please show all steps. The decomposition reaction of COC12 is, COCldg,-CO(g) + Cl2(g) Kc = 2.2...
The equilibrium constant, Kc. for the following reaction is 1.29×102 at 600 K. COC12(g) = CO(g) + Ch(g) Calculate the equilibrium concentrations of reactant and products when 0.305 moles of COCL() are introduced into a 1.00 L vessel a 600 K CoC] Co]
Consider the following reaction: COCl2(g) = CO(g) + Cl2(8) A reaction mixture initially contains 1.6 M COC12. Determine the equilibrium concentrations of COCI, CO, and Cl2 if Kc for the reaction at this temperature is 8.33 x 10-4. Calculate this based on the assumption that the answer is negligible compared to 1.6. Use x is small approximation. Show Q Validity check [Cl2] = [CO]= [COCI2] = Calculate the reaction quotient, Q A % Validity Check A Calculate the A/ equilibrium...
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
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 0.355 moles of CO and 0.355 moles of Cl2 are introduced into a 1.00 L vessel at 600 K. [CO] = M [Cl2] = M [COCl2] = M
A student ran the following reaction in the laboratory at 541 K: COC12(E) CO(g) + Cl2(g) When she introduced 1.13 moles of COC12(e) into a 1.00 liter container, she found the equilibrium concentration of Cl2(g) to be 3.83x10-2 M. Calculate the equilibrium constant, K, she obtained for this reaction.
Consider the reaction. PCI; (g) = PCI,(g) + Cl2(g) Kc = 0.0420 The concentrations of the products at equilibrium are [PC13] = 0.160 M and [Cl2] = 0.160 M. What is the concentration of the reactant, PCs, at equilibrium? [PCI31= C [PCIS] = M
For the following reaction, the initial concentrations of CO is 0.500M and Cl2 is 1.00 M. What are the equilibrium concentrations of each species at 400K? (show all work) COCl2(g) ⇌ CO(g) + Cl2 (g) Kc = 0.680 at 400 K
Consider the reaction. PCl5(g)−⇀↽−PCl3(g)+Cl2(g)Kc=0.0420 The concentrations of the products at equilibrium are [PCl3]=0.180 M and [Cl2]=0.280 M. What is the concentration of the reactant, PCl5, at equilibrium?
The equilibrium constant, Kc, for the following reaction is 77.5 at 600 K. CO(g) + Cl2(g) goes to COCl2(g) . Calculate the equilibrium concentrations of reactant and products when 0.320 moles of CO and 0.320 moles of Cl2 are introduced into a 1.00 L vessel at 600 K. [CO] = ___M [Cl2] = ___M [COCl2] = ___M
1. The initial concentrations of reactants and products for this reaction are given below. N2(g) + O2(g) ⇄ 2NO(g) Calculate Q for this reaction. Answer this to one decimal place (e.g. 10.2) The initial concentration of N2 is 1.0 M The initial concentration of O2 is 1.0 M The initial concentration of NO is 2.5 M 2. Calculate the equilibrium concentration of Cl2 in that results from the decomposition of COCl2 with an initial concentration of 0.3166 M. COCl2(g) ⇌ CO(g)...