P5.4 The diagram below shows three paths for 2.75 mol of a monatomic ideal gas between the initial (0.500 bar, 250. K) and final (6.50 bar, 650. K) states. Calculate AS for paths a and c and describe how you could calculate AS for path b. 700 a 600 2 500 400 300 1 3. P (bar) 9.
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- 2.25 moles of an ideal gas with Cv, m = 5R/2 are trans-formed from an initial state T= 680. K and P= 1.15 bar to afinal state I'= 298 K and P= 4.75 bar. Calculate for this pro-cess: AH & AS.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.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.
- Q#3 If the equation of state for a gas is described by the following equation: P.(V- b) =RT, where b=1200 cm3/mol Determine the ∆Ht when 5 moles of this gas go from State 1 (25°C, 10 bar) to State 2 (125°C, 20 bar). Assume CPig /R = 4Calculate the minimum constant Pext required for an isothermal compression of 1.5 mol of a vander Waals gas from 5.00 L to 0.850 L. Then, calculate w, q, and ΔU for the compression. a= 0.245 atm mol-2 L2, b=0.005 L mol-1. T=300K1.4 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.
- A 2.45 mole quantity of methane gas initially at 315K and a pressure of 12.4atm expands to a final pressure of 0.925atm which is also the constant ext pressure. The expansion occurs adiabatically and reversibly. calculate q, w, deltaH and deltaU4. For a certain ideal gas Cp= 8.58 cal/mol-deg. What will be the final volume and temperature when two moles of the gas at 20°C and 15 atm are allowed to expand adiabatically against a constant presure of 5 atm. Find also the W, Q, ∆? and ∆?.2.25 moles of an ideal gas with Cv,m=3R/2 undergoes the following process. The initial state is T=310K and the pressure = 1 atm. The gas is heated to 675K at a constant external pressure of 1 atm. Calculate q, w, delta U, delta H Please help. Thank you so much!!
- Use the data in Table 2.2 to determine Hp T for Ar at 0C and 1atm. Make any reasonable assumptions necessary.What are the following partial derivatives for an ideal gas when P, V, n, and T are variables? a) (მP / მn) V,T b) (მV / მn) P,T c) (მT / მn) P,V(a) An ideal gas undergoes an adiabatic expansion intoa vacuum. Are AS, ASsurrounding and AStotal positive, negative,or zero? Explain your reasoning.(b) 2.25 moles of an ideal gas with Cv, m = 5R/2 are trans-formed from an initial state T= 680. K and P= 1.15 bar to afinal state I'= 298 K and P= 4.75 bar. Calculate for this pro-cess: AH & AS.