particular temperature. A 2. For the reaction SO2C12(g) SO2(g) Cl2(g), Ke 0.011 at a + 2.00...
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....
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 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)
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
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
At a particular temperature, Kp-0.39 for the reaction below. N204(g) 2 NO2(g) (a) A flask containing only N204 at an initial pressure of 4.8 atm is allowed to reach equilibrium. Calculate the equilibrium partial pressures of the gases. N2O4 NO2 atm (b) A flask containing only NO2 at an initial pressure of 9.6 atm is allowed to reach equilibrium. Calculate the equilibrium partial pressures of the gases. No2 (e) From your answers to parts (e) and (b), does it matter...
The reaction 2 HI(g) + H2(g) + (x) has ke=0.020 at a certain temperature. If you nil a flask with 1.50 MHI. 2.50 MHz, and 3.00 M12, which statement below is true? Q-5.00 and the reaction will proceed toward reactants to reach equilibrium Q -3.33 and the reaction will proceed toward reactants to reach equilibrium 0-5.00 and the reaction will proceed toward products to reach equilibrium Q-3.33 and the reaction will proceed toward products to reach equilibrium Qc-ke and the...
consider the following reaction: SO2Cl2(g)⇌SO2(g)+Cl2(g) At a given point in a reaction, [SO2Cl2] = 0.12 M, [Cl2] = 0.16 M and [SO2] = 0.050 M. Kc = 0.078. Determine if the following system is at equilibrium. If not, in which direction will the system need to shift to reach equilibrium?
5. 2.00 mol each of SO2 and NO2 are introduced into a 1.00 L reactor at 300°C where Kp = 3.4. SO2(g) + NO2(g) <=> SO3(g) + NO(g) a) Give the general expression for K, for this system in terms of the concentrations ci b) Give the general expression for Kp for this system in terms of the partial pressures Pi. c) Assuming that the gases all behave ideally what is the relationship between K, and Kp? d) What is...
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.