For which of the following reactions is AS° > 0. Choose all that apply. CH4(g) + H₂O(g) → 3H₂(g) + CO(g) 2NO(g) + 2H₂(g) → N₂(g) + 2H₂O(l) 2NO(g) + O₂(g) → 2NO₂(g) 2CO₂(g) + N₂(g) → 2CO(g) + 2NO(g) ONH₂HS(s)→ NH3(g) + H₂S(g)

A student dissolves 10.9 g of ammonium chloride (NH,Cl) in 200. g of water in a well-insulated open cup. She then observes the temperature of the water fall from 20.0 °C to 16.1 °C over the course of 3.8 minutes. Use this data, and any information you need from the ALEKS Data resource, to answer the questions below about this reaction: NH,CI (s) → NH (aq) + Cl¯(aq) You can make any reasonable assumptions about the physical properties of the solution. Be sure answers you calculate using measured data are rounded to the correct number of significant digits. Note for advanced students: it's possible the student did not do the experiment carefully, and the values you calculate may not be the same as the known and published values for this reaction. Ar exothermic Is this reaction exothermic, endothermic, or neither? endothermic neither If you said the rea heat that was released or absorbed by the reaction in this case. I kJ ion was exothermic or endothermic, calculate the amount of kJ…

A student dissolves 11.8 g of sodium hydroxide (NaOH)in 250. g of water in a well-insulated open cup. She then observes the temperature of the water rise from 20.0 °C to 33.6 °C over the course of 8 minutes. Use this data, and any information you need from the ALEKS Data resource, to answer the questions below about this reaction: NaOH(s) Na (aq) + OH (ag) You can make any reasonable assumptions about the physical properties of the solution. Be sure answers you calculate using measured data are rounded to the correct number of significant digits. Note for advanced students: it's possible the student did not do the experiment carefully, and the values you calculate may not be the same as the known and published values for this reaction. Is this reaction exothermic, endothermic, or neither? If you said the reaction was exothermic or endothermic, calculate the amount of heat that was released or absorbed by the reaction in this case. Calculate the reaction enthalpy AH per mole of NaOH. O…

Which one of the following reactions cannot proceed spontaneously as written at any temperature? Assume that ΔH°rxn does not depend on temperature.   A.  2Cl2O(g)  →  2Cl2(g) + O2(g)                      ΔH°rxn = –151 kJ   B.   3O2(g)  →  2O3(g)                                        ΔH°rxn = +284 kJ   C.  COCl2(g)  →  CO(g) + Cl2(g)                      ΔH°rxn = +112 kJ   D.  2C(s) + 2S(s) + O2(g)  →  2COS(g)            ΔH°rxn = –137 kJ   E.  N2O4(g)  →  2NO2(g)                                   ΔH°rxn = +171 kJ

Calculate the standard enthalpy change for the reaction at 25 °C. Standard enthalpy of formation values can be found in this list of thermodynamic properties. MgCl₂ (s) + H₂O(1) AH;xn= V → B MgO(s) + 2 HCl(g) MacBook Air H N M 1 9 DD $10 P m kJ

Calculate ∆H for the reaction below using Hess’s law.

What is AS for the combustion of propane? C3H8(g) +502(g) → 3CO2(g) + 4H₂O(g) Substance C3H8(g) O2(g) CO2(g) H₂O(g) S(J/K mol) 269.9 205.0 213.6 188.7

Calcium ΔHof (kJ/mol) ΔGof (kJ/mol) So (J/mol K) Ca (s) 0 0 41.4 Ca (g) 178.2 144.3 158.9 Ca2+ (g) 1925.9     CaC2 (s) -59.8 -64.9 70.0 CaCO3 (s, calcite) -1206.9 -1128.8 92.9 CaCl2 (s) -795.8 -748.1 104.6 CaF2 (s) -1219.6 -1167.3 68.9 CaH2 (s) -186.2 -147.2 42.0 CaO (s) -635.1 -604.0 39.8 CaS (s) -482.4 -477.4 56.5 Ca(OH)2 (s) -986.1 -898.5 83.4 Ca(OH)2 (aq) -1002.8 -868.1 -74.5 Ca3(PO4)2 (s) -4126.0 -3890.0 241.0 CaSO4 (s) -1434.1 -1321.8 106.7 CaSiO3 (s) -1630.0 -1550.0 84.0       Carbon ΔHof (kJ/mol) ΔGof (kJ/mol) So (J/mol K) C (s, graphite) 0 0 5.7 C (s, diamond) 1.9 2.9 2.4 C (g) 716.7 671.3 158.1 CCl4 (l) -135.4 -65.2 216.4 CCl4 (g) -102.9 -60.6 309.9 CHCl3 (l) -134.5 -73.7 201.7 CHCl3 (g) -103.1 -70.3 295.7 CH4 (g) -74.8 -50.7 186.3 CH3OH (g)…

Answer this question without using numbers from the book (or anywhere else!) ΔS for the following reaction is negative. True or false?   2 CO(g) + O2(g) → 2 CO2(g)

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 129.0 °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. AH = -92. kJ J - 197. K AS = ? N, (g) + 3H, (g) 2NH, (3) AG = ||| kJ 2 Which is spontaneous? this reaction the reverse reaction neither