24. A mixture of O2(g) and O3(g) is present at equilibrium in a rigid container at 152 torr and 125° C. The density of the gaseous mixture is 0.228 g/L. Calculate Kp at 125° C for the reaction 3O2(g) 2O3(g)
24. A mixture of O2(g) and O3(g) is present at equilibrium in a rigid container at...
1. 2O3(g)↔ 3O2(g) ; if 10.0g of O2 is at equilibrium with 7.50g of O3 calculate Kp if the total pressure is 1.10atm. A. 2.94 B. 0.499 C. 0.339 ^ I submitted this question already but the answer was wrong, I worked through it and still couldn't find one of these options. Suggestions? 2. For: N2(g) + O2(g) ↔ 2NO(g) 0.500M O2 and 0.750M N2 is allowed to reach equilibrium. Kc = 1.00 x 10-1. Calculate equilibrium concentration of N2...
46.1 g of ethanol (C2H5OH) is burnt in a rigid 5.00 L container resulting a mixture of gaseous products according to the reaction equation: C2H5OH(g) + 3O2(g) -> 2CO2(g) + 3H2O(g) Calculate the total pressure in the reaction vessel at 200 °C. (A) 1660 kPa (B) 3930 kPa (C) 3.93 x10^6 kPa (D) 38.8 kPa (E) 787 kPa
Given the following data: 2O3(g) 3O2(g) -427 kJ O2(g) 2O(g) 495 kJ NO(g) + O3(g) NO2(g) + O2 -199kJ Calculate (in kJ) for the reaction: NO(g) + O(g) NO2(g)
Be sure to answer all parts. A) Calculate Kp for the following equilibrium: 3 O2(g) ⇌ 2 O3(g) Kc =1.8 × 10 −56 at 450 K __× 10__ B) Gaseous ammonia was introduced into a sealed container and heated to a certain temperature: 2 NH3(g) ⇌ N2(g) + 3 H2(g) At equilibrium, [NH3] = 0.0233 M, [N2] = 0.119 M, and [H2] = 0.369 M. Calculate Kc for the reaction at this temperature. Kc = __
For the following reaction, if the initial [O3] = 0.50 M, and the equilibrium [O2] = 0.60 M, what is the value of Kc? 2 O3(g) ⇄ 3O2(g)
Assume the reaction 3 O2(g) <===> 2 O3(g) (Delta H° =285 kJ/mol) is at equilibrium. What effect will each of the following have (explain each)? a) adding more O2 b) adding more O3 c) removing O3 d) increasing pressure in the container e) adding an inert gas f) increasing the temperature in the container
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.
A rigid vessel containing only NO2 (g) is heated to 337 °C and allowed to come to equilibrium according to the following reaction: 2 NO2 (g) 22 NO(g) + O2 (g) The density of theresulting mixture is measured to be 0.520 g/L at a total pressure of 0.750 atm. What is the value of Kp? A) 0.13 atm B) 7.8 atm C) 0.65 atm D) 1.5 atm E) 1.3 atm
i need 2,3,4,5,and 6. 2. (6 Pts) Write the equilibrium expression, Kp, for the reactions in problem 1. 3. (8 Pts) At 127°C, Kc = 2.6 x 10-5 for the reaction: 2 NH3(g) + N2(g) + 3 H2(g) Calculate Kp at this temperature. 4. (10 Pts) A 1.00-L flask was filled with 2.00 mol gaseous SO2 and 2.00 mol gaseous NO, and heated. After equilibrium was reached, it was found that 1.30 mol gaseous NO was present. Assume that the...
A reaction vessel contains an equilibrium mixture of SO2, O2,, and SO3. The reaction proceeds such that: 2SO2 (g) + O2 (g) ----> <---- 2SO3 (g) The partial pressures at equilibrium are Pso2=0.001111 atm PO2 = 0.002728 atm PSO3 =0.0166 Calculate the Kp for the reaction.