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- 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.A 1.65 mole sample of an ideal gas for which Cv, m = 3/2 R undergoes the following two-step process: (a) From an initial state of the gas described by T = 14.5 oC and P = 2x104 Pa, the gas undergoes isothermal expansion against a constant external pressure of 1.0x104 Pa until the volume has doubled. (b) Then the gas is cooled to constant volume. The temperature drops to -35.6 oC. Calculate q, w, ΔH, ΔU for each step and for the overall process.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 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 K2O1.65 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.5. A sample consisting 3.0 moles of a perfect gas molecules initially at thermal equilibrium with the surroundings 273 K undergoes an irreversible isochoric change to a final temperture of 207 K. Calculate ∆Ssys, ∆Ssurr, and ∆Stotal for the process. Assume Cp,m is 7/2 R throughout the entire temperature range.
- 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.During the industrial synthesis of methanol (CH3OH), carbon monoxide (CO) reactswith hydrogen gas. For methanol, ΔH= -100.4 kJ/mol. a) Is it preferable to maintain this system at high or low pressure? Explain.1.4 g of N2 are placed in a cylinder at an initial volume of 3.8 L and allowed to expand isothermally to a final volume of 10.8 liters against a constant external pressure of 0.8 bar. (A) Treating N2 as a perfect gas, find q, w, ΔU, ΔH, and ΔS for this process. (B) Now assume that the same process occurs, but that N2 can be assumed to have attractive forces between the molecules. In this case, how would q differ from the answer given in (A)? Specifically, would the value be larger, smaller, or unchanged? Explain your answer in 10 words or less. Can you please explain part a and b? <reference> Ne has a mass of 20.18 amu, N2 has a mass of 28.01 amu, H2 has a mass of 1.01 amu, Ar has a mass of 39.95 amu, and He has a mass of 4.00 amu.
- Limestone stalactites and stalagmites are formed in caves by the following reaction:Ca2+(aq)+2HCO−3(aq)→CaCO3(s)+CO2(g)+H2O(l)Ca2+(aq)+2HCO3−(aq)→CaCO3(s)+CO2(g)+H2O(l)If 1 molmol of CaCO3CaCO3 forms at 298 KK under 1 atmatm pressure, the reaction performs 2.47 kJkJ of P−VP−V work, pushing back the atmosphere as the gaseous CO2CO2 forms. At the same time, 38.75 kJkJ of heat is absorbed from the environment. What is the value of ΔHΔH for this reaction? Express your answer using four significant figures.A 1.000 mol sample of ideal gas, initially at 0.9000 atm and 310.0 K, is taken to 1.100 atm and 500 K. Calculate ΔU and ΔH for this process. Use two steps to go from one state to another. Recall H (=U+PV) and U are functions of temperature for ideal gasesCalculate q, ∆H and ∆U for the process during which 2 mol NO2 is heated at a constant pressure of 1 atm and the temperature increases from 25 0C to 50 0C (assume that NO2 is a perfect gas). IF ∆H and ∆U differ for the process, explain this difference.R