Using the following formula, calculate the entropy of a system that has 42 microstates. S = k In W; k = 1.38 x 10-23 J/K (report answer to 3 sig figs; answer format: 3.33 x 10^-33)

0/5 Nerbs A chemical engineer is studying the two reactions shown in the table below. In each case, she fills a reaction vessel with some mixture of the reactants and products at a constant temperature of 85.0 °C and constant total pressure. Then, she measures the reaction enthalpy AH and reaction entropy AS of the first reaction, and the reaction enthalpy AH and reaction free energy AG of the second reaction. The results of her measurements are shown in the table. Complete the table. That is, calculate AG for the first reaction and AS for the second. (Round your answer to zero decimal places.) Then, decide whether, under the conditions the engineer has set up, the reaction is spontaneous, the reverse reaction is spontaneous, or neither forward nor reverse reaction is spontaneous because the system is at equilibrium. do AH = -2220. kJ J AS = -6189 K C,H, (g) + 50, (g) 3Co, (g) + 4H,0(1) AG = KJ Which is spontaneous? O this reaction O the reverse reaction O neither AH = -50. kJ 0- AS =…

Suppose we redefine the standard state as P=3 bar. Find the new standard AG values of the following substances. ▾ Part A ▾ HCI(g) AC 96.3 kJ mol 1 Submit ✓ Correct Part B Previous Answers N₂O (9) Express your answer using four significant figures. IVD ΑΣΦ ΔεG = |105.1 Submit Previous Answers Request Answer Part C X Incorrect; Try Again; 4 attempts remaining Review your calculations and make sure you round to 4 significant figures in the last step. H(g) Express your answer using four significant figures. AC 204.7 kJ mol-1 ? Submil Previous Answers kJ mol 1 ✓ Correct Correct answer is shown. Your answer 201.9 kJ mol was either rounded differently or used a different number of significant figures than required for this part. Review | Constants | Periodic Table

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M Preq 3 Consider the reaction 00 E D 4HCI(g) + O₂(g) 2H₂O(g) + 2Cl₂(8) for which AH° = -114.4 kJ and AS° = -128.9 J/K at 298.15 K. J/K (1) Calculate the entropy change of the UNIVERSE when 1.775 moles of HCI(g) react under standard conditions at 298.15 K. ASuniverse (2) Is this reaction reactant or product favored under standard conditions? Submit Answer (3) If the reaction is product favored, is it enthalpy favored, entropy favored, or favored by both enthalpy and entropy? If the reaction is reactant favored choose 'reactant favored'. 4 000 000 R F DO LO V % 5 [Review Topics] [References] Use the References to access important values if needed for this question. T Retry Entire Group 8 more group attempts remaining Cengage Learning Cengage Technical Support G 6 B Y H & 7 N U 1 * 8 J M 9 K बैं O < L P Previous Email Instructor Save and Exit { + 11 Next ? } ]

A chemicai engineer is studying the two reactions shown in the table below. In each case, he fills a reaction vessel with some mixture of the reactants and products at a constant temperature of 42.0 °C and constant total pressure. Then, he measures the reaction enthalpy AH and reaction entropy AS of the first reaction, and the reaction enthalpy AH and reaction free energy AG of the second reaction. The results of his measurements are shown in the table. Complete the table. That is, calculate AG for the first reaction and AS for the second. (Round your answer to zero decimal places.) Then, decide whether, under the conditions the engineer has set up, the reaction is spontaneous, the reverse reaction is spontaneous, or neither forward nor reverse reaction is spontaneous because the system is at equilibrium. ΔΗ Ξ - 70. kJ J AS = -151. K TiCl, (g) + 2H,0(g) → Tio, (s) + 4H Cl (g) AG = || kJ Which is spontaneous? this reaction the reverse reaction neither AH = 439. kJ AS = K 4H,PO, (s) →…

O-234 kJ 234 kJ -150. kJ -117 kJ Given: -1835kJ AH°, AHᵒf (kJ/mol) -941 -840 QUESTION 12 Use the standard reaction enthalpies given below to determine AH°rxn for the following reaction: P4(g) + 10 Cl₂(g) → 4 PC|5(s) PC15(s) → PC13(g) + Cl₂(g) P4(g) + 6 Cl₂(g) → 4 PCl3(g) rxn IF7(g) IF 5(9) 2(g) 62.42 = ? ΔΗ° rxn AH°rxn = +157 kJ = -1207 KJ QUESTION 13 Use the AH°f and AH°rxn information provided to calculate AH°f for IF: IF7(9) + 12(g) → IF5(g) + 2 IF(g) AH°rxn = -89 kJ

Which statement best aligns with one of the three laws of thermodynamics? O AG--T(AS+AS) O AG-AU-PAV-TAS O AG-TAS O AG-T(AS-AS)

Enthalpy and Gibb's Free Energy Chemical energy is released or absorbed from reactions in various forms. The most easily measurable form of energy comes in the form of heat, or enthalpy. The enthalpy of a reaction can be calculated from the heats of formation of the substances involved in the reaction: AHxn = AH₂ (products) - AH (reactants) Entropy change, AS°, is a measure of the number of energetically equivalent microstates introduced into the system during the reaction. The degree of spontaneity of a reaction is represented by the Gibbs free energy, AGO. The Gibbs free energy depends on both the enthalpy and entropy changes that take place during the reaction: AG=AH° - TAS° where T is standard temperature, 298 K. ▼ Part A Calculate the standard enthalpy change for the reaction where the heats of formation are given in the following table: ΔΗ Substance (kJ/mol) A B C D -241 -407 191 -501 Express your answer in kilojoules. ► View Available Hint(s) {—| ΑΣΦ AHixn= 2A+B=2C+2D ? kJ…