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The equilibrium constant, K., for the following reaction is 1.20 10-2 at 500 K. PCI(8) =PC13(g)...
The equilibrium constant, Kc, for the following reaction is 83.3 at 500 K. PC13(g) + Cl2(g) = PC15(g) Calculate the equilibrium concentrations of reactant and products when 0.389 moles of PC13 and 0.389 moles of Cl2 are introduced into a 1.00 L vessel at 500 K [PC13] = [Cl] = [PC15] - The equilibrium constant, Kc, for the following reaction is 5.10x10-6 at 548 K. NH4Cl(s) NH3(g) + HCl(g) Calculate the equilibrium concentration of HCl when 0.467 moles of NHACI(S)...
The equilibrium constant, Kc, for the following reaction is 83.3 at 500 K. PCl3(g) + Cl2(g) = PCl5(g) Calculate the equilibrium concentrations of reactant and products when 0.249 moles of PCl3 and 0.249 moles of Cl2 are introduced into a 1.00 L vessel at 500 K. [PCl3] = M [Cl2] = M [PCl5] = M The equilibrium constant, Kc, for the following reaction is 1.80×10-2 at 698 K. 2HI(g) = H2(g) + I2(g) Calculate the equilibrium concentrations of reactant and...
a) The equilibrium constant, Kc, for the following reaction is 9.52×10-2at 350 K. CH4(g) + CCl4(g) -> 2 CH2Cl2(g) Calculate the equilibrium concentrations of reactants and product when 0.251 moles ofCH4and 0.251 moles of CCl4are introduced into a 1.00 L vessel at 350 K. [ CH4] = M [ CCl4] = M [ CH2Cl2] = M b) The equilibrium constant, Kc, for the following reaction is 1.20×10-2 at 500 K. PCl5(g) ->PCl3(g) + Cl2(g) Calculate the equilibrium concentrations of reactant...
The equilibrium constant, Kc, for the following reaction is 83.3 at 500 K. PCl3(g) + Cl2(g) ⇌ PCl5(g) Calculate the equilibrium concentrations of reactant and products when 0.253 moles of PCl3 and 0.253 moles of Cl2 are introduced into a 1.00 L vessel at 500 K. [PCl3] = ___ M [Cl2] = ___ M [PCl5] = ___M
9b. The equilibrium constant, Kc, for the following reaction is 83.3 at 500 K. PCl3(g) + Cl2(g) PCl5(g) Calculate the equilibrium concentrations of reactant and products when 0.560 moles of PCl3 and 0.560 moles of Cl2 are introduced into a 1.00 L vessel at 500 K. [PCl3] = M [Cl2] = M [PCl5] = M
The equilibrium constant, Kc, for the following reaction is 83.3 at 500 K. PCl3(g) + Cl2(g) -----> PCl5(g) Calculate the equilibrium concentrations of reactant and products when 0.504 moles of PCl3 and 0.504 moles of Cl2 are introduced into a 1.00 L vessel at 500 K. [PCl3] = _____ M [Cl2] = _____M [PCl5] = _____M
The equilibrium constant, Kc, for the following reaction is 83.3 at 500 K. PCl3(g) + Cl2(g) PCl5(g) Calculate the equilibrium concentrations of reactant and products when 0.366 moles of PCl3 and 0.366 moles of Cl2 are introduced into a 1.00 L vessel at 500 K. [PCl3] = ____M [Cl2] = _____M [PCl5] = ____M
The equilibrium constant, Kc, for the following reaction is 10.5 at 350 K. 2CH2Cl2(g) >>CH4(g) + CCl4(g) Calculate the equilibrium concentrations of reactant and products when 0.327 moles of CH2Cl2 are introduced into a 1.00 L vessel at 350 K. [CH2Cl2] = M [CH4] = M [CCl4] = M The equilibrium constant, Kc, for the following reaction is 1.29×10-2 at 600 K. COCl2(g) >>CO(g) + Cl2(g) Calculate the equilibrium concentrations of reactant and products when 0.275 moles of COCl2(g) are...
The equilibrium constant, Kc, for the following reaction is 1.29×10-2 at 600 K. COCl2(g) ----> CO(g) + Cl2(g) Calculate the equilibrium concentrations of reactant and products when 0.362 moles of COCl2(g) are introduced into a 1.00 L vessel at 600 K. [COCl2] = _____ M [CO] = _____ M [Cl2] = ____ M
The equilibrium constant, Kc, for the following reaction is 77.5 at 600 K. CO(g) + Cl2(g) COCl2(g) Calculate the equilibrium concentrations of reactant and products when 0.325 moles of CO and 0.325 moles of Cl2 are introduced into a 1.00 L vessel at 600 K. [CO] = M [Cl2] = M [COCl2] = M