08:41<46...Homework 8-Kinetic theory of Gases.pdfHomework 81. Calculate, in the standard state:(1) What is the average translational kinetic energy of the oxygenmolecules and the hydrogen molecules?(2) How many molecules are there in 1 m³ gas?2. Supposing there is one mole oxygen at 300K, find (1) the translationalkinetic energy; (2) the rotational kinetic energy for the gas. How aboutthe change of the total netic energy when AT-IK?3. What is the change in internal energy as the temperature increases 1K?(1) For 1 mol of monatomic molecules, Imol diatomic molecules and1mol polyatomic molecules respectively. (2) Answer the samequestion for 1g of N₂ and 1g of H₂.85%← 13:00<ا... 46ofHomework 9-Foundamentalsthermodynamics(2).pdfHomework 91. A monatomic ideal gas is contained in a cylinder closed with amovable piston. The initial pressure is 8 atm. and the initial volume is0.5L. The gas is heated first at constant pressure until the volumebecomes to 1.5L, then expands isothermally until the volume isdoubled, finally cooled down at constant volume until the pressuredrops to 1 atm. (1) How much work is done by the gas in the threeprocesses? (2) What is the change in internal energy? (3) How muchheat is supplied to system?2. 2 mol of Helium (assume an ideal gas) expanded adiabatically froman initial state (T; =300K) until the volume is doubled. (1) Calculatethe work done by the gas; (2) What would be the answer if the gas hadexpanded isothermally from the same initial state to the same finalvolume?Pt3. One mole of a monatomic ideal gas iscaused to go through the cycle asshown in the figure. Process be isadiabatic expansion. P-10 atm,V-1.0m³ and V-8.0m³. Find (a)which processes absorb heat fromsurroundings and how much heat isadded in the processes; (b) whichaVprocesses remove heat from systemand the heat amount leaving the gas; (c) the net work done by the gas;(d) the efficiency of the cycle.43%←

Note: We are authorized to answer one question at a time, since you have not mentioned which…

Homework 8 1. Calculate, in the standard state: (1) What is the average translational kinetic energy of the oxygen molecules and the hydrogen molecules? (2) How many molecules are there in 1 m³ gas? 2. Supposing there is one mole oxygen at 300K, find (1) the translational kinetic energy; (2) the rotational kinetic energy for the gas. How about the change of the total kinetic energy when AT=IK? 3. What is the change in internal energy as the temperature increases 1K? (1) For 1 mol of monatomic molecules, 1 mol diatomic molecules and Imol polyatomic molecules respectively. (2) Answer the same question for 1g of N₂ and 1g of H₂.

Homework 8 1. Calculate, in the standard state: (1) What is the average translational kinetic energy of the oxygen molecules and the hydrogen molecules? (2) How many molecules are there in 1 m³ gas? 2. Supposing there is one mole oxygen at 300K, find (1) the translational kinetic energy; (2) the rotational kinetic energy for the gas. How about the change of the total kinetic energy when AT=IK? 3. What is the change in internal energy as the temperature increases 1K? (1) For 1 mol of monatomic molecules, 1 mol diatomic molecules and Imol polyatomic molecules respectively. (2) Answer the same question for 1g of N₂ and 1g of H₂.

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter12: Thermodynamic Processes And Thermochemistry

Section: Chapter Questions

Problem 81AP

See similar textbooks

Similar questions

A process for ethanol synthesis has been developed and the ethylene hydration operating conditions have been optimized in order to reduce production costs (Ayaou et al., 2019). Ethanol is manufactured by reacting ethylene with steam at 150 °C (423.15 K). The reaction takes place in a gas phase and the formation of the ethanol is an exothermic process and assume as ideal gases. ?2?4 (?) + ?2?(?) → ?2?5??(?) Your classmate claims that the equilibrium constant decreases as the temperature decreases. Evaluate the effect of reducing the temperature to 100 °C whether this observation make sense. Support your answer with the necessary calculations. Available information for the calculation are as follows ∆?? ∆?? ∆?? ∆?? ΔHo298 (J/mol) ΔGo298 (J/mol) -1.376 4.157X10-3 -1.610X10-6 -1.210X10+4 -45,792 -8,378
A sample of K(s) of mass 3.226 gg undergoes combustion in a constant volume calorimeter at 298.15 K. The calorimeter constant is 1849 J⋅K−Mol-, and the measured temperature rise in the inner water bath containing 1538 gg of water is 1.776 K. CP,m(H2O,l)=75.3J⋅mol−1⋅K−1CP,m(H2O,l)=75.3J⋅mol−1⋅K−1. 1) Calculate ΔU��f for K2O 2) Calculate ΔH∘f for K2O
4. A sample consisting of 150 g of CO molecules at 300 K is expanded isothermally from an initial pressure of 5.0 bar to a final pressure of 2.0 bar. Calculate q, w, ∆U, ∆H, ∆Ssys, ∆Ssurr, and ∆Stotal for the process two ways: (a) reversibly and (b) irreversibly against a constant pressure of 2.0 bar. Cp,m is constant at a value of 29.14 J/mol* K, and temperature of the surroundings is 273 K. State whether each process is spontaneous.
. A 2.50 mole sample of a perfect gas for which Cv,m = 3R/2 (assume constant over T-range) undergoes the following two-step process: (1) from an initial state of the gas described by T = 13 ºC and P = 1.75 x 105 Pa, the gas undergoes an isothermal expansion against a constant pressure of 3.75 x 104 Pa until the volume has doubled. (2) subsequently, the gas is cooled at constant volume. The temperature falls to -24ºC. Calculate q, w, ∆U, and ∆H for each step and for the overall process.
Heterogeneous chemical reactionConsider the following reaction to form an industrially important solid product B:A (g) ↔ B (s) + C (g) + D (g)a) How many phases are present?b) What is the maximum amount of solid product B you can make for each mole of A fed to the reactorif the reactor is operating at 400 ºC and 1 bar. Data: K = 10.43 at 400 ºC
Consider the following reaction: H2(g) + ½ O2 (g) ------> H2O (g) The standard enthalpy of formation of gaseous H2O at 298 K is -241.82 kJ mol-1. Calculate the value at 153 0C. Given Cp,m for H2O(g): 33.58 kJ mol-1; H2 (g): 28.84 kJ mol-1; O2 (g): 29.37 kJ mol-1. Assume heat capacities are independent of T. NOTE:answer in kilojoules per mole (kJ/mol)
2.30 mol of an ideal gas with CV,m=5R/2 are transformed from an initial state T=750.K and P=1.65bar to a final state T=273K and P=5.25bar Calculate ΔS for this process.
The boiling point of water at p = 1.0 atm is 100°C and its enthalpy of vaporization is delta Hvap = 40.7 kJ mol-1. Calculateq, w and delta Uand delta S for the process in which 2.0mol of water is vaporized at 100°C and p=1.0atm
Please help answer unanswered parts: Calculations 1 and 2 (at bottom, red boxes) Equation used was as follows: C [crystal graphite] + CO2 [gas ] ⇌ 2CO [gas ] ; Formation of carbon monoxide Equation: C [crystal graphite] + CO2 [gas] + <---> 2CO [gas] + + Standard Enthalpy of Formation and Entropy ∆fHo(T) (KJ/mol) So(T) (J/mol.K) C [crystal graphite] 18.51 30.32 CO2 [gas] -343.41 283.87 CO [gas] -78.69 243.42
Calculate △U and △H for the transformation of one mole of a ideal gas from 27°C and 1atm to 327°C and 17atm. Cp=(20.9 + 0.042T) J/Kmol. Provide the given, asked, formula/s to be used and solution.
The feed gas to a methanol synthesis reactor consists of %75 mol H2, %12 mol CO, %8 mol CO2 and %5 mol N2. The system comes to equilibrium at 550 K and 100 bar according to the reactions given in the appendix. Calculate the equilibrium composition of the mixture, assuming the ideal gas and the temperature-independent reaction enthalpy.
1.65 mol of a perfect gas for which Cv,m = 12.47 J K–1 mol–1 is subjected to two successive changes in state: (1) from 37.0 oC and 1.00´105 Pa, the gas is expended isothermally against a constant pressure of 16.5´103 Pa to twice its initial volume. (2) At the end of the previous process, the gas is cooled at constant volume from 37.0 oC to - 23.0 oC. (a) Calculate q , w , DU, DH for each of the stages.