A mixture of 0.448 M Cl2 , 0.462 M F2 , and 0.833 M ClF is enclosed in a vessel and heated to 2500 K . Cl2(g)+F2(g)↽−−⇀2ClF(g)?c=20.0 at 2500 K Calculate the equilibrium concentration of each gas at 2500 K . [Cl2]. [F2], [ClF]

Phosphorus pentachloride decomposes according to the chemical equation PCI, (g) = PCI, (g) + Cl, (g) K. 1.80 at 250 °C A 0.1952 mol sample of PCl, (g) is injected into an empty 2.15 L reaction vessel held at 250 °C. Calculate the concentrations of PCl, (g) and PCl, (g) at equilibrium. [PCI,] = M [PCI,] = M

The equilibrium constant, Kc, for the following reaction is 55.6 at 698 K. H2(g)+I2(g) <-----> 2HI(g) Calculate the equilibrium concentrations of reactants and product when 0.301 moles of H2 and 0.301 moles of I2 are introduced into a 1.00 L vessel at 698 K. [H2] =       M [I2]   =     M [HI] =        M

A mixture of 0.5110 M CO and 0.3590 M Cl, is enclosed in a vessel and heated to 1000 K. CO(g) + Cl, (g)= COCI,(g) K. = 255.0 at 1000 K Calculate the equilibrium concentration of each gas at 1000 K. [CO] = M %3D [CI,] = M [COCI,] = M

At 400 K, an equilibrium mixture of H2, 12, and HI consists of 0.065 mol H2, 0.079 mol 12, and 0.13 mol HI in a 4.50-L flask. What is the value of K, for the following equilibrium? (R= 0.0821 L atm/(K • mol)) 2HI(g) = H2(g) + 12(8) 0.29 8.2 0.039 O 26 3.4

explain step by step

N2(g) +3H2(g) 2NH3 (g) what is the value of K. at 500 °C if the equilibrium concentrations are as follows: H2 = 0.50 M , N2] = 0.60 M , and [NH3] = 2.2 M ? Express the equilibrium constant to two significant figures. ? Ke =

The equilibrium constant, Kc, for the following reaction is 1.20\times 10 - 2 at 500 K. PCl5(g) PCl3(g) + Cl2(g) Calculate the equilibrium concentrations of reactant and products when 0.331 moles of PCl5(g) are introduced into a 1.00 L vessel at 500 K.