Consider the following reaction at equilibrium at 400 K: 2SO2(g) + O2(g)  ⇌  2SO3(g)                      K = 15.0 If the partial pressures of SO2(g) and O2(g) are 0.23 atm and 0.35 atm, respectively, then what is the partial pressure of SO3(g)?

7. Given the reaction, N2 (g) + O2 (g) = 2 NO (g), Ke = 2.5 x 103 at 2130°C, decide whether the following mixture is at equilibrium or if a net forward or reverse reaction will occur. [NO] = 0.0050 M, JO2] = 0.25 M, and [N2] = 0.020 M.

Consider the following reaction:2SO3(g) 2SO2(g) + O2(g)If 8.04×10-2 moles of SO3, 0.396 moles of SO2, and 0.261 moles of O2 are at equilibrium in a 19.8 L container at 1.31×103 K, the value of the equilibrium constant, Kp, is

A mixture of hydrogen, nitrogen, and ammonia is brought to equilibrium at 25 °C. Analysis of the mixture reveals the following concentrations: [H2(g)] = 0.00092: [N2(g)] = 0.981; [NH3(g)] = 0.523. What is the value of Kc at this temperature for the following equilibrium? 3H2(g) + N2(g) 2 2NH3(g) Select one: a. 2.8 x 10-9 O b. 3.6 x 108 O c. 5.7 x 102 O d. 1.7 x 10-3

The following reaction can be used to make H2 for the synthesis of ammonia from the greenhouse gases carbon dioxide and methane: CH4 (g) + CO2 (g) ⇌ 2 CO (g) + 2 H2 (g) At 1200. K, Kp = 3.548 × 106. What is the partial pressure of CH4 at equilibrium when 10.00 atm of CH4 reacts with 15.00 atm of CO2 at 1200. K? Use small x approximation and calculate the percent error

At 900 K, the following reaction has Kp = 0.345: 2 SO2(g) + O2(g) ⇋ 2 SO3(g). In an equilibrium mixture, the partial pressure of SO2 and O2 are 0.135 atm and 0.455 atm, respectively. What is the equilibrium partial pressure of SO3 in the mixture?

Initially, 2.0 moles of N2(g) and 4.0 moles of H2(g) were added to a 1.0-liter container and the reaction below then occurred. The equilibrium concentration of NH3(g) = 0.55 M at 700.°C. The value for Kc at 700.°C for the formation of ammonia is: 3H2(g) + N2(g) ⇌ 2NH3(g) a) 1.0 x 10^-1 b) 5.5 x 10^-2 c) 5.5 x 10^-3 d) 3.0 x 10^-1 e) The correct answer was not initially available

Consider the equilibrium system below, 2C2H6(g)   +   7O2(g)   ⇌   4CO2(g)   +   6H2O(g)         ∆H = -3120 kJ How will the amount of ethane (C2H6) at equilibrium be affected by: decreasing the temperature? decrease, increase, no effect decreasing the volume of the container at constant temperature? decrease, increase, no effect