2) For the equilibrium: 2 SO2(g) + O2(g) < => 2 503(g) Kp = 2.98 at...
2) For the equilibrium: 2 SO3(g) <=> O2(g) + 2 SO2(g) Kp = 0.269 at 625 °C What is Ke at this temperature? Kp = Kc[RT]An R = 0.08206 L-atm/mol K
2) For the equilibrium: 2 SO3(g) <=> 02(g) + 2 SO2(g) Kp = 0.269 at 625 °C What is Ke at this temperature? Kp = K[R R = 0.08206 L-atm/mol K (5pts)
For the equilibrium: 2 SO3(g) < = > O2(g) + 2 SO2(g) Kp = 0.269 at 625 oC What is Kc at this temperature? Kp = Kc[RT]Δn R = 0.08206 L-atm/mol K
how to solve this? Sulphur trioxide decomposes at high temperature in a sealed container: 2 SO3(g) <--> 2 SO2(g) + O2(g). Initially, the vessel is charged at 1000 K with SO3(g) at a partial pressure of 0.500 atm. At equilibrium the SO3 partial pressure is 0.200 atm. Calculate the value of Kp at 1000 K to 3 decimal places.
Given a chemical reaction below, 2502(g) + O2(g) = 2 503(8) Kc = 2.7 102 at 960K what is the value of K, for this reaction? (R = 0.08206 L'atm/mol K, K, = K (RT)An) 0 21 x 104 0.29 0.023 Question 9 1 pts The reaction system SO2(g) + NO2(g) = NO(g) + SO3(g) is at equilibrium. When NO2 is added to the container, the reaction shifts to Select] the partial pressure of SO2 [Select) , and the partial...
5. For the reaction... SO2 + O2 <=> SO3 If the equilibrium position shifts to the right, the concentration of O2 will (2 points) o remain constant increase Decrease
The equilibrium constant in terms of pressures, Kp, for the reaction of SO2 and O2 to form SO3 is 0.365 at 1.15×103 K: SO2(g) + O2(g) = 2SO3(g) A sample of SO3 is introduced into an evacuated container at 298 K and allowed to dissociate until its partial pressure reaches an equilibrium value of 0.867 atm. Calculate the equilibrium partial pressures of SO2 and O2 in the container. PSO2 = PO2 =
n = Products-react (gas only) cuent Kp = kelet Practice exercises: Give the K, expression and the value for the given reactions. 1. NO.(g) = 2 NO. (g) At equilibrium [N.O.]=18.6 torr, (NO )= 4.58 torr. 18. Eberl shin Ke=P(NO₂)² 7600 101024) Ko= 101024)2 To 70.096 P(N2O4) (0.006) 4.58 _60.C 760 2. A673B(g) = 2 C(g)+D At equilibrium P,034 atm, Pc-0.52 atm Ko - (0.32 - Kp = 6.88] 3. 250() + 0x0= 250,(g) At equilibrium (80.)- 14.5 mmHg (0.)-...
The equilibrium constant, Kp, for the following reaction is 2.74 at 1.15x103K. 2803(g) 22502(g) + O2(g) + If an equilibrium mixture of the three gases in a 10.9 L container at 1.15*10²K contains SO3 at a pressure of 1.77 atm and SO2 at a pressure of 0.926 atm, the equilibrium partial pressure of O2 is atm.
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...