7) with thermodynamics, one cannot determine (blank). 8) the value of deltaS for

Question

7) with thermodynamics, one cannot determine (blank).

8) the value of deltaS for the catalytic hydrogenation of acetylene to ethene, C2H2 + H2 --> C2H4, is ?

9) the value of deltaG at 373 K for the oxidation of solid elemental sulfur to gaseous sulfur dioxide, S(s,rhombic) + O2 --> SO2, is ?? (At 298 K, deltaH for this reaction is -269.9 kJ/mol and deltaS is +11.6 J/K).

Reference the above image for all the questions

7) With thermodynamics, one cannot determine 7) A) the value of the equilibrium constant B) the speed of a reaction C) the extent of a reaction D) the direction of a spontaneous reaction E) the temperature at which a reaction will be spontaneous Use the table below to answer the questions that follow. Thermodynamic Quantities for Selected Substances at 298.15 K (25 °C) Substance Hof (kJ/mol) Gf (kJ/mol) S(J/K-mol) Carbon C (s, diamond) 1.88 C (s, graphite)0 C2H2 (g) C2H4 (g) C2H6 (g) CO (g) C02 (g) 2.84 2.43 5.69 200.8 219.4 229.5 197.9 213.6 226.7 209.2 52.30 -84.68 110.5 68.11 -32.89 137.2 394.4 -393.5 Hydrogen H2( g) 130.58 Oxygen 02 (9) H20 () 205.0 285.83 237.13 8) The value of AS"for the catalytic hydrogenation of acetylene to ethene, 8) C2H2 (g) + H2 (g) C2H4 (g) is J/K. mol A) -18.6 B) +18.6 C) +112.0 D) +550.8 E) 112.0 9) The value of G° at 373 K for the oxidation of solid elemental sulfur to gaseous sulfur dioxide, 9) S (s, rhombic) + 02 (g) SO2 (g) is kJ/mol. At 298 K, AH° for this reaction is -269.9 kJ/mol, and AS° is +11.6 J/K. A) +300.4 B) -4,597 C) +4,597 D) -274.2 E) -300.4

Explanation / Answer

7) with thermodynamics, one cannot determine (blank).

Solution :- The speed of reaction cannot be determined by using the thermodynamics

Because speed of reaction can be determined by kinetics and not by thermodynamics.

8) the value of deltaS for the catalytic hydrogenation of acetylene to ethene, C2H2 + H2 --> C2H4, is ?

Solution :-

C2H2 + H2 --> C2H4

Lets calculate the entropy change using the standard entropy values

Delta Srxn = sum of delta S product – sum of delta S reactant

Lets put the values in the formula

Delta S rxn = [1*C2H4]-[(1*C2H2)+(1*H2)]

Delta S rxn = [1*219.4 ] –[(1*200.8)+(1*130.58)]

Delta S rxn = -112 J

Therefore correct answer is option -112 J

9) the value of deltaG at 373 K for the oxidation of solid elemental sulfur to gaseous sulfur dioxide, S(s,rhombic) + O2 --> SO2, is ?? (At 298 K, deltaH for this reaction is -269.9 kJ/mol and deltaS is +11.6 J/K).

Solution :- formula to calculate the delta G is as follows

Delta G= delta H- (T*deltaS)

Lets put the values in the formula

Delta G =-269.9 kJ –(373 K * 0.0116 kJ per K)

              = -274.2 kJ/mol

Therefore correct answer is optin D

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