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Chapter 15 Solutions
Chemistry: Atoms First
- Describe 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_forwardShow 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_forward
- The 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 4.23 kJ · mol-1 at 2000. K and –56.22 kJ · mol-1 at 3000. K. Determine the value of the thermodynamic equilibrium constant, K, at each temperature. At 2000. K, AG; = 4.23 kJ · mol-1. What is K at that temperature? K at 2000. K = At 3000. K, AG{ -56.22 kJ · mol-1. What is K at that temperature? K at 3000. K =arrow_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_forwardNitrogen and oxygen react at high temperatures.(a) Write the expression for the equilibrium constant (Kc) for the reversible reactionN2(g) + O2(g) ⇌ 2NO(g) ΔH = 181 kJarrow_forward
- The 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_forwardThe equilibrium constant for the reaction 2NO(g) + Br2 (g) = 2NOBr(g) is Ke = 1.2 × 10¬ at a certain temperature. -2arrow_forwardThe equilibrium constant for the equilibrium CO (g) +H 2 O (g) =CO 2(g) +H 2(g) ) is 302 at 600K. What is the value of the equilibrium constant for the reverse reaction at the same temperature?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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