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 mixtur 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 C compound H₂ Cl₂2 HC1 H₂ CL₂ HCI H₂ Cl₂ 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 (O) ↑ increase O decrease ↓ O ↑ increase O decrease Ot increase O decrease O ↑ increase O decrease Ot increase ↑ O ↑ increase Ot increase Ot increase O † increase O decrease ↓ O decrease O decrease O decrease O decrease O (no change) O (no change) O (no change) O (no change) O (no change) O (no change) O (no change) O (no change) O (no change)

Chemical equilibrium is the reaction state when the concentrations of reactants and products remain constant over time. The reaction does not stop, but it reaches a dynamic equilibrium when the rates of the forward and reverse reactions become equal. A mixture of reactants and products in the equilibrium state is called an equilibrium mixture. Let's consider a general reversible reaction where AA and BB are the reactants and CC and DD are the products: aA+bB⇌cC+dD�A+�B⇌�C+�D   The concentrations in an equilibrium mixture are related by the equilibrium equation Kc=[C]c[D]d[A]a[B]b�c=[C]c[D]d[A]a[B]b where Kc�c is the equilibrium constant.   Part A The following pictures represent the equilibrium mixtures of five different chemical reactions. All the reactions proceed according to the general balanced chemical reaction A+B⇌ABA+B⇌AB Red spheres represent AA atoms, blue spheres are BB atoms, and red-blue clusters are ABAB molecules. Rank the reactions in order of increasing…

Answer with two decimal places, please!

A chemical engineer is studying the following reaction: CH,CH,NH,(aq)+HCl(aq) → Cl (aq)+CH,CH,NH;(aq) At the temperature the engineer picks, the equilibrium constant K¸ for this reaction is 0.92. The engineer charges ("fills") four reaction vessels with ethylamine and hydrogen chloride, 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 CH, CH,NH, 0.79 M f increase I decrease (no change) HCl 0.69 M f increase I decrease (no change) А Cl 0.62 M f increase I decrease (no change) CH,CH,NH, 0.81 M f increase I decrease O (no change) CH, CH,NH, 1.09 M f increase I decrease (no change) HCl 0.99 M f increase I decrease (no change)

Suppose a 500. mL flask is filled with 1.9 mol of O, and 1.8 mol of SO2. This reaction becomes possible: 2s0,(g) +0,(g) – 2so,(g) Complete the table below, so that it lists the initial molarity of each compound, the change in molarity of each compound due to the reaction, and the equilibrium molarity of each compound after the reaction has come to equilibrium. Use x to stand for the unknown change in the molarity of O,. You can leave out the M symbol for molarity. So, O2 initial 口 D. change equilibrium

Carbon monoxide is a colorless, odorless gas that binds irreversibly to hemoglobin in our blood, causing suffocation and death. Co is formed during incomplete combustion of carbon. One way to represent this equilibrium is: 2c0(g)=2 C(s) + 02(g) We could also write this reaction three other ways, listed below. The equilibrium constants for all of the reactions are related. Write the equilibrium constant for each new reaction in terms of K, the equilibrium constant for the reaction above. 1) C(s) + 1/2 02(g)=co(g) K = 2) 2 C(s) + 02(g) =2c0(g) K2 = %3D 3) CO(g) C(s) + 1/2 02(g) K3 = Drag and drop your selection from the following list to complete the answer: 1/K K1/2 (1/K)1/2

A chemical engineer is studying the following reaction: HCN(aq)+NH,(aq) → CN (aq)+NH(aq) At the temperature the engineer picks, the equilibrium constant K, for this reaction is 1.0. 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 0.06 M O f increase OI decrease O (no change) NH, 0.22 M f increase OI decrease (no change) A CN 0.97 M increase I decrease (no change) NH, 1.23 M f increase OI decrease O (no change) HCN 0.53 M f increase OI decrease (no change) NH, 0.69 M f increase O I decrease (no change) В CN 0.50 M t increase OI decrease O (no change) NH, 0.76 M f increase Ot decrease (no change)…

Methanol liquid burns readily in air. One way to represent this equilibrium is: 2 CH3ОН(1) + 3 02(9)+ 2 CO2(g) + 4 H20(g) We could also write this reaction three other ways, listed below. The equilibrium constants for all of the reactions are related. Write the equilibrium constant for each new reaction in terms of K, the equilibrium constant for the reaction above. 1) CНH3ОН(1) + 3/2 02(9)+ =cO2(g) + 2 H20(g) K1 = %D 2) 2 CO2(9) + 4 H20(g) 2 CH3ОН (1) + 3 02(9) K2 = 3) СO2(g) + 2 H20(g) еснзон (1) + 3/2 02(g) K3 : %3D Drag and drop your selection from the following list to complete the answer: к1/2 1/K (1/K)!/2

Chemistry

Suppose a 250. mL flask is filled with 1.5 mol of CO, 0.50 mol of H₂O and 1.2 mol of CO₂. The following reaction becomes possible: CO(g) +H₂O(g) CO₂(g) +H₂(g) The equilibrium constant K for this reaction is 0.503 at the temperature of the flask. Calculate the equilibrium molarity of CO. Round your answer to two decimal places. M ܢܢ X E 00 Ar