Predict the conditions (high temperature, low temperature, all temperatures, or no temperatures) under which each of the following reactions will be spontaneous. Drag the appropriate items to their respective bins. ► View Available Hint(s) High temperature 2NO₂(g) → 2NO(g) + O₂(g) (endothermic) Low temperature H₂(g) → 2H(g) CO₂ (s) → CO₂(g) H₂O(g) → H₂O(1) All temperatures No temperatures Reset Help

Predict the conditions (high temperature, low temperature, all temperatures, or no temperatures) under which each of the following reactions will be spontaneous. Drag the appropriate items to their respective bins. ► View Available Hint(s) High temperature 2NO₂(g) → 2NO(g) + O₂(g) (endothermic) Low temperature H₂(g) → 2H(g) CO₂ (s) → CO₂(g) H₂O(g) → H₂O(1) All temperatures No temperatures Reset Help

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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One industrial, large-scale method for refining iron ore to elemental iron is the reaction at high temperatures with carbon monoxide. Calculate AGº for the reaction of iron(III) oxide with carbon monoxide to give elemental iron and carbon dioxide. Use data in the table below: Substance Ag(s) AgCl(s) Al(s) Al₂O3(s) C(s) (graphite) CO(g) CO₂(g) CH4(g) CH₂Cl(g) CH₂OH(1) C₂H₂(g) C₂H4(g) C₂H6(g) C₂H18(1) C₂H,OH() Ca(s) CaCO3(s) CaCl₂(s) 197.9 213.6 186.2 234.2 126.8 CO(NH,),(s) 104.6 CO(NH,),(aq) 173.8 200.8 219.8 229.5 466.9 161 Substance Ag(s) AgBr(s) AgCl(s) Al(s) Al₂O3(s) C(s) (graphite) C₂H₂(g) C₂H₂(g) C₂H6(g) C₂H Ca(s) Standard Entropies of Some Typical Substances at 298.15 K CaBr₂(s) CaCO3(s) CaCl₂(s) CaO(s) Fe₂O3(s) H₂(g) H₂O(g) H₂O(1) (J mol-¹ K-¹) 42.55 96.2 28.3 51.0 CO(g) CO₂(g) CH4(g) CH₂Cl(g) CH31(g) CH₂OH(1) CO(NH₂)2(s) (urea) CO(NH,),(aq) AG° = kJ 5.69 Ca(OH)2 (s) CaSO4(s) CaSO4 H₂O(s) CaSO4-2H₂O(s) Cl₂(g) Fe(s) 41.4 92.9 114 Substance (J mol-¹ K-¹) CaO(s) 40 Ca(OH)₂ (s)…
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
For a given reaction, dH = 32 kJ/mol and dS = 117 J/mol. At approximately what temperature would this reaction become spontaneous?
Calculate ΔHf for HCN(g) at 25°C, given the following related reaction at 25°C, 2 NH3(g) + 3 O2(g) + 2 CH4(g) ---> 2 HCN(g) + 6 H2O(g); ΔHrxn = -870.8 kJ and the heats of formation of some species are ΔHf = -80.3 kJ/mol for NH3(g), -74.6 kJ/mol for CH4, and -241.8 kJ/mol for H2O(g). Answers are in kJ/mol.
The decomposition of N2O4 is an endothermic reaction, shown below:N2O4(g) → 2 NO2(g) Will this reaction be favored at all temperatures, at high temperatures, at low temperatures or at no temperatures?Justify your selection.
From the data at 25 °C: Fe2O3(s) + 3C(graphite) → 2 Fe(s) + 3 CO(g) ∆Ho = 492.6 kJ/mol FeO(s) + C(graphite) → Fe(s) + CO(g) ∆Ho = 155.8 kJ/mol C(graphite) + O2(g) → CO2(g) ∆Ho = - 393.5 1 kJ/mol CO(g) + ½ O2(g) → CO2(g) ∆Ho = - 282.98 kJ/mol Compute the standard heat of formation of FeO (s) and of Fe2O3(s).
Show work. Given the following reactions, M represents a generic metal. All reactions are balanced. 1. 2 M(s) + 3 Cl2 (g) = 2 MCl3(s) ∆H° = -6201.8 kJ/mol 2. H2 (g) + Cl2 (g) = 2 HCl(g) ∆H° = -1855.0 kJ/mol 3. HCl(g) = HCl(aq) ∆H° = -71.8 kJ/mol 4. MCl3(s) = MCl3 (aq) ∆H° = -169.0 kJ/mol Use the above information to determine the enthalpy of this reaction: 2 M(s) + 6 HCl(aq) = 2 MCl3 (aq) + 3 H2 (g) ∆H° = ???
When 2.53 g of CaCl2 was dissolved in 30.00 g of water in an adiabatic calorimeter at 23.0°C, the temperature of the solution went up to 36.5°C. Find ΔH (in kJ/mol) for the dissolution of one mole of CaCl2 in water. (The molar mass of CaCl2 is 110.978 g/mol.)
1. On the basis of your experience, predict which of the following reactions are spontaneous. 1) NaCl(s)→→ NaCl(/) at 25 °C 2) 2 NaCl(s)→→ 2 Na(s) + Cl₂(g) 3) CO2(g) → CO2(s) at 25 °C 4) CO2(g) → C(s) + O2(g) 5) H₂O(s)→ H₂O() at 25 °C a) 1, 2, and 3 b) 1, 2, and 4 c) 3 and 5 d) 3 e) 5
Read the descriptions of physical or chemical changes in the table below. Then decide whether the change will be spontaneous, if you can. Change During an endothermic chemical reaction, four moles of gaseous reactants are turned into two moles of gaseous products. A solid precipitates from a solution, releasing heat as it does so. A solid absorbs heat and turns to a gas. Is this change spontaneous? Yes. O No. O Can't decide with information given. O Yes. O No. O Can't decide with information given. O Yes. O No. O Can't decide with information given.
Under what temperature conditions (low T, high T, all T, nonspontaneous at all T) would this reaction occur spontaneously? Explain your reasoning. 2NH4NO3(s) → 2N2(g) + 4H2O(l) + O2 (g) , ∆Horxn = -236.0 kJ
. 2 H2S(g) + 3 O2(g) → 2 SO2(g) + 2 H2O(g) Delta Hrxn = -1036 kJ; Delta Srxn = -153.2 J/K At above what temperature (roughly) the reaction becomes nonspontanesous? A)158.7 K B) 298 K C) 6.762 × 103 K D) 273.16K F) 6.762 K