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3. Determine the standard melting point of CCl4 using the following thermodynamic data: Substance AH S°(J/mol...
3. Determine the standard melting point of CCl4 using the following thermodynamic data: Substance AH S°(J/mol K CCl4 (g) CCl4 (1) -106.7 -193.3 309.4 214.4
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3. Determine the standard melting point of CCl4 using the following thermodynamic data: Substance AH S®(J/mol K) CCl4 (g) CCl4 (1) -106.7 -193.3 309.4 214.4
1. In the metallurgy of antimony, the pure metal is recovered from the sulfide ore by the following reaction: SbS(s) + 3Fe (s) 2 Sb(s) + 3FeS () AH-125 kJ Calculate AS un for this reaction at 25°C and 1 atm. 2. Predict the sign of AS., for each of the following reactions. Write "positive" or "negative". a. PCI (8) PCI (1) + Cl2 (g) b. CH. (g) +20, (g) CO2 (g) + 2 H20 (1) c. Mg(s) + Cl2...
Use the thermodynamic data provided below to estimate the boiling point (in K) of CCl4. Report your answer to zero decimal places in standard notation (i.e. 123. kJ *For numbers ending in zero, be sure to include the decimal!*). Substance ΔH°f (kJ/mol) S° (J mol-1K-1) CCl4 (l) -128.4 214.4 CCl4 (g) -96 309.6
Given the following table of thermodynamic data, substance S° C2H2 (g) 200.8 J/mol −K C2H4 (g) 219.4 C2H6 (g) 229.5 H2 (g) 130.58 determine the D S° (in J/mol −K) for the reaction: C2H2 (g) + H2 (g) ® C2H4 (g) −111.98 −101.88 −232.46 +111.98 +101.88
Consider the data in the table. Compound Melting point (°C) AHfus (kJ/mol) Boiling point (°C) AH ap (kJ/mol) HF -83.11 4.577 19.54 25.18 НСІ -114.3 1.991 -84.9 17.53 HBr - 86.96 2.406 -67.0 19.27 HI -50.91 2.871 -35.38 21.16 Using the data in the table, calculate ASfus and ASvap for HI. ASfus = J/(K.mol) AS vap = J/(K · mol) Determine the entropy change when 6.50 mol HI(1) boils at atmospheric pressure. AS = J/K
Additional Thermodynamic Data AH AG: Substance (25°C kJ/mol) (25°C kJ/mol (25°C J/mol-K) CH3NO(1) -112.6 -14.6 171.8 CH3NO, (g) -74.3 -6.8 275.0 SO2 (s) -454.5 -374.2 70.7 soz (1) -441.0 -373.8 Soz (g) -395.7 256.8 113.8 Compute Pvap for nitromethane at 15°C and 70°C. Pvap at 15°C = 0.5368 Pvap at 75°C = 9.22
Consider the data in the table. Compound Melting point (°C) AH (kJ/mol) Boiling point (°C) AHap (kJ/mol HF -83.11 4.577 19.54 25.18 HCI -114.3 1.991 -84.9 17.53 HBr -86.96 -67.0 19.27 HI -50.91 -50.91 2.871 -35.38 21.16 Using the data in the table, calculate ASfus and AS vap for HI. 2.406 A Stus = 24.1 J/(K mol) ASvap = J/(K.mol) Determine the entropy change when 7.50 mol HI(1) freezes at atmospheric pressure. AS = J/K Question Source: MRG - General...
Given the following table of thermodynamic data: Substance S° /J mol−1K−1 X(g) 150.1 Y(g) 194 Z(g) 128 Calculate the ΔS° (in J mol −1K −1) for the reaction: X(g) + 3 Y(g) → 2 Z(g)
Calculate the equilibrium constant from the standard free energy change. Using standard thermodynamic data (linked), calculate the equilibrium constant at 298.15 K for the following reaction 2502(g) + O2(0) 2503(9) AH°F (kJ/mol) AGⓇ, (kJ/mol sº (/mol K) 205.1 Oxygen 02(0) (9) O3(9) 249.2 231.7 161.1 142.7 163.2 238.9 AH°: (kJ/mol Agºr (kJ/mol) 5° (J/mol K) 31.8 0.3 0.3 278.8 3 3.0 167.8 33.0 - 15.0 Sulfur S(s, rhombic) S(s, monodinic) S(g) Sz"(aq) Sg(9) SzCl2(g) SF6(9) H2S(9) soz(9) SO3(0) 1 0....