Comment if any problem
For the following reaction at 600 °C: 2502(g) + O2 (g) = 2SO3(g) Kc = 4.32...
Work the following problem using the algorithm we covered in class. Show your work by listing all the steps, Use Example 13.8 on page 706. For the following reaction at 600 °C: 2SO2 (g) + O2 (g) ⇌ 2SO3(g) Kc = 4.32 What are the equilibrium concentrations of all species in a mixture that was prepared with [SO3] = 0.500 M, [SO2] = 0 M, and [O2] = 0.350 M?
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 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.
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]?
A student ran the following reaction in the laboratory at 1185 K: 2SO2(g) + O2(g) 2SO3(g) When she introduced 8.07×10-2 moles of SO2(g) and 7.94×10-2 moles of O2(g) into a 1.00 liter container, she found the equilibrium concentration of O2(g) to be 5.86×10-2 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc=?
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....
Use the equilibrium constants for the following reactions at 700 °C 2SO2(g) + O2(g) 2SO3(g) K1 = 4.8 2NO(g) + O2(g) 2NO2(g) K2 = 16 to determine the equilibrium constant for the following reaction. SO 3( g) + NO( g) SO 2( g) + NO 2( 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 is equal to 5.00 at 1300 K for the reaction: 2502(g) + O2(g) = 2503(g) If initial concentrations are [SO2] = 10.8 M, [O2] = 0.45 M, and (SO3) = 16.2 M, the system is not at equilibrium and will remain in an unequilibrated state. not at equilibrium and will shift to the left to achieve an equilibrium state. O at equilibrium. not at equilibrium and will shift to the right to achieve an equilibrium state.