Problem 1 When a certain freon used in refrigeration was expanded adiabatically from an initial pressure of 32 atm and 0°C to a final pressure of 1.00 atm, the temperature fell by 22 K. Calculate the Joule- Thomson coefficient, μ, at 0°C, assuming it remains constant over this temperature range.

12) Between 0 °C and 100 °C, the heat capacity of Hg(l) is given by: Cp,m (Hg, l) [units: J mol-1 K-1] = 30.093 – 4.944 x 10-3T Calculate ΔH and ΔS if the temperature of 1.75 moles of Hg(l) is raised from 0.00 °C to 100.00 °C at constant P.

A mixture of He, N2, and Ar has a pressure of 12.4 atm. The partial pressure of He is 461k Pa and the partial pressure of Ar is 233 kPa. Calculate the mole fracticn of N2 O 0.124 O 562 kPa O 555 atm 0.185 O 0,448 How much heat is required to raise the temperature of 1.50 kg of water from 25.0°C to 52.0°C? The specific heat of water is 4.184 Vg"C. O 1500 K QUESTION 14 O 6.27 40.5 k 169 k O 157 K

13) Calculate the AGᵒrxn at 298 K using the following information. 2 H2S(g) + 3 O2(g) → 2 SO2(g) + 2 H₂O(g) - 33.4 -300.1 -228.6 AG°f (kJ/mol) A) -990.6 kJ B) +112.4 kJ C) +66.8 kJ 2A1 (s) + 312 (s) AG°r rxn ? D) -528.7 kJ 14) The standard cell potential for the cell using the overall cell reaction below is +2.20 V: 2A13+ (aq) + 61- (aq) The voltage generated by the cell when [A13+] = 4.5 × 10-3 M and [I-] = 0.15 Mis A) 2.32 B) 2.10 C) 2.39 D) 2.20 E) -495.3 kJ V. E) 2.23

der the following reaction: 2NO2(g) N₂O4 (9) Part A Part B Calculate AG at 298 K if the partial pressures of NO₂ and N₂O4 are 0.36 atm and 1.64 atm, respectively. Express the free energy in kilojoules to two decimal places. |ΨΕΙ ΑΣΦ AG= -6288.99 Submit Previous Answers Request Answer ? Review I Consta kJ X Incorrect; Try Again; 4 attempts remaining This value of free energy is more negative than AG for the reaction (i.e., more spontaneous), but the partial pressure of ta about four times greater than that of the reactant, so the free-energy change is expected to be more positive than AG (i.e spontaneous). Given that AG = AG + RTln Q, calculate the value of Q (it should be greater than 1 for the specified conditions), and free energy from Part A to find the free-energy change at the given partial pressures. Make certain values are expressed in before summing them.

3. Given: CH:(8) = 2C(graphite) + H:(g) AG° = -209 kJ A sample of gaseous C,H; (acetylene, or ethyne) was stored for one year, yet at the end of this period the sample remained unchanged and no graphite or hydrogen gas had been formed. Briefly explain why there is no inconsistency between the sign of AG* and the apparent stability of the sample.

7:52 PM Mon Nov 21 7.) Two blocks of Cu, one mass 100 g and the other mass 150 g, are placed in thermal contact with one another in an adiabatic chamber, such that no heat can escape. If the 100 g piece is initially at 300 K and the 150 g piece is 400 K, then what is the final equilibrium temperature of the system? (note: Cp for Cu = 0.386 J/g K, also the heat lost by one will be gained by the other) q=0 (p= 0.386 g.K T Ti Vi Vf TA -10 c= Cv.m R 100 g 300 K 150g 400K

Mark the correct statements. (Select all that apply.) O [The reaction 2H20(g) → 2H2(g) + O2(g) is expected to have a positive value of ASº.] O [If a sample of pure ozone changed to oxygen at constant T and P, the entropy of the sample would decrease.] O [For the process H20(1) → H20(s) occurring at 0°C and 1 atm, the sign of AS is negative.] O [The value of AS for the process CHC13(1) – CHC13(g) is negative.] O [The reaction CH4(g) + 202(g) → CO2(g) + 2H2O(g) has a negative value of ASsurr-]

Calculate ?G for 1.0 mole of ethanol (d = 0.789 g/cm3) if the pressure is increased isothermally from 94.6 kPa to 202.6 kPa. Molar mass of ethanol is 46.07 g/mol

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 q for each step in the process.