Rate of formation of SO3 according to the reaction 2SO2+O2→2SO3is1.6×10−3kgmin−1. Hence rate at which SO2 reacts is:

For the reaction system: 2SO2(g) + O2(g)  ⇋   2SO3(g)the equilibrium concentrations are: [SO3] = 0.150 M; [SO2] = 0.940M; [O2] = 0.430MCalculate the value of K for the reactionQuestion 5Select one:a.16.9b.0.16c.2.7d.0.0590e.0.37

A chemistry graduate student is studying the rate of this reaction:→2SO3g+2SO2gO2gShe fills a reaction vessel with SO3 and measures its concentration as the reaction proceeds:time(seconds) SO30 0.0600M10. 0.0232M20. 0.0144M30. 0.0104M40. 0.00818MUse this data to answer the following questions.Write the rate law for this reaction. rate =k Calculate the value of the rate constant k.Round your answer to 2 significant digits. Also be sure your answer has the correct unit symbol. =k

Consider the equilibrium reaction represented by the equation: 2SO2(g) + O2(g) ⇌ 2SO3(g) ∆H = - 197 kJmol-1. At equilibrium, increase in the total pressure of the system brings aboutA. decrease in rate of the reaction of the systemB. decrease in temperature of the systemC. increase in temperature of SO3D. increase in concentration of SO2

The equilibrium constant, KC, for the following reaction is 280 at 1,000 K.2SO2(g) + O2(g) ⇌ 2SO3(g)If [SO2]eq = 0.80 M and [O2]eq = 0.35 M, then [SO3]eq = 6.2 × 10-27.9262.72792 M.

An equilibrium mixture of O2, SO3, and SO2 contain equal concentrations of SO2 and SO3. Calculate the concentration of SO3 if the Keq = 220. 2SO2 (g) + O2 (g) → 2SO3 (g)