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Chapter 15 Solutions
Chemistry: Atoms First
- The 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_forwardActually, 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_forward
- Given the following data: PtCl42(aq)+2ePt(s)+4Cl(aq)Ered=0.73VPt2+(aq)+2ePt(s)Ered=1.20V Find Kffor PtCl42- at 25°C.arrow_forwardThe equilibrium constant of a reaction is 3.1 ✕ 103 at 359 K and 1.8 ✕ 102 at 450. K. What are ΔH° and ΔS° for the reaction?arrow_forwardWrite the equilibrium constant for the reaction P4(s) + 6 H2(g) ⇋ 4 PH3(g), with the gases treated as perfect.arrow_forward
- Write down the thermodynamic equilibrium constant expressions of the following reactions. If possible, associate them with Kc and Kp.(a) Si (k) + 2 Cl₂ (g) ↔ SiCl ₄ (g)(b) Cl₂ (g) + H₂O (s) ↔ HOCl (aq) + H⁺ (aq) + Cl- (aq)arrow_forwardThe equilibrium constant for the reaction N2(g) + 3 H2(g) ⇌ 2 NH3(g), which corresponds to the formation of ammonia by the Haber process, is 2.13 x 106 at 288 K and 1.75 x 105 at 308 K. Calculate the standard reaction enthalpy at 298 K.arrow_forwardThe equilibrium constant for the reaction N2(g) + 3 H2(g) ⇋ 2 NH3(g) is 2.13 × 106 at 288 K and 1.75 × 105 at 308 K. Calculate the standard reaction enthalpy, assuming it to be constant over this temperature range.arrow_forward
- The decomposition reaction, C(g) -><- A(g) + 3B(g) has Kc = 39 at 298 K. What is the value of Kp for this system at 298 K?arrow_forwardAt 400 degrees celsius, Kp = 64 for the following reaction: H2 (g) + I2 (g) 2 HI (g) What is the value of Kc for this reaction?arrow_forwardWrite the reaction quotient for each of the following reaction:a). The decomposition of dinitrogen pentoxide, N2O5(g) ↔ NO2(g) + O2(g)b). The combustion of propane, C3H8(g) + O2(g) ↔ CO2(g) + H2O(g)arrow_forward
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