At 113 oC the equilibrium constant for the reaction: 2 HBr(g)  H2(g) + Br2(g) is KP = 1.81e-12. If the initial pressure of HBr is 0.00631 atm, what are the equilibrium partial pressures of HBr, H2, and Br2?

The equilibrium constant, Kp, for the following reaction is 9.52×10-2 at 350 K:CH4(g) + CCl4(g) 2CH2Cl2(g) Calculate the equilibrium partial pressures of all species when CH4 and CCl4, each at an intitial partial pressure of 0.997 atm, are introduced into an evacuated vessel at 350 K. PCH4 = atm PCCl4 = atm PCH2Cl2 = atm

1. At 900K, Kp = 0.345 for the following reaction, 2SO2(g) + O2(9) = 2SO3(g) ee ert grilcot In the equilibrium mixture, the partial pressure of SO2 is 0.165atm while that of O2 is 0.755atm. Calculate the equilibrium partial pressure of SO3 in the mixture. 2. For the reaction, co(9) H2(g) + CO2(9) 4 H2O(g) + oubo yd ateutbs meleya Kc is equal to 0.771 at 750°C. If 0.0100mol of H2 and 0.0100mol of CO2 were mixed in a liter container and allowed to react at 750°C, what will be the resulting equilibrium concentration of all substances? lomexe 1o

For the reaction: 24(g) +B(s)=2C(s) + D(g)Kp = 8210 At 250K in a 10.0L vessel, the known equilibrium values are follows: 0.030atm of A, 0.22mol of B, and 10.5mol of C. What is the equilibrium partial pressure of D ?