Consider the following generic reaction: 2A2B (g) ⇌ 2A2 (g) + B2 (g) Some molecules of A2B are placed a 1.0-L container. As time passes, several snapshots of the reaction mixture are taken as illustrated below. Which illustration is the first to represent an equilibrium mixture? Explain. How many molecules of A2B reacted initially?

Nitrogen and water react to form nitrogen monoxide and hydrogen, like this: N2(9) + 2 H,O(g) 2 NO(g) + 2 H2(g) → Also, a chemist finds that at a certain temperature the equilibrium mixture of nitrogen, water, nitrogen monoxide, and hydrogen has the following composition: compound pressure at equilibrium N2 92.2 atm H,O 76.1 atm NO 19.3 atm H2 33.6 atm Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits. K = 0

CO2 and H, are allowed to react until an equilibrium is established as follows: CO2 (g) + H, (g)H,0 (g) + CO (g) What will be the effect on the equilibriumn of removing CO from the equilibrium mixture?

The following reaction is exothermic. 2 NO(g) + 2 H2(g) ⇔ N2(g) + 2 H2O(g) In which direction does the equilibrium shift as a result of each of the following changes? Here are the possible answers: to the right, to the left, no effect Place these actions in chronological order. Space 1: The hydrogen gas is removed. Space 2: The gas pressure in the reaction vessel is increased by decreasing its volume. Space 3: The gas pressure in the reaction vessel is increased by pumping argon gas into it while keeping the volume constant. Space 4: We raise the temperature. Space 5: A catalyst is used.

At a certain temperature, Keq for the following reaction between sulfur dioxide and nitrogen dioxide is 4.8.   SO2(g)   +   NO2(g)   ↔   NO(g)   +   SO3(g)   SO2(g) and NO2(g) have the same initial concentration:   0.36 mol/L.  What amount of SO3(g) is present in a 5.0 L container at equilibrium?

SC At a certain temperature, the equilibrium constant K for the following reaction is 506.: Br₂(g) + OC1₂(g) BrOCI(g) + BrCl(g) Use this information to complete the following table. Suppose a 46. L reaction vessel is filled with 0.62 mol of Br₂ and 0.62 mol of OCI₂. What can you say about the composition of the mixture in the vessel at equilibrium? ! 1 What is the equilibrium constant for the following reaction? Round your answer to 3 significant digits. BrOCI(g)+BrCl(g) Q A What is the equilibrium constant for the following reaction? Round your answer to 3 significant digits. 2 Br₂(9)+20C1₂(9) P 2 BrOCI(g)+2BrCl(9) Explanation NO 2 W S Check *3 # E Br₂(9)+OCL₂(9) D D DS 4 C R F % LO 5 O There will be very little Br₂ and OCl₂. O There will be very little BrOCI and BrCl. ONeither of the above is true. K = 0 K = 0 T MacBook Pro 20 ^ 6 G Y C & 7 H 2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy C U 00 8 J X I ( 9 K 0 0 < F

The following reaction has an equilibrium constant of 2.65 x10-3 at 300K. Br2 (g) + Cl2 (g) 2 BrCl (g) Which of the following statements is true?   Question 5 options:   The system has a higher concentration of reactant molecules than product molecules at equilibrium, but there are significant quantities of both.   The system consists almost entirely of reactant molecules at equilibrium.   The system consists almost entirely of product molecules at equilibrium.   The system has approximately equal concentrations of product and reactant molecules at equilibrium.   The system has higher concentrations of product molecules than reactant molecules at equilibrium, but there are significant quantities of both.

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Iron and water react to form iron(III) oxide and hydrogen, like this: 2 Fe(s) + 3 H₂O(g) → Fe₂O3(s)+ 3 H₂(g) At a certain temperature, a chemist finds that a 2.5 L reaction vessel containing a mixture of iron, water, iron(III) oxide, and hydrogen at equilibrium has the following composition: compound Fe H₂O Fe₂O3 H₂ amount 4.04 g 2.87 g 3.49 g 2.08 g Calculate the value of the equilibrium constant K for this reaction. Round your answer to 2 significant digits. C K = 0 C Dx1 x10 X Ś