The equilibrium constant, Kp, for the following reaction is 2.74 at 1150 K. 2SO3(g) 2SO2(g) + O2(g) If ΔH° for this reaction is 198 kJ, what is the value of Kp at 1270 K? Kp =
The equilibrium constant, Kp, for the following reaction is 2.74 at 1150 K. 2SO3(g) 2SO2(g) +...
The equilibrium constant, Kp, for the following reaction is 2.74 at 1150 K. 2SO3(g) 2SO2(g) + O2(g) If ΔH° for this reaction is 198 kJ, what is the value of Kp at 1260 K? Kp= ?
The equilibrium constant, Kp, for the following reaction is 2.74 at 1150 K. 2SO3(g) 2 25O2(g) + O2(g) If AH° for this reaction is 198 kJ, what is the value of K, at 1030 K? Kp = 1 The equilibrium constant, Kp, for the following reaction is 6.25 at 298 K. 2NO(g) + Brz(g) 2NOBr(g) If AHⓇ for this reaction is -16.1 kJ, what is the value of K, at 200 K? Kp =
At 900 K the following reaction has Kp=0.345: 2SO2(g)+O2(g)???2SO3(g) In an equilibrium mixture the partial pressures of SO2 and O2 are 0.150atm and 0.465atm , respectively. What is the equilibrium partial pressure of SO3 in the mixture?
Consider the following equilibrium reaction. 2SO2(g)+O2(g)↽−−⇀2SO3(g)Δ?=−198 kJ/mol Which characteristics of this reaction will be affected by a change in temperature? I. value of equilibrium constant II. equilibrium concentrations Or both
At 850 K, the equilibrium constant for the reaction 2SO2(g)+O2(g)↽−−⇀2SO3(g) is ?c=15. If the given concentrations of the three gases are mixed, predict in which direction the net reaction will proceed toward equilibrium.
At a given temperature, the equilibrium constant Kc for the reaction 2SO2(g)+O2(g)<==>2SO3(g) is 2.99x10^-3. What is the value of the equilibrium constant for each of the following reactions at that temperature? a. SO2(g)+ 1/2 O2(g)<==> SO3(g) b. 2SO3(g)<==>2SO2(g)+O2(g) c. SO3(g)<==> SO2(g)+ 1/2 O2(g)
Consider the following reaction where Kc = 34.5 at 1150 K: 2SO2(g) + O2(g) =2SO3(g) A reaction mixture was found to contain 4.39x10-2 moles of SO2(g), 4.28x10-2 moles of O2(g) and 4.23x10-2 moles of SO3(), in a 1.00 Liter container. Indicate True (T) or False (F) for each of the following: 1. In order to reach equilibrium SO3(g) must be consumed. 2. In order to reach equilibrium Kc must decrease. 3. In order to reach equilibrium SO2 must be consumed....
For the reaction: 2SO2(g) + O2(g) ⇄ 2SO3(g) At 650K, Kc = 345 and Kp = 6.47. What is ΔGo ? a) −10.1 kJ b) +31.6 kJ c) −31.6 kJ d) −311 J e) −99.7 J
The equilibrium constant for the reaction 2SO2(g) + O2(g) ⇌ 2SO3(g) is 7 × 103 at a certain temperature. If at equilibrium, [SO2] = 0.0451 M and [O2] = 0.078 M, what is the equilibrium [SO3]?
For the equilibrium reaction 2SO2(g) + O2(g) 2SO3(g), delta Hrxn = -198 kJ/mol. Which one of these factors would cause the equilibrium constent to increases? Decrease the temperature. Add SO2 gas Remove O2 gas Add a catalyst. None of these Consider this reaction at equilibrium If the volume of the system is compressed at constent temperature, what change will occure in the position of the equilibrium?