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Chapter 15 Solutions
Chemistry: Atoms First
- Actually, the carbon in CO2(g) is thermodynamically unstable with respect to the carbon in calcium carbonate(limestone). Verify this by determining the standardGibbs free energy change for the reaction of lime,CaO(s), with CO2(g) to make CaCO3(s).arrow_forwardDescribe a nonchemical system that is not in equilibrium, and explain why equilibrium has not been achieved.arrow_forwardThe ionization constant, Ka, for acetic acid is 1.8 105 at 25 C. What is the value of rG for this reaction? Is this reaction product- or reactant-favored at equilibrium?arrow_forward
- Show that the complete chemical equation, the total ionic equation, and the net ionic equation for the reaction represented by the equation KI(aq)+I2(aq)KI3(aq) give the same expression for the reaction quotient. KI3 is composed of the ions K+ and I3-.arrow_forwardAt 276.7 oC, the Kp for the reaction 2 A (g) + 1 B (g) ↔ 5 AB is Kp = 3.07⋅10-2 What is Keq?arrow_forwardConsider the following equilibria: 2A(g) 2B(g) + C(g) A(g) + E(g) → B(g) + D(g) Calculate the equilibrium constant for the reaction 2E(g) C(g) → 2D(g) ( K1 K₂arrow_forward
- The equilibrium constant for the reaction 2NO(g) + Br2 (g) = 2NOBr(g) is Ke = 1.2 × 10¬ at a certain temperature. -2arrow_forwardAgBr(s) ⇄ Ag+(aq) + Br-(aq) Ksp = 7.7 x 10-13Ag+(aq) + 2NH3(aq) ⇄ Ag(NH3)2+(aq) Kf = 1.5 x 107 When NH3 is added to AgBr(s), a combination of these reactions result:AgBr(s) + 2NH3(aq) ⇄ Ag(NH3)2+(aq) + Br-(aq)What mass of AgBr will dissolve in a 5.0 L container of 2.7 M NH3 solution? * 8.6×100 g * 2.8×10-2 g * 5.2×100 g * 9.2×10-3 g * 4.6×10-2 garrow_forwardThe decomposition of a generic diatomic element in its standard state is represented by the equation x,(g) → X(g) Assume that the standard molar Gibbs energy of formation of X(g) is 5.51 kJ · mol-! at 2000. K and –57.84 kJ · mol- at 3000. K. Determine the value of the thermodynamic equilibrium constant, K, at each temperature. At 2000. K, AGf = 5.51 kJ · mol-. What is K at that temperature? K at 2000. K = At 3000. K, AGf = -57.84 kJ · mol-1. What is K at that temperature? K at 3000. K =arrow_forward
- Given the following ionic equilibria and their K values: AgBr(s) ⇌ Ag+(aq) + Br–(aq); Ksp = 5.0 x 10–13 Ag+(aq) + 2NH3(aq) ⇌ Ag(NH3)2+(aq); Kf = 1.7 x 107 What is Kc for the following equilibrium? AgBr(s) + 2NH3(aq) ⇌ Ag(NH3)2+(aq) + Br–(aq); (A) 8.5 x 10–6 (B) 2.9 x 10–20 (C) 3.4 x 1019 (D) 1.7 x 107arrow_forwardThe decomposition of a generic diatomic element in its standard state is represented by the equation X,(g) X(g) > Assume that the standard molar Gibbs energy of formation of X(g) is 4.25 kJ · mol- at 2000. K and -65.74 kJ · mol- at 3000. K. Determine the value of the thermodynamic equilibrium constant, K, at each temperature. At 2000. K, AG; = 4.25 kJ · mol-. What is K at that temperature? K at 2000. K : At 3000. K, AG¢ = -65.74 kJ · mol-1. What is K at that temperature? K at 3000. K =arrow_forwardThe equilibrium constant, Kc, for the following reaction is 6.54 × 10-³ at 298 K. -3 2NOBr(g) 2NO(g) + Br₂(g) Calculate Ke at this temperature for the following reaction: с NO(g) + 1/2Br2(g) → NOBr(g) Kc =arrow_forward
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