The change in entropy, ASxn, is related to the the change in the number of moles of gas molecules, Angas. Determine the change in the moles of gas for each of the reactions and decide if the entropy increases, decreases, or has little or no change. А. K(s) + O,(g) KO, (s) The entropy, ASixn Angas = mol decreases. has little or no change. increases. В. CO(g) + 3 H, (g) CH, (g) + H, (g) The entropy, ASixn, Angas = mol decreases. increases. has little or no change. С. S(s) + 0,(g) so, (g) The entropy, ASixn, Angas mol increases. decreases. O has little or no change. D. 2 NH, (g) – N,(g) + 3 H, (g) The entropy, ASxn Angas = mol decreases. has little or no change. increases. O O O ООО O O O

The change in entropy, ASxn, is related to the the change in the number of moles of gas molecules, Angas. Determine the change in the moles of gas for each of the reactions and decide if the entropy increases, decreases, or has little or no change. А. K(s) + O,(g) KO, (s) The entropy, ASixn Angas = mol decreases. has little or no change. increases. В. CO(g) + 3 H, (g) CH, (g) + H, (g) The entropy, ASixn, Angas = mol decreases. increases. has little or no change. С. S(s) + 0,(g) so, (g) The entropy, ASixn, Angas mol increases. decreases. O has little or no change. D. 2 NH, (g) – N,(g) + 3 H, (g) The entropy, ASxn Angas = mol decreases. has little or no change. increases. O O O ООО O O O

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter16: Thermodynamics: Directionality Of Chemical Reactions

Section16.3: Measuring Dispersal Of Energy: Entropy

Problem 16.3CE

See similar textbooks

Similar questions

For ammonia (NH3), the enthalpy of fusion is 5.65 kJ/mol and the entropy of fusion is 28.9 J/K mol. a. Will NH3(s) spontaneously melt at 200. K? b. What is the approximate melting point of ammonia?
Use data from Appendix D to calculate the standardentropy change at 25°C for the reaction CH3COOH(g)+NH3(g)CH3NH2(g)+CO2(g)+H2(g) Suppose that 1.00 mol each of solid acetamide, CH3CONH2(s), and water, H2O(l), react to give thesame products. Will the standard entropy change belarger or smaller than that calculated for the reactionin part (a)?
Calculate the standard Gibbs free-energy change when SO3 forms from SO2 and O2 at 298 K. Why is sulfur trioxide an important substance to study? (Hint: What happens when it combines with water?)
In the thermodynamic definition of a spontaneous process, why is it important that the phrase “continuous intervention” be used rather than just “intervention?”
A key component in many chemical engineering designs is the separation of mixtures of chemicals. (a) What happens to the entropy of the system when a chemical mixture is separated? (b) Are designs for chemical separation more likely to rely on spontaneous or nonspontaneous processes?
The standard molar entropy of iodine vapor, I2(g), is 260.7 J Kl mol-1 and the standard molar enthalpy of formation is 62.4 kJ/mol. a) Calculate the entropy change for vaporization of 1 mol of solid iodine (use data from Table 16.1 or Appendix J). b) Calculate the enthalpy change for sublimation of iodine. c) Assuming that rSdoes not change with temperature, estimate the temperature at which iodine would sublime (change directly from solid to gas).
The evaporation of one mole of water at 298 K has a standard free allergy change of 8.58 kJ. H2O(l)H2O(g)G298=8.58kJ (a) Is the evaporation of water under standard thermodynamic conditions spontaneous?. (b) Determine the equilibrium constant, KP, for this physical process. (c) By calculating G, determine if the evaporation of water at 298 K is spontaneous when the partial pressure of water, PH2O, is 0.011 atm.. (d) If the evaporation of water were always nonspontaneous at room temperature, wet laundry would never dry when placed outside. In order for laundry to dry, what must be the value of PH2O in the air?
For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 atm for all species. For the reaction N2(g)+3H2(g)↽−−⇀2NH3(g) the standard change in Gibbs free energy is Δ?°=−72.6 kJ/mol. What is ΔG for this reaction at 298 K when the partial pressures are ?N2=0.450 atm, ?H2=0.200 atm, and ?NH3=0.800 atm?
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 150.0 °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.
Calculate the standard reaction entropy (∆????∅) at 298 K for the reaction of carbon dioxide with calcium oxide which proceeds according to the following:CaO(?) + CO2(?) → ?aCO3(?)
The change in entropy, ΔSrxn∘, is related to the change in the number of moles of gas molecules, Δngas. Determine the change in the moles of gas for each of the reactions and decide if the entropy increases, decreases, or has little or no change. A. C(s)+H2O(g) ⟶ CO(g)+H2(g) Δ?gas= ? The entropy, ΔSrxn∘, 1) has little or no change 2) increases 3) decreases B. H2O2(l) ⟶ H2(g)+O2(g) Δ?gas=? The entropy, ΔSrxn∘, 1) has little or no change 2) increases 3) decreases C. C2H2(g)+3O2(g) ⟶ 2CO2(g)+2H2O(l) Δ?gas=? The entropy, ΔSrxn∘, 1) has little or no change 2) increases 3) decreases D. PCl5(s) ⟶ PCl3(l)+Cl2(g) Δ?gas=? The entropy, ΔSrxn∘, 1) has little or no change 2) increases 3) decreases
A chemical 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 72.0 °C and constant total pressure. Then, he measures the reaction enthalpy A/ and reaction entropy AS of the first reaction, and the reaction enthalpy A/ 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.