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.
At a particular temperature, K = 3.75 for the reaction: SO2(g) + NO2(g) SO3(g) +...
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....
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).
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).
How is this solved using the method of succesive approximations? Q13. At a particular temperature, K = 3.75 for the reaction: SO2(g) + NO2(g) = SO3(g) + NO(9) If sulfur dioxide and nitrogen dioxide initially were put into a container with initial concentrations of 0.800M, what are the equilibrium concentrations of all four gases?
The reaction NO2(g) + SO2(g) ⇌NO (g) + SO3(g) has a Kc =10 under some conditions. If the initial concentrations of both NO2 and SO2 are 0.5 M, then calculate the equilibrium concentrations of all four species. [NO2]eq= __________ [SO2]eq= __________ [NO]eq= __________ [SO3]eq= _________
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
At some temperature, the value of the equilibrium constant for the reaction: SO2 (g) + NO2(g) ↔ SO3(g) + NO(g) has the value K = 0.640. If all four gases are placed into a container, each with an initial partial pressure of 1.25 atm, calculate the equilibriuym partial pressure (in atm) of SO3(g)
Name: (print clearly) 12. (10 pts) At 25 °C, K. - 3.75 for the reaction SO2(g) + NO2(g) SO(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 NaNO2 solution (K. - 4.5 x 104 for HNO.).
36) At a certain temperature a reaction has K = 2.06 x 101. If all four gases have an initial concentration of 0.800M, what are the equilibrium concentrations? x = change in concentration. Choose all the correct answers. SO3 (g) + NO (g) <--> SO2 (g) + NO2 (g) (Select 6)(6pts) O [SO3) = [NO] = 1.101 M x=0.454 O Q = 1.0 [SO2] = [NO2] = 0.499 M OK=[SO3][NOJ/ [S02] - [NO2] [SO3] = [NO) = 0.499 M O...
5 At some temperature, the value of the equilibrium constant for the reaction: SO2 (g) + NO2(g) →→ SO3(g) + NO(g) has the value K = 0.640. If all four gases are placed into a container, each with an initial partial pressure of 1.25 atm, calculate the equilibriuym partial pressure (in atm) of SO3(g) W AM