QUESTION 6. Calculate the standard entropy change for the following process at 298 K: 2 P(g) + 5 Cl₂(g) →→→ 2 PCI, (g) The standard entropies are as follows: Sp(g) = 163.2 mol KSC₂(g) = 223.1 mol K and S (g) • Include a negative sign in your answer, if appropriate. • Round your answer to the nearest tenth.. Provide your answer below: = 364.6 mol K

Discuss the spontaneity of each process in the following scenarios, based on the use of the Gibbs free energy equation: 1. N₂(g) + 3H₂(g) + 2NH3(g), AH = -46.11 kJ/mol 2. An exothermic reaction with an increase in entropy 3. A block of solid carbon dioxide subliming to gaseous carbon dioxide

For a chemical reaction that has a ∆Go value of +24 kJ/mol, what value must Q have for this system to be at equilibrium

What is the change in entropy, AS, for the following reaction? Use Table G in your book for values of standard entropies. Your answer should be in J/K mol. CaCO3(s) + 2 H'(aq) → → Ca² (aq) + H₂O(l) + CO2(g) O 264.9 J/K mol O 118.6 J/K mol 394.3 J/K mol 137.7 J/K mol 2

Given the values of AH, ASn, and T, determine ASuniy and predict whether or not each reaction is spontaneous. (Assume that all reactants and products are in their standard states.) a. AH = -95 kJ; AS;n = -157 J/K; T = 298 K b. AH = -95 kJ; AS"n = -157 J/K; T = 855 K Calculate the Gibbs free energy for the above sets (a) and (b)

Calculate ΔS when 25.0 g ethanol at 50.0 °C is added to 75.0 g ethanol at 10.0 °C in an insulated container where Cp = 111.5 J/mol K. Calculate the change in entropy of each ethanol sample, and then the total entropy change. Comment on what is happening to each sample, and overall. (answers: warm = -6.11 J/K; cold = +5.69 J/K; total = 0.42 J/K)

Consider the following reaction: C(graphite) + 1/2 O2 (g) → CO(g) Is it spontaneous under standard conditions at 298 K? Answer this question by calculating AS" (system), AS° (surroundings), and AS (universe). (Define reactants and products as the system.) S* (J/mol · K) A¡H° (kJ/mol) at 298 K (kJ/mol) Compound at 298 K C(s, graphite) 5.6 CO(g) 197.674 -110.525 CS2 (g) 237.8 116.7 CCL (e) 214.39 -128.4 Cl2 (g) 223.08 Si(s) 18.82 SİCL, (g) 330.86 -662.75 S(s, rhombic) 32.1 Br2 (e) 152.2 HBr(g) 198.70 -36.29 H2 (g) 130.7 H2O2 (e) 109.6 -187.78 O2 (g) 205.07 O yes O no

Use the data to calculate the standard entropy change for the following reaction: 5. S°[Mt(s)] 43.2 J/K mol Mt(s) + ½ O2(g) → MtO(s) S°[O2(g)] = 305.1 J/K-mol S°[MtO(s)] 62.6 J/K mol a) -133.2 J/K b) -285.7 J/K c) 285.7 J/K d) 133.2 J/K

Which one of the following choices of gaseous molecules is rank ordered correctly from lowest standard molar entropy (left hand side) to highest standard molar entropy (right hand side)?     He, Ne, CO, SiH4     SiH4 , CO, Ne, He     SiH4 , Ne, CO, He     CO, SiH4 , Ne, He