One mole of an ideal gas undergoes the cycle, A⟶B⟶C⟶A, as shown in the graph. For this gas, CV = 1.5R.  Step C⟶A is isothermal and reversible. 1) Calculate W for each step in the process.

One mole of an ideal gas is contained in a cylinder with a movable piston. The temperature is constant at 78°C. Weights are removed suddenly from the piston to give the following sequence of three pressures. a. P₁ b. P2 c. P3 = 5.20 atm (initial state) = 2.53 atm = 1.00 atm (final state) What is the total work (in joules) in going from the initial to the final state by way of the preceding two steps? J What would be the total work if the process were carried out reversibly? J

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General Chemistry 4th Edition McQuarrie • Rock • Gallogly University Science Books presented by Macmillan Learning Consider an ideal gas enclosed in a 1.00 L container at an internal pressure of 24.0 atm. Calculate the work, w, if the gas expands against a constant external pressure of 1.00 atm to a final volume of 24.0 L. w = J Now calculate the work done if this process is carried out in two steps. 1. First, let the gas expand against a constant external pressure of 1.50 atm to a volume of 16.0 L. 2. From the end point of step 1, let the gas expand to 24.0 L against a constant external pressure of 1.00 atm. w = J

Under what temperature conditions (low T, high T, all T, nonspontaneous at all T) would this reaction occur spontaneously? Explain your reasoning. 2NH4NO3(s) → 2N2(g) + 4H2O(l) + O2 (g)  , ∆Horxn = -236.0 kJ

1. Argon is allowed to expand isothermally (at 298 K) and reversibly from an initial molar volume of 5.0 L/mol to a final molar volume of 11 L/mol. (a) Calculate the work (in units of kJ to 4 sig. figs.) done assuming it behaves as an ideal gas (b) Calculate the work (in units of kJ to 4 sig. figs) assuming it is non-ideal using the van der Waals equation where a = 1.34 atm L2 mol-2 b = 3.20 x 10-2 L mol-1

00 IN L OUniversity Science Book: presented by Macmillan Learning Stry 4th Edition McQuarrie Rock Gallogly Consider an ideal gas enclosed in a 1.00 L container at an internal pressure of 18.0 atm. Calculate the work, w, if the gas expands against a constant external pressure of 1.00 atm to a final volume of 18.0 L. Now calculate the work done if this process is carried out in two steps. 1. First, let the gas expand against a constant external pressure of 1.80 atm to a volume of 10.0 L. 2. From the end point of step 1, let the gas expand to 18.0 L against a constant external pressure of 1.00 atm. = M Question Source: McQuarrie, Rock, And Gallogly 4e - General Chemsitry Publisher. University Science Books MacBook Pro Q Search or enter website name { [ 7. $4 P. 5. 4. U E. K. H. B. gE

A system expands in volume from 2.0 L to 24.5 L at constant temperature. Calculate the work (w) if the expansion occurs against a constant pressure of 5.00 atm.

Calculate ΔE for a system that absorbs 506.0  kJ of heat from its surroundings and does 379.0  kJ of work on its surroundings.