e39-a112-3812ff2d5573%2F46819b59-b713-4dd8-a1c7-e7a4a4f415ec%2F4bl3xtu_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Q1)
The heat capacity at constant volume of hydrogen sulfide at low pressures is given by Eq. Q1-1:
C[kJ/(mol*C)] = 0.0252 + 1.547 × 10-$T – 3.012 × 10-°7²
- Eq. Ql-1
Where, Tis temperature in °C.
A quantity of H;S is kept in a piston-fitted cylinder with initial temperature, pressure, and
volume equal to 25°C, 2.0 atm, and 3.0 liters, respectively.
i- Calculate the heat (kJ) required to raise the gas temperature from 25°C to 1000°C, if the
heating takes place at constant volume (i.e., if the piston does not move).
ii- For a closed system at constant pressure with negligible kinetic and potential energy changes,
the specific heat is determined by Eq. Q1-2:
Cp = C, + 0 008314
Eq. Q1-2
calculate the heat (J) required to raise the gas from 25°C to 1000°C at constant pressure. What
would the piston do during this process?
Given the gas constant = 0 08206 atm. Lit/ (mol. K)
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