For the following reaction, K, = 0.262 at 1000°C: C(s) + 2 H2(g) = CH4(g) At equilibrium, Pa, is 1.22 atm and 1.35 g of carbon is present. What is the equilibrium partial pressure of CH4(g)? 0.390 atm 5.68 atm 0.997 atm 0.320 atm 0.624 atm None of these

The equilibrium system shown below was analyzed and the concentrations of H2(g), I2(g) and HI(g), were found, in mol/L, to be 4.2, 3.8, 1.6 respectively. The equilibrium constant must be? H2(g) + I2(g) <=====> 2HI(g) + 65 kJ

At 1000 K, a sample of pure NO₂ gas decomposes: 2 2NO₂(g) = 2NO(g) + O₂(g) The equilibrium constant Kp, is 158. Analysis shows that the partial pressure of O₂ is 0.41 atm at equilibrium. Part 1 of 2 What is the pressure of NO? Be sure your answer has the correct number of significant digits. Part 2 of 2 atm x10 atm X What is the pressure of NO₂? Be sure your answer has the correct number of significant digits. Ś x10

following equilibrium reaction at 160.00 °C. If 0.420 atm of H2O2(g) is initially present, calculate the equilibrium partial pressures of H2(g), O2(g), and H2O2(g).

Phosphorous pentachloride decomposes according to the reaction PCl5(g)↽−−⇀PCl3(g)+Cl2(g)PCl5⁢(g)⁢↽−−⇀⁢PCl3⁢(g)+Cl2⁢(g) A 13.1 gsample of PCl5 is added to a sealed 1.25 L flask and the reaction is allowed to come to equilibrium at a constant temperature. At equilibrium, 48.4% of the PCl5 remains. What is the equilibrium constant, Kc , for the reaction?

An evacuated reaction vessel is filled with 0.800 atm of N₂ and 1.681 atm of Br2. When equilibrium is established according to the reaction below, there are 1.425 atm of Br2 remaining in the vessel. What is the equilibrium partial pressure of NBr3? 2 NBr3 (g) = N₂ (g) + 3 Br2 (g)

An empty steel container is filled with 3.10 atm of H₂ and 3.10 atm of F2. The system is allowed to reach equilibrium. If Kp = 0.450 for the reaction below, what is the equilibrium partial pressure of HF? H₂ (g) + F₂ (g) → 2 HF (g)

Consider the following equilibrium system at 817 K. SO2 Cl2 (g) 2 SO2(g) + Cl2 (g) If an equilibrium mixture of the three gases at 817 K contains 1.60 x 10-3 M SO2 Cl2, 3.57 x 10-2 SO2, and 2.12 x 10-2 M Cl2, what is the value of the equilibrium constant К? M K =

Consider the equilibrium system below. For this reaction, Kp = 205. If the equilibrium partial pressure of Cl2 is 0.050 atm and the partial pressure of NOCl is 0.095 M what is the equilibrium partial pressure of NO?   2 NO (g) + Cl2 (g) <-> 2 NOCl (g)