Consider the decomposition of the compound C5H6O3 as follows:C5H6O3(g) → C2H6(g) + 3CO(g)When a 5.63-g sample of pure C5H6O3(g) was sealed into an otherwise empty 2.50-L flask and heated to 200°C, the pressure in the flask gradually rose to 1.63 atm and remained at that value. Calculate K for this reaction

3.) For the following equilibrium reaction2NO2(g) ↔N2O4(g) + Δlook in the Tro text to see what LeChatelier's principle states about gases. Assume that the reaction occurs in an enclosed movable piston. [Hint: remember that PV=nRT] a.) The pressure of the reaction is increased. b.) The volume of the reaction is decreased. c.) The volume of the reaction is increased.

The equilibrium constant, Kc, for the following reaction is 55.6 at 698 K.H2 (g) + I2 (g) 2 HI (g)Calculate the equilibrium concentrations of reactants and product when 0.228 moles of H2 and 0.228 moles of I2 are introduced into a 1.00 L vessel at 698 K. [ H2 ] = M [ I2 ] = M [ HI ] = M

The equilibrium constant, Kp, equals 3.40 at 25°C for the following isomerization reaction- cis-2-butene trans-2-butene If a flask initially contains 1.00 atm of each gas, what will happen in order for the system to reach equilibrium? More cis-2-butene will be produced. It is already at equilibrium. More trans-2-butene will be produced. The system will not reach equilibrium.

The equilibrium constant Kp for the reaction PC15(g) = PC13(g) + Cl₂(g) is 1.05 at 250°C. The reaction starts with a mixture of PC15, PC13, and Cl₂ at pressures 0.177 atm, 0.233 atm, and 0.161 atm, respectively, at 250°C. When the mixture comes to equilibrium at that temperature, which pressure(s) will have decreased? Cl₂ PC13 PC15

1. 2.00 moles of ammonia are heated in a sealed 1.00 L container at 650°C. At this temperature, ammonia decomposes to nitrogen and hydrogen gas. 2 NH3 (g) = N2 (g) + 3 H2 (g) At equilibrium, the concentration of ammonia in the container is 1.00 M. What is the value of Ke for this reaction at 650°C?

● Nitrogen dioxide decomposes according to the rection: 2NO₂(g) → 2 NO(g) + O₂(g) where Kp = 4.48x 10-13. A pressure of 0.75 atm of NO₂ is introduced into a 1.00 L container and allowed to come to equilibrium. What are the equilibrium partial pressure of NO(g) and O₂(g)?

Carbon tetrachloride can be produced by the following reaction: C5₂(g) + 3Cl₂(g) + S₂Cl₂(g) + CCl₂) In an experiment, 0.120 mol of CS₂ and 0.360 mol of Cly were placed in a 1.00-L flask at a particular temperature. After equilibrium has been achieved, the mixture contains 0.040 mol CCl Calculate the value of K under the experimental conditions

A chemical engineer is studying the following reaction: H₂(g) + Cl₂(g) → 2 HCl(g) At the temperature the engineer picks, the equilibrium constant K, for this reaction is 0.83. The engineer charges ("fills") three reaction vessels with hydrogen and chlorine, and lets the reaction begin. He then measures the composition of the mixture inside each vessel from time to time. His first set of measurements are shown in the table below. Predict the changes in the compositions the engineer should expect next time he measures the compositions. reaction vessel A C compound H₂ Cl₂ HCI H₂ CL₂ HCI H₂ CL₂ HCI pressure 4.00 atm 1.97 atm 3.36 atm 4.27 atm 2.82 m 3.84 atm 1.81 atm 3.69 atm expected change in pressure 1 increase O decrease decrease Of increase Of increase Ⓒ↓ decrease Of increase O decrease decrease O1 increase Ot increase O decrease Of increase O decrease Of increase O decrease decrease Of increase O (no change) (no change) O(no change) (no change) (no change) (no change) (no change) (no…