Consider the following reaction: A2 + 2B+2 AB The initial concentrations are [A2] = 0.69OM and [B] = 0.384M. The reaction proceeds to equilibrium where [B] = 0.0281 M. Determine the value of the equilibrium constant.
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- 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…9a Please help me with the brief solution and answer, thank youGiven this equilibrium 2A(g)+3B———C(g)+4D+ energy Discuss what happens to this equilibrium if the temperature increases while the pressure is held constant. Make sure to include a discussion of rates of the forward and reverse reactions as well as changes in the concentrations of A, B, C and D.
- 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…A chemical engineer is studying the following reaction: N₂(g) + 3H₂(g) → 2 NH3(g) At the temperature the engineer picks, the equilibrium constant K for this reaction is 0.018. The engineer charges ("fills") three reaction vessels with nitrogen and hydrogen, 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 N₂ 11.46 atm ↑ increase ↓decrease (no change) H, 18.35 atm A ↑ increase ↓ decrease (no change) NH3 32.54 atm ↑ increase (no change) N₂ 10.77 atm ↑ increase ↓ decrease ↓decrease ↓decrease decrease B H₂ 16.30 atm (no change) (no change) (no change) ↑ increase 33.91 atm ↑ increase NH3 N₂₂ 11.20 atm ↑ increase ↓ decrease (no change) H₂ 17.58 atm с ↑ increase ↓decrease (no change) NH₂ 33.05 atm ↑…Bromine monochloride is synthesized using the reaction Br₂ (g) + Cl₂(g) = 2 BrCl(g) Kp = 1.1 x 10-4 at 150 K A 208.0 L flask initially contains 0.953 kg of Br₂ and 1.184 kg of Cl₂. Calculate the mass of BrCl, in grams, that is present in the reaction mixture at equilibrium. Assume ideal gas behavior. mass of BrCl: What is the percent yield of BrCl? percent yield: 6.D g %
- A chemical engineer is studying the following reaction: N₂(g) + 3H₂(g) → 2 NH3(g) At the temperature the engineer picks, the equilibrium constant K for this reaction is 0.018. The engineer charges ("fills") three reaction vessels with nitrogen and hydrogen, 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 N₂ 11.46 atm ↑ increase ↓ decrease (no change) A H₂ 18.35 atm ↑ increase ↓ decrease (no change) NH3 32.54 atm ↑ increase ↓decrease (no change) N2₂ 10.77 atm ↑ increase B H₂ 16.30 atm ↑ increase ↓decrease decrease ↓decrease (no change) (no change) (no change) (no change) NH₂ 33.91 atm O ↑ increase N₂ 11.20 atm ↑ increase C H₂ 17.58 atm O ↑ increase ↓ decrease ↓decrease ↓decrease (no change) NH3…Assume the following reaction system: H2 S(g) + Ci2(g) = S(s) + 2HCI(g) has arrived at a point of equilibrium. Predict how each of the following adjustments will affect the position of the object. equilibrium. Determine whether the equilibrium will shift to the right. to the left, or not at all (No effect). a. The system is supplemented with more chlorine gas. b. The system's sulfur content is reduced by half. C. An "acid scrubber" is placed to the container, which reacts with hydrochloric acid to remove it from the system. d. The activation energy is split in half thanks to a very efficient catalyst.Consider the reaction 2 A + B <=> 3C + D. 3.00 moles A and 2.00 moles B was placed in a 2.00 L flask and allowed to reach equilibrium. At equilibrium the concentration of D was 0.500 M. Calculate Kc for this reaction.
- 3. Given the chemical reaction A(aq) + 2B(aq) → C(aq) + 3D(aq) Initially, you have 2 moles of A and 3 moles of B dissolved in a total volume of 3 L. a. X moles of A reacted, and the solution reached equilibrium. Solve for the End state in term of x b. Write down the expression of the equilibrium constant (Keq) in term of x and volume.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 compound concentration expected change in concentration vessel HCH;CO, 1.18 M f increase I decrease (no change) CH, NH, 0.97 M f increase OI decrease O (no change) A CH,CO, 0.39 M f increase O I decrease (no change) + CH,NH, 0.39 M f increase Ot decrease (no change) HCH,CO, 1.15 M f increase OI decrease O (no change) CH,NH, 0.88 M t increase I decrease (no change) В CH,CO, 0.86 M f increase OI decrease (no change) CH,NH,…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…