Tiny samples of aqueous solutions are sketched below, as if under a microscope so powerful that individual molecules could be seen. (The water molecules are not shown.) The two substances in each sample can interconvert. That is, each kind of molecule can turn into the other. The equilibrium constant K for each interconversion equilibrium is shown below the sketch. Decide whether each solution is at equilibrium. K=4 K = At equilibrium? At equilibrium? O yes O no O yes O no K=9 K = At equilibrium? At equilibrium?

At a certain temperature, the equilibrium constant K for the following reaction is ×2.0510−7 : Br2g + OCl2g BrOCl g+BrClg Use this information to answer the following question.   What is the equilibrium constant for the following reaction? Round your answer to 3 significant digits. K= 3Br2 (g) +3OCl2 (g)   3BrOCl (g) +3BrCl (g

For the chemical equation 2SO2(g) + NO2(g) 2SO3(g) + NO(g) The equilibrium constant at a certain temperature is 5.50. At this temperature, calculate the number of moles of NO2(g) that must be added to 1.20 mol SO2(g) in order to form 0.80 mol SO3(g) at equilibrium.

True/False. Explain your answer in one sentence or less.   In an equilibrium process, the concentrations of products and of reactants are equal. The value of the equilibrium constant for a given reaction depends on the initial concentrations of reactants. Large value for equilibrium constant K means the reaction will be less complete at the equilibrium point. The concentration of a pure solid is left out of an equilibrium constant expression but a pure liquid is included.

Consider the combustion of methane (as represented by the following equation). This is the reaction that occurs for a Bunsen burner, which is a source of heat for chemical reactions in the laboratory. CH 4(9) +20 2(g) =CO2(g) + 2H 20(g) For the system at chemical equilibrium, which of the following explains what happens if the temperature is reduced? O a. The equilibrium position is shifted to the left and the value for K increases. O b. The equilibrium position is shifted to the right and the value for K increases. O c. The equilibrium position is shifted to the right and the value for K decreases. O d. The equilibrium position is shifted but the value for K stays constant. Oe. The equilibrium position is shifted to the left and the value for K decreases.

A chemist is studying the following equilibirum, which has the given equilibrium constant at a certain temperature: 2 CH₂(g)3H₂(g) + C₂H₂ (g) K₂=6. x 108 He fills a reaction vessel at this temperature with 11. atm of methane gas. Use this data to answer the questions in the table below. Can you predict the equilibrium pressure of H₂, using only the tools available to you within ALEKS? If you said yes, then enter the equilibrium pressure of H₂ at right. Round your answer to 1 significant digit. yes no at atm x10 X

Consider the equilibrium system described by the chemical reaction below. Determine the concentration of O, at equilibrium by writing the equilibrium constant expression and solving it. Complete Parts 1-2 before submitting your answer. = 2 H₂O(g) 2 H2(g) + O̟₂(g) 1 2 NEXT At this temperature, the Kc = 2.4 × 103 and the equilibrium concentrations of H2O and H2 are 0.11 M and 0.019 M, respectively. If [x] represents the equilibrium concentration of O2, set up the equilibrium expression for Kc to solve for the concentration. Each reaction participant must be represented by one tile. Do not combine terms. Кс = 2' = 2.4 × 103 > RESET [0.11] [0.019] 2[0.11] 2[0.019] [0.11]² [0.019]² [x] [x]² [2x] [2x]²

A chemist is studying the following equilibirum, which has the given equilibrium constant at a certain temperature: N2(g) + 2H2O(g) 2 NO(g) + 2 H2(g) K=2.x 10 -10 He fills a reaction vessel at this temperature with 6.0 atm of nitrogen gas and 11. atm of water vapor. Use this data to answer the questions in the table below. Can you predict the equilibrium pressure of H2, using only the tools available to you within ALEKS? ○ yes x10 O no If you said yes, then enter the equilibrium pressure of H₂ at right. Round your answer to 1 significant digit. atm 5

1. What conditions of temperature and pressure favor products in the following reaction: PCl5(g) ⇌ PCl3(g) + Cl2(g) ΔH = 238 kJ/mol   2. Consider the system below. When equilibrium is restored, how will the number of each type of molecule and the concentration of each substance compare to those before the stress was introduced? Complete the following table using the words “decrease,” “same,” or “increase.” 2 NH3(g) ⇌ N2(g) + 3 H2(g)      ΔH = 92.4 kJ/mol       Decrease Volume Decrease Temperature Equilibrium Concentration N2     H2     NH3     Equilibrium Number N2     H2     NH3     3. Nitric acid is produced commercially by the Ostwald process. The first step of the Ostwald process is: 4 NH3(g) + 5 O2(g) ⇌ 4 NO(g) + 6 H2O(g) + energy In which direction will the above system shift in the following situations: 3. (a) Some NO is added.

Calculating an equilibrium constant from a partial equilibrium.. Sulfur dioxide and oxygen react to form sulfur trioxide during one of the key steps in sulfuric acid synthesis. An industrial chemist studying this reaction fills a 2.0 L flask with 3.9 atm of sulfur dioxide gas and 0.74 atm of oxygen gas, and when the mixture has come to equilibrium measures the partial pressure of sulfur trioxide gas to be 1.2 atm. Calculate the pressure equilibrium constant for the reaction of sulfur dioxide and oxygen at the final temperature of the mixture. Round your answer to 2 significant digits. K, = [ %3D do x10 Ar Eplanation Check O 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center Accessibility FEB tv 23 30 MacBook Air DII DD F12 F11 F10 F9 80 888 F8 F7 F5 F6 F4 F3 esc F2 F1 $ % @ 8. 3 4 5 6 2 U