The equilibrium constant, Ke, for the following reaction is 55.6 at 698 K. H₂(g) + 12 (9) 2HI(g) Calculate the equilibrium concentrations of reactants and product when 0.210 moles of H₂ and 0.210 moles of I2 are introduced into a 1.00 L vessel at 698 K. [H₂] = M [1₂] [HI] = = M M

= [Review Topics] [References] Use the References to access important values if needed for this question. The equilibrium constant, Ke, for the following reaction is 10.5 at 350. K. 2CH₂Cl2 (9) CH4 (9) + CCl4 (9) = Calculate the equilibrium concentrations of reactant and products when 0.315 moles of CH₂Cl2 (g) are introduced into a 1.00 L vessel at 350. K. [CH₂Cl₂] = [CH4] [CC14] = = Submit Answer Show Hint NOV 30 Q F4 M M M Retry Entire Group 9 F5 + tv ♫ 8 9 more group attempts remaining MacBook Air C F6 < F7 DII F8 Previous Email Instructor F9 O Next Save and Exit J F10

The equilibrium constant, Ke, for the following reaction is 7.00 x 10-5 at 673 K. to access important values if needed for this question. NH₂I(s) ⇒ NH3(g) + HI(g) If an equilibrium mixture of the three compounds in a 4.33 L container at 673 K contains 1.71 mol of NH₂I(s) and 0.445 mol of NH3, the number of moles of HI present is mol.

The equilibrium constant, Kc, for the following reaction is 0.0180 at 698 K. 2HI(g) → H₂(g) + 12 (9) Calculate the equilibrium concentrations of reactant and products when 0.305 moles of HI(g) are introduced into a 1.00 L vessel at 698 K. HI [H₂] [1₂] = = = M 3 M

The equilibrium concentrate of H2: 0.048 M The equilibrium concentrate of N2: 0.304M

Please provide the correct answer. We typically use ICE tables with these problems but I need help

The equilibrium constant, Kc, for the following reaction is 0.0180 at 698 K. 2HI(g) — H₂(g) + I₂ (9) Calculate the equilibrium concentrations of reactant and products when 0.305 moles of HI(g) are introduced into a 1.00 L vessel at 698 K. [HI] = [ [H₂] [1₂] = M M 3