Consider the equilibrium reaction 2 A + B =4C Write the equation for the reverse reaction. reverse reaction: Write the equilibrium-constant expression in terms of [A], [B], and [C] for the reverse reaction.

A 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 1.3. 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 BF3 NH₂ 0.99 M O increase Odecrease O (no change) 0.72 M O increase O decrease O (no change) BF3NH3 0.92 M O increase O decrease O (no change) BF3 1.25 M O increase Odecrease O (no change) B NH₁ 0.91 M O↑ increase Odecrease O(no change) BF3NH3 1.48 M O increase Odecrease O (no change) BF 0.52 M O increase Odecrease O (no change) C NH, 0.25 M O↑ increase Odecrease O (no…

Consider the production of phosgene gas from carbon monoxide and chlorine gases which has an equilibrium constant of Kc = 3.36 at a certain temperature.  If the initial concentration of carbon monoxide is 0.430 M and that of chlorine gas is 0.229 M, what will the equilibrium concentration of Cl2 (g) be? CO (g) + Cl2 (g) <---. COCl2 (g)

Titanium(IV) chloride decomposes to form titanium and chlorine, like this: TICI (1)→ Ti(s)+2 Cl,(9) At a certain temperature, a chemist finds that a 7.9 L reaction vessel containing a mixture of titanium(IV) chloride, titanium, and chlorine at equilibrium has the following composition: compound amount TiCl4 2.46 g Ti 2.26 g Cl2 1.21 g Calculate the value of the equilibrium constant K for this reaction. Round your answer to 2 significant digits.