A sample of an organic compound is added to a mixture of octanol and water. After the mixture has reached equilibrium the concentration of the compound in the octanol layer is found to be 2.00x10 mol/L. The concentration in the water layer is found to be 8.50x10 mol/L. Calculate the octanol/water partition coefficient (LogP) for the compound. 2.

During an experiment, 0.217 mol of H₂ and 0.217 mol of 12 were placed into a 1.64 liter vessel of a high-pressure reactor where the reaction H₂(g) +12(g) → 2HI(g) came to equilibrium. For this reaction, Kc = 49.5 at the temperature of the experiment. What were the equilibrium concentrations of H₂, 12, and HI?

Bromine monochloride is synthesized using the reaction Br, (g) + Cl, (g) = 2BrCl(g) Кр 1.1 x 10-4 at 150 K A 206.0 L flask initially contains 0.965 kg of Br, and 1.012 kg of Cl,. Calculate the mass of BrCl, in grams, that is present in the reaction mixture at equilibrium. Assume ideal gas behavior. mass of BrCl: g What is the percent yield of BrCl? percent yield:

Consider the reaction: P(s) + 3/2Cl₂ (9) ⇒ PCls (g) Write the equilibrium constant for this reaction in terms of the equilibrium constants, K₁ and K₂, for the reactions below: $ 4 P(s) +5/2C1₂ (9) PC15 (9) K1 PC13 (9) + Cl₂ (g) =PC15 (9) K₂ Submit Answer For answers with both a subscript and a superscript, enter the subscript first. For example, enter K? If the first equilibrium constant should be squared. K = 000 000 F4 R F Show Hint % 5 Retry Entire Group 9 more group attempts remaining [Review Topics] [References] Use the References to access important values if needed for this question. F5 T Cengage Learning Cengage Technical Support G A 6 MacBook Air F6 Y H & ✓ 7 ◄◄ F7 U * 8 J F8 ( 9 ►► K F9 O ) DIO 1108 chat 0 L F10 - P - ^ Previous F11 SAVAGE X FENTY... { + = Next> Save and Exit F12 11 G

Initial (M) Change (M) Equilibrium (M) Consider the reaction of SO₂ and O₂ described by the chemical reaction below. Determine the equilibrium constant for this reaction by constructing an ICE table, writing the equilibrium constant expression, and solving it. Complete Parts 1-2 before submitting your answer. 2 SO₂(g) + O₂(g) = 2 SO₂(g) NEXT A 2.00 L reaction vessel was filled 0.0432 mol SO₂ and 0.0296 mol O₂ at 900 K and allowed to react. At equilibrium, the concentration of SO, was found to be 0.0175 M. Fill in the ICE table with the appropriate value for each involved species to determine concentrations of all reactants and products. -0.00875 0.0209 0 0.00875 2SO₂(g) Question 20 of 33 2.00 0.0216 0.0432 0.0148 0.0296 0.0041 O₂(g) 0.0175 2 0.0129 -0.0175 0.0061 RESET -0.0350 0.0257 2SO₂(g)

Consider the following reaction where K. = 5.10×10-6 at 548 K. NHẠCI(s)ENH3(g) + HCl(g) A reaction mixture was found to contain 5.15x10² moles of NHCI(s), 1.56×103 moles of NH3(g), and 2.26x103 moles of HCI(g), in a 1.00 liter container. Is the reaction at equilibrium? If not, what direction must it run in order to reach equilibrium? The reaction quotient, Qc, equals The reaction A. must run in the forward direction to reach equilibrium. B. must run in the reverse direction to reach equilibrium. C. is at equilibrium.

Write the reaction and Ksp expression for dissolving silver sulfate in water.

For the aqueous [Co(NH3)] complex K = 1.58 × 1035 at 25 °C. Suppose equal volumes of 0.0036M Co (NO3), solution and 0.84M NH3 solution are mixed. Calculate the equilibrium molarity of aqueous Co 3+ ion. Round your answer to 2 significant digits. Шм ☐

For the reversible decomposition/hydration reaction of CH3CO2CH3 (0.308 M) and H2O (0.110 M) to yield acetic acid (0.211 M) and methanol (0.076 M), what is the value for the Law of Mass Action?  The equilibrium concentrations for each chemical are provided in parentheses after their name.  This reaction occurs in the aqueous phase.     629     0.0110     0.00159     0.0521     19.2

The equilibrium constant, K, for the following reaction is 77.5 at 600 K. CO(g) + Cl₂(g) Calculate the equilibrium concentrations of reactant and products when 0.470 moles of CO and 0.470 moles of Cl₂ are introduced into a 1.00 L vessel at 600 K. [CO] [Cl₂] [COCI₂] = COCI₂(g) || M ΣΣ M