A chemical engineer is studying the following reaction: HCH;CO,(aq)+CH,NH,(aq) → - CH;CO,(aq)+CH;NH(aq) At the temperature the engineer picks, the equilibrium constant K, for this reaction is 0.73. The engineer charges ("fills") four reaction vessels with acetic acid and methylamine, 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 HCH,CO, 1.18 M Ot increase O I decrease O (no change) CH;NH, 0.97 M O t increase O ! decrease O (no change) A CH,Co, O t increase 0.39 M O I decrease O (no change) CH, NH, 0.39 M O t increase I decrease (no change) HCH,CO, 1.15 M O t increase O I decrease (no change) CH,NH, 0,88 M O t increase O I decrease (no change) B CH,CO, 0.86 M O tincrease O I decrease (no change) CH,NH, 0.86 M O t increase O I decrease (no change) HCH,CO, 1.33 M O t increase O I decrease O (no change) CH,NH, O I decrease O (no change) 1.12 M O increase CH, CO, 0.24 M O t increase O I decrease O (no change) CH,NH, 0.24 M O t increase O I decrease O (no change)

Ammonia has been studied as an alternative "clean" fuel for internal combustion engines, since its reaction with oxygen produces only nitrogen and water vapor, and in the liquid form it is easily transported. An industrial chemist studying this reaction fills a 25.0 L tank with 5.3 mol of ammonia gas and 2.4 mol of oxygen gas, and when the mixture has come to equilibrium measures the amount of nitrogen gas to be 1.4 mol. Calculate the concentration equilibrium constant for the combustion of ammonia at the final temperature of the mixture. Round your answer to 2 significant digits. K = -0 ☐ x10 G

Suppose a 500. mL flask is filled with 1.6 mol of Br,, 1.9 mol of OCl, and 1.7 mol of BrCl. The following reaction becomes possible: Br, (g) +OCl, (g) BROC1 (g) +BrC1(g) The equilibrium constant K for this reaction is 0.630 at the temperature of the flask. Calculate the equilibrium molarity of OCl,. Round your answer to two decimal places. | M

What can be said about the magnitude of the equilibrium constant in a reaction whose equilibrium lies far to the right? To the left?

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…

The following chemical reaction describes how carbonic acid is formed when carbon dioxide is combined with water; the following equation describes ocean acidification:    H2O(l) + CO2(g)⇋ H2CO3(aq)   Describe 2 actions people can take to prevent ocean acidification.  Relate both examples back to the ocean acidification chemical equation and explain how the action will reduce ocean acidification as a result of a shift in equilibrium.

Suppose a 250. mL flask is filled with 0.10 mol of Br,, 1.7 mol of OC1, and 0.20 mol of BrCl. The following reaction becomes possible: Br, (g) + OC1,(g) -BROC1 (g) + BrCl (g) The equilibrium constant K for this reaction is 0.343 at the temperature of the flask. Calculate the equilibrium molarity of Br,. Round your answer to two decimal places. | M

Hydrofluoric acid and water react to form fluoride anion and hydronium cation, like this: + HF(aq)+H,O(1)→F (aq)+H;O"(aq) At a certain temperature, a chemist finds that a 2.7 L reaction vessel containing an aqueous solution of hydrofluoric acid, water, fluoride anion, and hydronium cation at equilibrium has the following composition: compound amount HF 2.21 g H,0 857. g F 0.169 g H;O 0.141 g Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits. K = 0

Ammonia has been studied as an alternative "clean" fuel for internal combustion engines, since its reaction with oxygen produces only nitrogen and water vapor, and in the liquid form it is easily transported. An industrial chemist studying this reaction fills a 25.0 L tank with 1.5 mol of ammonia gas and 2.4 mol of oxygen gas, and when the mixture has come to equilibrium measures the amount of nitrogen gas to be 0.60 mol. Calculate the concentration equilibrium constant for the combustion of ammonia at the final temperature of the mixture. Round your answer to 2 significant digits. K_ = ] |x10 ?

A chemical engineer is studying the following reaction: HCN(aq)+NH3(aq) → CN (aq)+NH (aq) At the temperature the engineer picks, the equilibrium constant K, for this reaction is 0.91. 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 compound concentration expected change in concentration vessel HCN 0.64 M (O↑ increase O I decrease (no change) NH, 0.61 M O ↑ increase I decrease (no change) A CN 0.54 M ↑ increase O I decrease (no change) NH, 0.66 M O ↑ increase O Į decrease (no change) HCN 1.11 M O ↑ increase Į decrease (no change) NH, 1.08 M O ↑ increase O I decrease (no change) В CN 0.07 M O ↑ increase O Į decrease (no change) NHA 0.19 M O ↑ increase O I…