A chemical engineer is studying the following reaction: CH4(9)+2H₂S(g) → CS₂(g) + 4H₂(g) At the temperature the engineer picks, the equilibrium constant K for this reaction is 1.7 × 10³. P The engineer charges ("fills") four reaction vessels with methane and hydrogen sulfide, 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 B compound CH4 H₂S CS₂ H₂ CH4 H₂S CS₂ H₂ pressure 5.65 atm 3.56 atm 5.77 atm 7.93 atm 4.69 atm 1.62 atm 6.73 atm 11.81 atm expected change in pressure † increase ↑ increase Ot increase Ot increase Ot increase Ot increase ↑ Ot increase ↑ increase O decrease Odecrease Odecrease Odecrease decrease Odecrease Odecrease Odecrease (no change) O(no change) O(no change) (no change) (no change) (no change) O(no change) (no change)

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 0.33. The engineer charges ("fills") three reaction vessels with hydrogen and chlorine, and lets the reaction begin. She then measures the composition of the mixture inside each vessel from time to time. Her first set of measurements are shown in the table below. Predict the changes in the compositions the engineer should expect next time she measures the compositions. reaction vessel A B с compound H₂ C1₂ HC1 H₂ CL, HCl H₂ CL₂2 HC1 pressure 4.42 atm 5.14 atm 1.90 atm 3.61 atm 4.33 atm 3.53 atm 4.59 atm 5.31 atm 1.57 atm expected change in pressure ↑ increase ↑ increase ↑ increase ↑ increase ↑ increase ↑ increase ↑ increase ↑ increase ↑ increase ↓ decrease ↓decrease ↓ decrease ↓ decrease ↓ decrease ↓ decrease ↓decrease ↓decrease ↓ decrease (no change) (no change) (no change) (no change) (no change) (no change) (no…

At a certain temperature, the equilibrium constant K for the following reaction is 5.36 x 10": H,(g) + Cl,(g) = 2 HCI(g) Use this information to complete the following table. Suppose a 33. L reaction vessel is filled with 0.63 mol of HCI. What can you say about the composition of the mixture in the vessel at equilibrium? O There will be very little H2 and Cl2. O There will be very little HCI. O Neither of the above is true. What is the equilibrium constant for the following reaction? Round your answer to 3 significant digits. K = ] 2 HCl(g) H,(9)+Cl,(9) What is the equilibrium constant for the following reaction? Round your answer to 3 significant digits. K = ] 2 H,(9)+2Cl,(9) 4 HCl(g) Continue O 2022 McGraw Hill LLC. All Rights Reserve 43,203 FEB 18 9 PP SESS

Using the general properties of equilibrium constants At a certain temperature, the equilibrium constant K for the following reaction is 7.45 × 10-5: NO₂(g) + CO(g) ⇒ NO(g) + CO₂(g) Use this information to complete the following table. Suppose a 20. L reaction vessel is filled with 1.5 mol of NO and 1.5 mol of CO₂. What can you say about the composition of the mixture in the vessel at equilibrium? What is the equilibrium constant for the following reaction? Round your answer to 3 significant digits. NO(g)+CO,(9) NO₂(9)+CO(9) What is the equilibrium constant for the following reaction? Round your answer to 3 significant digits. 3 NO₂(g) + 3 CO(g) P 3 NO(g)+ 3 CO₂(9) There will be very little NO2 and CO. There will be very little NO and CO₂. Neither of the above is true. K = 0 K = 0 x10 Ś ? ollo 18 Ar BA

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 5.0 L flask with 4.3 atm of sulfur dioxide gas and 3.9 atm of oxygen gas, and when the mixture has come to equilibrium measures the partial pressure of sulfur trioxide gas to be 3.9 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, = 0

A chemical engineer is studying the following reaction: H₂(g)+I₂(g) → 2 HI(g) At the temperature the engineer picks, the equilibrium constant The engineer charges ("fills") three reaction vessels with hydrogen and iodine, 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 B C compound H₂ 1₂ HI H₂ 1₂ HI H₂ 1₂ HI pressure 2.39 atm 3.83 atm 4.71 atm 2.82 atm 4.26 atm 3.85 atm 3.81 atm 5.76 atm 5.21 atm expected change in pressure ↑ increase increase ↑ increase ↑ increase ↑ increase ↑ increase ↑ increase for this reaction is 1.2. р ↑ increase ↑ increase ↓ decrease ↓decrease ↓ decrease ↓ decrease ↓decrease ↓ decrease ↓ decrease ↓decrease ↓ decrease X (no change) (no change) (no change) (no change) (no change) (no change) (no change) (no change)…

A chemical engineer is studying the following reaction: H,(g)+L,(g) 2 HI(g) At the temperature the engineer picks, the equilibrium constant K for this reaction is 1.0. The engineer charges ("fills") three reaction vessels with hydrogen and iodine, 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 compound pressure expected change in pressure H, 2.86 atm O 1 increase O (no change) decrease 2.34 atm O t increase OI decrease O (no change) HI 1.38 atm O f increase decrease O (no change) H, 2.45 atm O t increase decrease O (no change) 1.93 atm O t increase O I decrease o (no change) B O t increase O (no change) HI 2.21 atm decrease 2.75 atm O t increase o (no change) H, decrease 2 23 atm O t Increase decrease O (no change) HI O T increase decrease…

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 500. mL flask with 1.2 atm of sulfur dioxide gas and 4.7 atm of oxygen gas, and when the mixture has come to equilibrium measures the partial pressure of sulfur trioxide gas to be 0.60 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, -0 x10 5

Suppose a 500. mL flask is filled with 1.1 mol of NO2, 1.7 mol of NO and 0.90 mol of CO2. The following reaction becomes possible: NO, (g)+CO(g) NO(g) +CO,(s) The equilibrium constant K for this reaction is 0.292 at the temperature of the flask. Calculate the equilibrium molarity of NO. Round your answer to two decimal places. м B C ol

A chemical engineer is studying the following reaction: 2 H,S(g)+302(9) → 2 SO,(g)+2H,O(9) At the temperature the engineer picks, the equilibrium constant K, for this reaction is 3.2. The engineer charges ("fills") four reaction vessels with hydrogen sulfide and oxygen, and lets the reaction begin. She then measures the composition of the mixture inside each vessel from time to time. Her first set of measurements are shown in the table below. Predict the changes in the compositions the engineer should expect next time she measures the compositions. reaction compound pressure expected change in pressure vessel H,S 2.22 atm O f increase OI decrease O (no change) 3.39 atm O t increase O I decrease O (no change) so, O I decrease O (no change) 6.16 atm O t increase H,0 8.72 atm O increase O! decrease O (no change) H, S 1.96 atm O t increase OI decrease O (no change) 0, 3.00 atm O f increase O I decrease O (no change) so, OI decrease O (no change) 6.42 atm O f increase H,0 8.98 atm O f…