Consider the system at 25.0°C A(g) + 2B(g) + C(g) = 2D(g) At time zero, only A, B and C are present in a sealed container. The reaction reaches equilibrium 10 minutes after the reaction is initiated. The partial pressures of A, B, C and D are written as FA, PB, Pc and PD. At equilibrium, Q is K. More information required K for the forward reaction is K for More information required the reverse reaction. PA at 5 min is PA at 7 min. More information required After the system is at equilibrium, more of gas B is added. After the system returns back to More information required equilibrium, K before the addition of B is K after the addition of B. Pp at 11 min is Pp at 12 min. More information required Pc at 10 min is Pc at 9 min. More information required

Consider the following reaction initially at equilibrium in a fixed container at 25 °C: P4(s) + 5 O₂(g) = P4O10(s) If Ne(g) is introduced into the vessel, keeping the volume constant, such that the total pressure of the vessel increases, the rate of the forward reaction will and the system will If the volume of the container is cut in half, the rate of the forward reaction will and the system will - -- -- 11 V When the temperature is increased, the moles of O₂(g) increase. Is the forward reaction endotherm Save 1. Submit an

The equilibrium constant Kp for the reaction CCl4(g) —> C(s) + 2Cl2(g) at 700˚C is 0.76. Determine the initial pressure of carbon tetrachloride that will produce an equilibrium pressure of 1.5 atm for Cl2 at 700˚C. (Since C is a solid it can be left out of the ICE chart.)

Phosphine gas (PH3), decomposes by the reaction shown below.  A total pressure of 0.64 atm of pure phosphine gas was placed in a sealed 1.00-L flask at 298 K. After equilibrium was attained, the total pressure inside the flask was found to be 0.93 atm. Calculate the mass of solid phosphorous in the flask. PH3(g)   <-->   P(s)   +   3 H2(g)