chemical engineer is studying the following reaction: BF3(aq)+NH3(aq) → BF3NH3(aq) At the temperature the engineer picks, the equilibrium constant K for this reaction is 0.61. The engineer charges ("fills") three reaction vessels with boron trifluoride and ammonia, 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 concentration expected change in concentration A BF 3 NH₂ 0.98 M Of increase ↓ decrease O(no change) 0.84 M O↑ increase Odecrease BF, NH₂ 0.50 M O↑ increase O decrease (no change) O(no change) BF3 1.42 M O increase ↓ decrease O(no change) B NH3 1.28 M O↑ increase ↓ decrease O(no change) BF3NH3 0.06 M O↑ increase Odecrease (no change) BF3 0.54 M O↑ increase Odecrease C NH₂ 0.40 M ↑ increase BF3NH3 0.94 M O↑ increase O↓ decrease O decrease (no change) O(no change) (no change)

Consider the reaction H2(g) + I2(g) → 2 HI(g). It is reported that an equilibrium mixture of this reaction system contains the following concentrations of the reacting species: Species Concentration (M) H2 1.18 x 10-2 I2 1.2 x 10-3 HI 2.59 x 10-2 Given this information, the equilibrium constant for this reaction may be calculated to have a value of:

A chem gineer is studying the following reaclon! HCN(aq)+NH,(aq) - CN (aq)+NH,(aq) At the temperature the engineer picks, the equilibrium constant K for this reaction is 0.99. The engineer charges ("fills") four reaction vessels with hydrogen cyanide and ammonia, 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 concentration expected change in concentration HCN 0.84 M O t increase OI decrease O (no change) NH, 1.00 M O t increase O, decrease O (no change) CN 0.42 M O 1 increase O. decrease O (no change) NH, 0.33 M O t increase O, decrease O (no change) HCN 1.01 M O t increase O. decrease O (no change) NH, 1.17 M O t increase O. decrease O (no change) CN 0.25 NM M t increase O. decrease O (no change) NH. 0.16 MM O t increase O.…

A chemical engineer is studying the following reaction: HCH3CO2(aq)+CH3NH2(aq) → CH3CO2(aq) + CH3NH3(aq) At the temperature the engineer picks, the equilibrium constant K for this reaction is 0.54. The engineer charges ("fills") four reaction vessels with acetic acid and methylamine, 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 compound concentration expected change in concentration HCH,CO₂ 1.01 M O↑ increase CH3NH2 1.22 M O decrease O↑ increase O decrease O (no change) O (no change) A CH,CO, 0.64 M O↑ increase O decrease O (no change) CH, NH3 1.04 M O ↑ increase O decrease O (no change) HCH CO₂ 0.33 M O↑ increase O decrease O(no change) CHÍNH, 0.50 M O↑ increase O decrease O (no change) B CH,CO, 1.01 M O increase O decrease O (no…

O KINETICS AND EQUILIBRIUM Using the small x approximation to solve equilibrium problems A chemist is studying the following equilibirum, which has the given equilibrium constant at a certain temperature: 2 NO(g) + Cl,(g) 2 NOCI(g) K,=2. x 107 He fills a reaction vessel at this temperature with 8.0 atm of nitrogen monoxide gas and 9.7 atm of chlorine gas. Use this data to answer the guestions in the table below. O yes Can you predict the equilibrium pressure of NOCI, using only the tools available to you within ALEKS? O no If you said yes, then enter the equilibrium pressure of NOCI at right. Round your answer to 1 significant digit. atm II

A chemist is studying the following equilibirum, which has the given equilibrium constant at a certain temperature: 2 CH₂(g) C₂H₂(g) + 3H₂(g) K₂=2.x10-5 P He fills a reaction vessel at this temperature with 15. atm of methane gas. Use this data to answer the questions in the table below. Can you predict the equilibrium pressure of C₂H₂, using only the tools available to you within ALEKS? If you said yes, then enter the equilibrium pressure of C₂H₂ at right. Round your answer to 1 significant digit. yes no atm ☐ x10 X ?

Ammonia will decompose into nitrogen and hydrogen at high temperature. An industrial chemist studying this reaction fills a 200. mL flask with 1.1 atm of ammonia gas, and when the mixture has come to equilibrium measures the partial pressure of hydrogen gas to be 1.2 atm. Calculate the pressure equilibrium constant for the decomposition of ammonia at the final temperature of the mixture. Round your answer to 2 significant digits. K = 0 P X Ś

Given the following reaction, the equilibrium constant, and the initial concentrations; answer the four bullet questions. 2 NO2 (g) - 2 NO (g) + O2 (g) Kc = 1.56 x 10-10 Initial Species Concentration (M) NO2 5.62 x 10-10 NO 3.99 x 10-16 O2 9.35 x 10-3 • Set up the equilibrium expression, and calculate the reaction quotient (Q). Note: ^ means "to the" Q = [ Select ] • How does Q compare to K? Q is [ Select]

A chemist is studying the following equilibirum, which has the given equilibrium constant at a certain temperature: 2 CH4 (g) 3H₂(g) + C₂H₂ (g) K₂=9. × 10-10 He fills a reaction vessel at this temperature with 5.0 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 atm X S ?

A chemical engineer is studying the following reaction: HCH;CO,(aq)+CH,NH,(aq) → CH;CO,(aq)+CH,NH,(2q) At the temperature the engineer picks, the equilibrium constant K, for this reaction is 1.6. The engineer charges ("fills") four reaction vessels with acetic acid and methylamine, 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 expected change in cor concentration concentration vessel HCH,CO, 0.96 M O T increase OI decrease O (no change) CH, NH, 0.88 M O f increase OI decrease O (no change) A CH,Co, 0.54 M O f increase OI decrease O (no change) CH,NH, 0.45 M O f increase OI decrease O (no change) HCH, CO, 0.88 M f increase OI decrease O (no change) CH,NH, 0.77 M O f increase OI decrease O (no change) B CH, Co, 1.09 M O increase OI…