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18 Nov 2019
In an experiment, 0.34 mol H_2 and 0.34 mol I_2 are mixed in a 1.00-L container, and the reaction forms HI. If K_c = 49, for this reaction, what is the equilibrium concentration of HI? I_2(g) + H_2(g) 2HI(g) A) 0.85 M B) 0.60 M C) 0.53 M D) 0.65 M E) 0.045 M A first-order chemical reaction is observed to have a rate constant of 32 min^-1. What is the corresponding half-life for the reaction? A) 46 min B) 1.3 min C) 45.8 s D) 1.3 s E) 1.9 s The rate law for the chemical reaction 5Br^-(aq) + BrO_3^-(aq) + 6H^+(aq) rightarrow 3Br^2(aq) + 3H_2O(l) has been determined experimentally to be Rate = k[Br^-][BrO_3^-][H^+]^2. What is the overall order of the reaction? A) 3 B) 5 C) 1 D) 4 E) 2 Consider the following equilibrium; PCI_3(g) + Cl-2(g) PCl_5(g); Delta H = -92 kJ The concentration of PCI_3 at equilibrium may be increased by A) increasing the pressure. B) adding Cl_2 to the system. C) the addition of neon. D) the addition of PCl_5. E) decreasing the temperature.
In an experiment, 0.34 mol H_2 and 0.34 mol I_2 are mixed in a 1.00-L container, and the reaction forms HI. If K_c = 49, for this reaction, what is the equilibrium concentration of HI? I_2(g) + H_2(g) 2HI(g) A) 0.85 M B) 0.60 M C) 0.53 M D) 0.65 M E) 0.045 M A first-order chemical reaction is observed to have a rate constant of 32 min^-1. What is the corresponding half-life for the reaction? A) 46 min B) 1.3 min C) 45.8 s D) 1.3 s E) 1.9 s The rate law for the chemical reaction 5Br^-(aq) + BrO_3^-(aq) + 6H^+(aq) rightarrow 3Br^2(aq) + 3H_2O(l) has been determined experimentally to be Rate = k[Br^-][BrO_3^-][H^+]^2. What is the overall order of the reaction? A) 3 B) 5 C) 1 D) 4 E) 2 Consider the following equilibrium; PCI_3(g) + Cl-2(g) PCl_5(g); Delta H = -92 kJ The concentration of PCI_3 at equilibrium may be increased by A) increasing the pressure. B) adding Cl_2 to the system. C) the addition of neon. D) the addition of PCl_5. E) decreasing the temperature.
Tod ThielLv2
30 Oct 2019