Consider a system of neon gas at room temperature (293 K) and atmospheric pressure (1 atm). Assume it behaves entirely as an ideal monatomic gas. (a) Suppose the gas undergoes quasistatic isothermal expansion, from initial volume 1.0L to final volume 1.1 L. What is the amount of heat (Q) that must added to, or removed from, the gas to maintain its constant temperature? (b) described in Part (a)? Based on the Sakur-Tetrode Equation, what is the change in entropy of the gas for the expansion (c) Based your answers to (a) and (b), verify that Q, T, and AS are related as you would have expected. Now consider a mole of neon gas at atmospheric pressure. (d) 150 °C, assuming the neon's molar heat capacity at constant pressure (20.79 J/mol/K) also remains constant with temperature. Calculate the change in entropy of the mole of gas when it is heated from room temperature to (e) For gases, molar heat capacity at constant pressure is often expressed as a function of temperature in the form of the Shomate Equation: C, (T) = A + B · T+ C•T² + D·T³ + E / T? (where A, B, C, D, E are all coefficients that take different values for different gases.) For neon, the A = 20.79 J/mol/K, C= -1.582916 x 1016 J/mol/K³ , D = 1.525102 × 102º J/mol/Kª , coefficients are: B = 4.851 x 1013 J/mol/K?, E = 3.196347×10$J•K/mol Re-calculate the change in entropy of the mole of neon gas when it is heated at atmospheric pressure from room temperature to 150 °C, using the Shomate Equation to take into account the dependence of Cp on temperature. Comparing the result to your answer to (d), was the simplifying assumption in (d) valid?
Consider a system of neon gas at room temperature (293 K) and atmospheric pressure (1 atm). Assume it behaves entirely as an ideal monatomic gas. (a) Suppose the gas undergoes quasistatic isothermal expansion, from initial volume 1.0L to final volume 1.1 L. What is the amount of heat (Q) that must added to, or removed from, the gas to maintain its constant temperature? (b) described in Part (a)? Based on the Sakur-Tetrode Equation, what is the change in entropy of the gas for the expansion (c) Based your answers to (a) and (b), verify that Q, T, and AS are related as you would have expected. Now consider a mole of neon gas at atmospheric pressure. (d) 150 °C, assuming the neon's molar heat capacity at constant pressure (20.79 J/mol/K) also remains constant with temperature. Calculate the change in entropy of the mole of gas when it is heated from room temperature to (e) For gases, molar heat capacity at constant pressure is often expressed as a function of temperature in the form of the Shomate Equation: C, (T) = A + B · T+ C•T² + D·T³ + E / T? (where A, B, C, D, E are all coefficients that take different values for different gases.) For neon, the A = 20.79 J/mol/K, C= -1.582916 x 1016 J/mol/K³ , D = 1.525102 × 102º J/mol/Kª , coefficients are: B = 4.851 x 1013 J/mol/K?, E = 3.196347×10$J•K/mol Re-calculate the change in entropy of the mole of neon gas when it is heated at atmospheric pressure from room temperature to 150 °C, using the Shomate Equation to take into account the dependence of Cp on temperature. Comparing the result to your answer to (d), was the simplifying assumption in (d) valid?
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Transcribed Image Text:Consider a system of neon gas at room temperature (293 K) and atmospheric pressure (1 atm). Assume
it behaves entirely as an ideal monatomic gas.
(a)
Suppose the gas undergoes quasistatic isothermal expansion, from initial volume 1.0L to final
volume 1.1 L. What is the amount of heat (Q) that must added to, or removed from, the gas to maintain
its constant temperature?
(b)
described in Part (a)?
Based on the Sakur-Tetrode Equation, what is the change in entropy of the gas for the expansion
Based your answers to (a) and (b), verify that Q, T, and AS are related as you would have
(c)
expected.
Now consider a mole of neon gas at atmospheric pressure.
(d)
150 °C, assuming the neon's molar heat capacity at constant pressure (20.79 J/mol/K) also remains
Calculate the change in entropy of the mole of gas when it is heated from room temperature to
constant with temperature.
(e)
temperature in the form of the Shomate Equation: C, (T) = A + B · T+ C T² + D· T³ + E / T?
(where A, B, C, D, E are all coefficients that take different values for different gases.) For neon, the
For gases, molar heat capacity at constant pressure is often expressed as a function of
B = 4.851 x 1013 J/mol/K²,
A = 20.79 J/mol/K,
C = -1.582916 x 10°16 J/mol/K³ , D = 1.525102 × 10 20 J/mol/Kª ,
coefficients are:
E = 3.196347×10$J•K/mol
Re-calculate the change in entropy of the mole of neon gas when it is heated at atmospheric pressure
from room temperature to 150 °C, using the Shomate Equation to take into account the dependence of
Cp on temperature. Comparing the result to your answer to (d), was the simplifying assumption in (d)
valid?
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