At 25°C, the equilibrium constant Kc for the following reaction is 7.9 x 10-4. A(aq) + B(aq) ⇄ C(aq) If the initial concentration of A is 0.200 M and of B is 0.300 M, what is the equilibrium concentration of C?

For the following reaction: A(aq) + B(aq) ⇌ 2 C(aq) Given the following information, what is the equilibrium concentration of C in mol L-1? Initial concentration of A = 1.108 mol L-1 Initial concentration of B = 1.108 mol L-1 Initial concentration of C = 0 mol L-1 K = 0.4 x 10-5

Choose the equilibrium constant expressions for the following reactions. a) 2SO2(g) + O2(g)  2SO3(g)      Keq =   b) CS2(g) + 4H2(g)   CH4(g) + 2H2S(g)                            Keq =

Consider the reaction:  4 A (g) + 3 B (g)   2 C (g)  +  5 E (g).   The reaction is initiated with 0.60 M in A, 0.45 M in B and 0.50 M in E.  At equilibrium, the value of  [A] = 0.36 M.  What is the equilibrium value of [E]?

Mercury and oxygen react to form mercury(II) oxide, like this: 2 Hg(1)+O2(g)→2 HgO(s) At a certain temperature, a chemist finds that a 7.0 L reaction vessel containing a mixture of mercury, oxygen, and mercury(II) oxide at equilibrium has the following composition: compound amount Hg 7.0 g O2 5.8 g HgO 16.5 g Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits. K_ = | x10

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…

A chem ngineer 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 1.1. C 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 A B C compound HCN NH3 CN NH4 HCN NH3 CN NH₁ HCN NH₂ CN NHA 4 concentration 0.28 M 0.12 M 1.05 M 0.94 M 0.67 M 0.51 M 0.66 M 0.55 M 0.31 M 0.15 M 1.02 M 0.91 M expected change in concentration ↑ increase ↑ increase ↑ increase ↑ increase ↑ increase ↑ increase ↑ increase ↑ increase ↑ increase ↑ increase ↑ increase ↑ increase ↓ decrease ↓decrease ↓ decrease 888888 ↓decrease ↓ decrease ↓decrease ↓ decrease ↓ decrease ↓decrease…

At a certain temperature the reaction CO2(g) + H2(g) ⇄ CO(g) + H2O(g) has Kc = 2.51. If 2.50 mol of carbon monoxide and 2.50 mol of water are placed in a 5.00 L vessel and equilibrium is established, what will be the concentration of carbon monoxide at equilibrium?

Ammonia and oxygen react to form nitrogen monoxide and water, like this: 4 NH3(9) + 5O2(g) → 4NO(g) + 6H,O(g) Also, a chemist finds that at a certain temperature the equilibrium mixture of ammonia, oxygen, nitrogen monoxide, and water has the following composition: compound concentration at equilibrium NH, 1.8M 1.6M NO 1.7M AH,0 1.9M Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits. C. K x10