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Chemistry - With Access (Looseleaf) (Custom)
- What is the sign of ΔS for the reaction Na2B4O7(s) 2 Na+(aq) + B4O72-(aq) ?arrow_forwardFor which set of conditions is the reaction always nonspontaneous? ΔH = + and ΔS = + ΔH = - and ΔS = - ΔH = - and ΔS = + ΔH = + and ΔS = - ΔH = 0 and ΔS = 0arrow_forwardEstimate the sign of the entropy change for the reaction: CaCO3 (s) → CaO (s) + CO2 (g) Select one: a. is zero b. negative c. not possible to determine the sign d. none of these e. positivearrow_forward
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- For the reaction conducted at 300 K below, 1.0 atm of A was placed in a chamber, and the equilibrium pressure of B was determined to be 0.4 atm. Based on this information answer the following: A (g) <---->2 B (g) If the same reaction were performed and the partial pressure of A was 0.6 atm when DG=18 kJ/mole, what would be the pressure of B? Is the reaction spontaneous in the forward or reverse direction at this point of the reaction?arrow_forwardUsing ΔG = ΔH – TΔS, explain under what circumstances the following processes would be spontaneous: a. ΔH<0 and ΔS>0 b. ΔH>0 and ΔS<0 c. ΔH<0 and ΔS<0 d. ΔH>0 and ΔS>0arrow_forwardFor a spontaneous chemical reaction which of the following are possible signs of ΔΔH and ΔΔS? Select one: a. both b and c b. ΔΔH = (+) and ΔΔS = (-) c. ΔΔH = (-) and ΔΔS = (+) d. neither b nor c Clear my choicearrow_forward
- Which of the following is NOT true for ΔGrxn? A) If ΔG°rxn > 0, the reaction is spontaneous in the forward direction. B) If Q = 1, then ΔGrxn = ΔG°rxn. C) ΔG°rxn = K D) If ΔG°rxn > 0, the reaction is spontaneous in the reverse direction. E) Under equilibrium conditions, ΔGrxn = 0.arrow_forwardAt 298 K, ΔH° for this reaction is -137.5 kJ/mol, and ΔS° is +120.5 J/K. What is the value of ΔG° (in kJ/mol) at 25 °C for the following the reaction? C₂H₄ (g) + H₂ (g) → C₂H₆ (g)arrow_forwardCalculate the entropy change when graphite burns insufficient supply of oxygen as shown in the following equation, C graphite (s) + O2 (g) -> CO2 (g) Given: S° of C graphite (s) = 5.7 J/molK S° of O2 (g) = 205 J/molK S° of CO2 (g) = 213.6 J/molKarrow_forward
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