10. (4 pts) The reaction: SO2Cl2(g)- SO2(g ) + Cl (g) is first order with respect...
Consider the reaction: SO2Cl2(g)⇌SO2(g)+Cl2(g) A reaction mixture is made containing an initial [SO2Cl2] of 0.024 M . At equilibrium, [Cl2]= 1.3×10−2 M . Calculate the value of the equilibrium constant (Kc)
Consider the equilibrium between SO2Cl2, SO2 and Cl2. SO2Cl2(g) <-->SO2(g) + Cl2(g) K = 0.552 at 412 K The reaction is allowed to reach equilibrium in a 6.30-L flask. At equilibrium, [SO2Cl2] = 0.142 M, [SO2] = 0.279 M and [Cl2] = 0.279 M. (a) The equilibrium mixture is transferred to a 12.6-L flask. In which direction will the reaction proceed to reach equilibrium? _________to the rightto the left (b) Calculate the new equilibrium concentrations that result when the equilibrium...
Consider the reaction: SO2Cl2(g) SO2(g) + Cl2(g) Kc = 2.99 x 10-7 (at 227oC) A reaction mixture initially contains 0.175 M SO2Cl2 and no SO2 and Cl2. What is the equilibrium concentration of Cl2 at this temperature (227oC)? Use the assumption that x is small compared to the initial concentration of reactant.
Consider the reaction: SO2Cl2(g) SO2(g) + Cl2(g) A reaction mixture contains an initial concentration of [SO2Cl2] = 0.020M. At equilibrium, [Cl2] = 1.2 x 10-2 M. Calculate the value of Kc.
4) If the reaction SO2Cl2 → SO2 + Cl2 is first-order reaction. At 230oC, k = 0.125 hr-1. If the initial concentration of SO2Cl2 is 0.250 M, what is the concentration after 7.6 hours? How long will it take for the concentration of SO2Cl2 to drop to 0.0651 M? What is the half-life for this first order reaction?
Sulfuryl chloride decomposes to sulfur dioxide and chlorine in a 2.0 L container SO2Cl2(g) 2 SO2(g) + Cl2(g) Ke is 0.045 at 648 K. A 0.1466 mol sample is allowed to decompose. Calculate the equilibrium concentrations of each species. (7 pts) ording to the
The gas phase reaction: SO2Cl2(g) → Cl2(g) + SO2(g) is first order in SO2Cl2(g) and has a first order rate constant of 0.0462 min-1. How long will it take for [SO2Cl2] to decrease from 0.500 M to 0.0100 M? 84.7 min 1.70 min 38.8 min 2.35 min
1) For the following reaction: SO2Cl2(g)<-> SO2(g) + Cl2 (g) Kp=2.91x10^3 at 298K In the reaction at equilibrium, the partial pressure of SO2 is 137 torr and that of CL2 is 285 torr. The partial pressure of SO2Cl2 is [x]torr. 2) For the following reaction:NH4HS(s)<->NH3(g) + H2S (g) Kc=8.5x10^-3 At any given point the reaction mixture has solid NH4HS, NH3 at 0.166M and H2S at 0.166M. a) Is the reaction at equilibrium? b)Will more of the solid form, or will...
Consider the following reaction: SO2Cl2(g)⇌SO2(g)+Cl2(g) A reaction mixture is made containing an initial [SO2Cl2] of 2.4×10−2 M . At equilibrium, [Cl2]= 1.0×10−2 M . Calculate the value of the equilibrium constant (Kc).
The reaction SO2Cl2(g)→SO2(g)+Cl2(g) is first order in SO2Cl2. Using the following kinetic data, determine the magnitude of the first-order rate constant: Time (s) Pressure SO2Cl2(atm) 0 1.000 2500 0.947 5000 0.895 7500 0.848 10000 0.803 k= s−1