Thermodynamics, Statistical Thermodynamics, & Kinetics
3rd Edition
ISBN: 9780321766182
Author: Thomas Engel, Philip Reid
Publisher: Prentice Hall
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Chapter 2, Problem 2.16NP
A 2.25 mole sample of an ideal gas with
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Suppose that attractions are the dominant interaction between gas molecules, and the equation of state is p = nRT/V – n2a/V2.
Determine the work (W(non-ideal gas)) of reversible, isothermal expansion of such a gas from initial volume V (initial) = 20.0 L to final volume V(final) = 40.0 L if n = 2.00 mol, T = 300 K, and a = 3.621 atm-L2/mol2. Watch your units.
Determine the work (W(ideal gas) of reversible, isothermal expansion of an ideal gas from initial volume V (initial) = 20.0 L to final volume V(final) = 40.0 L if n = 2.00 mol and T = 300 K.
Show the difference W(non-ideal) – W(ideal). If all your calculations are done correctly, this result shows you the effect of attractive interaction between gas particles on the work done by the system.
Calculate the change in molar enthalpy DHm when the given gas is heated from 25 oC to 500 oC using the expression above. The constants a, b, and c are available in Table 2B.1.
6E. A 2.25 mole sample of CO,(g), for which C,.m=37.1 J/K at
298 K, expands reversibly and adiabatically from a volume of
4.50 L and a temperature of 298 K to a final volume of 32.5 L.
Calculate the final temperature, q, w, AH and AU for the
process. Assume that the gas behaves ideally and that C.
is
p.m
constant over this temperature interval.
Chapter 2 Solutions
Thermodynamics, Statistical Thermodynamics, & Kinetics
Ch. 2 - Electrical current is passed through a resistor...Ch. 2 - Two ideal gas systems undergo reversible expansion...Ch. 2 - You have a liquid and its gaseous form in...Ch. 2 - Prob. 2.4CPCh. 2 - For a constant pressure process, H=qp. Does it...Ch. 2 - A cup of water at 278 K (the system) is placed in...Ch. 2 - In the experiments shown in Figure 2.4a and 2.4b,...Ch. 2 - What is wrong with the following statement? Burns...Ch. 2 - Why is it incorrect to speak of the heat or work...Ch. 2 - You have a liquid and its gaseous form in...
Ch. 2 - Prob. 2.11CPCh. 2 - Explain how a mass of water in the surroundings...Ch. 2 - A chemical reaction occurs in a constant volume...Ch. 2 - Explain the relationship between the terms exact...Ch. 2 - In the experiment shown in Figure 2.4b, the weight...Ch. 2 - Discuss the following statement: If the...Ch. 2 - Discuss the following statement: Heating an object...Ch. 2 - An ideal gas is expanded reversibly and...Ch. 2 - An ideal gas is expanded reversibly and...Ch. 2 - An ideal gas is expanded adiabatically into a...Ch. 2 - Prob. 2.21CPCh. 2 - Prob. 2.22CPCh. 2 - A student gets up from her chair and pushes a...Ch. 2 - Explain why ethene has a higher value for CV,m at...Ch. 2 - Prob. 2.25CPCh. 2 - Prob. 2.26CPCh. 2 - A 3.75 mole sample of an ideal gas with Cv,m=3R/2...Ch. 2 - The temperature of 1.75 moles of an ideal gas...Ch. 2 - A 2.50 mole sample of an ideal gas, for which...Ch. 2 - A hiker caught in a thunderstorm loses heat when...Ch. 2 - Count Rumford observed that using cannon boring...Ch. 2 - A 1.50 mole sample of an ideal gas at 28.5C...Ch. 2 - Calculate q, w, U, and H if 2.25 mol of an ideal...Ch. 2 - Calculate w for the adiabatic expansion of 2.50...Ch. 2 - Prob. 2.9NPCh. 2 - A muscle fiber contracts by 3.5 cm and in doing so...Ch. 2 - A cylindrical vessel with rigid adiabatic walls is...Ch. 2 - In the reversible adiabatic expansion of 1.75 mol...Ch. 2 - A system consisting of 82.5 g of liquid water at...Ch. 2 - A 1.25 mole sample of an ideal gas is expanded...Ch. 2 - A bottle at 325 K contains an ideal gas at a...Ch. 2 - A 2.25 mole sample of an ideal gas with Cv,m=3R/2...Ch. 2 - Prob. 2.17NPCh. 2 - An ideal gas undergoes an expansion from the...Ch. 2 - An ideal gas described by Ti=275K,Pi=1.10bar, and...Ch. 2 - In an adiabatic compression of one mole of an...Ch. 2 - The heat capacity of solid lead oxide is given by...Ch. 2 - Prob. 2.22NPCh. 2 - Prob. 2.23NPCh. 2 - Prob. 2.24NPCh. 2 - Prob. 2.25NPCh. 2 - A 2.50 mol sample of an ideal gas for which...Ch. 2 - A 2.35 mole sample of an ideal gas, for which...Ch. 2 - Prob. 2.28NPCh. 2 - A nearly flat bicycle tire becomes noticeably...Ch. 2 - Prob. 2.30NPCh. 2 - Prob. 2.31NPCh. 2 - Consider the isothermal expansion of 2.35 mol of...Ch. 2 - An automobile tire contains air at 225103Pa at...Ch. 2 - One mole of an ideal gas is subjected to the...Ch. 2 - Prob. 2.35NPCh. 2 - A pellet of Zn of mass 31.2 g is dropped into a...Ch. 2 - Calculate H and U for the transformation of 2.50...Ch. 2 - A 1.75 mole sample of an ideal gas for which...Ch. 2 - Prob. 2.39NPCh. 2 - Prob. 2.40NPCh. 2 - The Youngs modulus (see Problem P2.40) of muscle...Ch. 2 - DNA can be modeled as an elastic rod that can be...Ch. 2 - Prob. 2.43NPCh. 2 - Prob. 2.44NP
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- Benzoic acid, C6H5COOH, is a common standard used in bomb calorimeters, which maintain a constant volume. If 1.20 g of benzoic acid gives off 31, 723 J of energy when burned in the presence of excess oxygen and in a water bath having a temperature of 24.6 C, calculate q, w, H, and U for the reaction.arrow_forwardThe Dieterici equation of state for one mole of gas is p=RTe-aVRTV-b Where a and b are constants determined experimentally. For NH3g, a = 10.91 atm. L2 and b = 0.0401 L. Plot the pressure of the gas as the volume of 1.00 mol of NH3g expands from 22.4 L to 50.0 L at 273 K, and numerically determine the work done by the gas by measuring the area under the curve.arrow_forwardWhat is the finaltemperature of0.122 mole ofmonatomic ideal gas that performs 75J of work adiabatically if the initial temperature is 235C?arrow_forward
- a) Suppose that attractions are the dominant interaction between gas molecules, and the equation of state is p = nRT/V – n2a/V2. Determine the work (W(non-ideal gas)) of reversible, isothermal expansion of such a gas from initial volume V (initial) = 20.0 L to final volume V(final) = 40.0 L if n = 2.00 mol, T = 300 K, and a = 3.621 atm-L2/mol2. Watch your units. (b) Determine the work (W(ideal gas) of reversible, isothermal expansion of an ideal gas from initial volume V (initial) = 20.0 L to final volume V(final) = 40.0 L if n = 2.00 mol and T = 300 K. (c) Show the difference W(non-ideal) – W(ideal). If all your calculations are done correctly, this result shows you the effect of attractive interaction between gas particles on the work done by the system.arrow_forwardTwo moles of an ideal gas are expanded reversibly and isothermally at 0 °C from 1 atm. Calculate the final volume (in L) occupied by the gas if the heat absorbed during the process is 750 cal.arrow_forwardFive moles of monatomic ideal gas enter the abc cycle and during a complete cycle 600 J of heat is removed from the gas. Process ab is under constant pressure and process bc is increasing at constant volume takes place at pressure. The temperatures of points a and b are Ta= 3°C and Tb= 63°C. What is the work in the ca process?arrow_forward
- Knowing that the molar heat capacity at constant pressure of CO₂ has the form Cp,m = (a + b + c/T²) J mol-¹K-¹, where a= 44.22, b= 8.79 x 10-³ K-¹, and c= -8.62 x 105 K 2,calculate how much heat can absorb 1.5 moles of this gas when the temperature is increased from 25°C to 150°C. NOTE: Give your answer in kJ mol-1arrow_forwardF-2 8. A 3.50 mole sample of an ideal gas with Cv= 3R/2 undergoes reversible expansion. The initial temperature and pressure are T1 = 310 K and P1 = 15.2 bar. The final pressure is P2 = 1.45 bar. Calculate ΔU in kJ for this process. (First calculate T2) Please show all steps.arrow_forwardAssuming ideal gas behavior, calculate ΔH Assuming ideal gas behavior, calculate q Assuming ideal gas behavior, calculate ΔU w =−2.48×104 Jarrow_forward
- How would I calculate work(w), heat(q), energy change(ΔU), enthalpy change(ΔH), and entropy (ΔS) from a sample of 10.0 L of oxygen, originally at 90.18 K and 0.500 atm, is brought to a temperature of 475.0 K and 1.00 atm. Assuming that the oxygen behaves as an ideal gas and that it’s constant pressure heat capacity is given by Cp= 29.96+4.18 x 10^-3 T - 1.75 x 10^5 / T^2arrow_forward1. Real-life heat Capacity is temperature dependent. Consider the formation of water vapor H2(g)+( )O2(g) → H20(g) The heat capacities Cp(T) for each of the reactants and the product is given by Cp-a+bT+CT2 where the constants a, b and c depend on the substance. The above equation is valid from 298 K to 2,000 K. a. The units of a, b and c are . ? b. Calculate AH given (298 K)=-60kCal. Express your answers in terms of a, b, c for the reactants and products (aH2, bH2 --) (Answers choices for part b) дН (T) — — 6оCal O AH (T) = -60kCal + (aH,0 – aĦ, – ļa0.) (T – 298K) + 4 (b#,0 – bH, – įbo.) (T² – 298° K²) – (CH,0 – CH, – țco.) (+ - ) AH (T) = (an,0 – an, – 40,) (T – 298K) + (bn,0 – bn, – bo;) (T² – 298° K²) – (cH,0 – CH, - co,) (- K) Ο ΔΗ (T)ε = -60kCal – (aH,0 – a#, - }a0.) (T – 298K) – | (bH,0 – bH, - bo.) (T² – 298° K²) + (cH,0 – CH, - co.) ( - K)arrow_forwardP3C.5 Use values of standard enthalpies of formation, standard entropies, and standard heat capacities available from tables in the Resource section to calculate the standard enthalpy and entropy changes at 298 K and 398 K for the reaction CO2(g) + H2(g) → CO(g) + H₂O(g). Assume that the heat capacities are constant over the temperature range involved.arrow_forward
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