36) At a certain temperature a reaction has K = 2.06 x 101. If all four...
At a certain temperature K = 0.500 for the following reaction: SO3 (g) + NO (g) ⇌ NO2 (g) + SO2 (g) If 0.200 mol of SO3 and 0.200 mol of NO are placed in a 2.000 L container and allowed to come to equilibrium, what will be the concentration of SO2?
please explain! thank you! 23) (5 pts) For the following reaction: SO2 (g)+ NO2 (g) SO3(g) + NO (g) given that the initial concentrations of SO2 and NO2 are 0.1 M, the initial concentrations of S03 and NO are 0.15 M, and that K 3.5, Calculate the concentration of all the gases at equilibrium. (Show work, correct units, use back if need be) IS
The reaction and equilibrium constant are provided. 2 SO2(g) + O2(g) 92 SO3(g) K = 5.8 x 103 Which direction will the reaction proceed if [502] = 0.015 M. [02] = 0.010 Mand (SO3) = 0.200 M? no shift shifts to make more product shifts to make more reactant
At 550 K, the reaction- SO2(g) + NO2(g) ⇌ SO3(g) + NO(g) has Kc = 770. If 0.496 moles of SO3 and 0.496 moles of NO are placed in a 5.00-L container at 550 K, what is the concentration of SO3 at equilibrium? A) 4.3 M B) 0.096 M C) 0.099 M D) 17 M E) 0.025 M
If the value of Ke for the reaction below is 3.45 at 298 K, what is the equilibrium concentration of the both products at 298 K if initially the reactants are both at 0.25 M? SO2(g) + NO2 (g) <> NO(g) + SO3 (8) 1.86 0.302 0.162 0.464
At a particular temperature, K = 3.75 for the reaction: SO2(g) + NO2(g) SO3(g) + NO(g). If all four gases had initial concentrations of 0.250 M, calculate the equilibrium concentrations of the gases.
1. At a particular temperature, K = 2.50 for the reaction: SO2 (g) + NO2 (g) ⇄ SO3 (g) + NO (g). If all four gases had initial concentrations of 1.00 M, calculate the equilibrium concentrations of SO2. 2. At a particular temperature, Kp = 0.25 for the reaction: N2O4 (g) ⇄ 2 NO2 (g). A flask containing only N2O4 at an initial pressure of 4.5 atm is allowed to reach equilibrium. a. Calculate the equilibrium partial pressure of N2O4....
Consider the following reaction where K. = 83.3 at 500 K: PC13(g) + Cl2(g) = PC15(8) A reaction mixture was found to contain 2.76x10-2 moles of PC13(g), 4.46x10-2 moles of Cl2(g) and 0.133 moles of PC13(g), in a 1.00 Liter container. Indicate True (T) or False (F) for each of the following: (- 1. In order to reach equilibrium PC15(g) must be consumed. 2. In order to reach equilibrium K, must increase. 3. In order to reach equilibrium PC1z must...
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.
12. (10 pts) At 25 °C, K. = 3.75 for the reaction SO2(g) + NO2(g) = SO3(g) + NO(g). Calculate the concentrations of all species at equilibrium, when the initial concentrations are all 0.800 M and equilibrium established. 13. (10 pts) Calculate the pH of a 0.10 M NaNO, solution (K, -4.5 x 10" for HNO2).