The equilibrium constant, Ke, 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 0.357 moles of HI(g) are introduced into a 1.00 L vessel at 698 K. [HI] = M [H₂] = [1₂] = = M M

Part A The equilibrium constant, Kc, for the decomposition of COC2 to CO and Cl2 is 0.68. If an equilibrium mixture contains 0.38 M CÓ and 0.55 M Cl2, what is the molar concentration of COCl2 ? COC2 (g) = CO(g) + Cl2 (g) Express your answer to two significant figures and include the appropriate units.

for this question. 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 0.316 moles of H₂ and 0.316 moles of I2 are introduced into a 1.00 L vessel at 698 K. [H₂] [1₂] = = [HI] = M M M Submit Answer 8 more group attempts remaining Retry Entire Group

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The equilibrium constant, K., for the following reaction is 5.10×10-6 at 548 K. NH,C(s)NH3(g) + HC(g) Calculate the equilibrium concentration of HCl when 0.501 moles of NH,CI(s) are introduced into a 1.00 L vessel at 548 K. [HCI] = |M

For the following reaction 6.0 moles of H₂ were combined with 4.5 moles of Cl₂. The reaction was allowed to proceed in a 1.5 L vessel. At equilibrium there were 3.0 moles of H₂ in the system. Determine the equilibrium concentrations for Cl₂ and HCI. 2HCI H₂ + Cl₂ 1b) Determine the % reaction and decide whether this reaction favours the products or reactants.

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What is the equilibrium concentration of BCl3 if a solid sample of PH3BC13 is placed in a 0.250 L closed vessel at 80.0 °C and decomposes until equilibrium is reached? Assume that there is solid present at equilibrium. At 80.0 °C, Kc = 1.87 x 10-³ for the reaction: PH3BC13(s) ⇒ PH3(g) + BCl3(g) Provide your answer in M, without units, and use the correct number of significant figures. 534.8

The equilibrium constant, K., for the following reaction is 1.29×102 at 600 K. COCI,(e)=CO(g) + Cl,(g) Calculate the equilibrium concentrations of reactant and products when 0.270 moles of COCl2(g) are introduced into a 1.00 L vessel at 600 K. [COC,] = | M [CO] M [Cl,] M

4) At high temperatures nitrogen (N₂) and oxygen (O₂) will react to form NO. N₂(g) + O₂(g) 2 NO(g) The value for the equilibrium constant for reaction 4.1 is Kc = 2.7 x 10-¹7 at some temperature T. A system initially has [N₂] = 0.0800 M and [0₂] = 0.0500 M. There is no NO initially present in the system. Find the value for [NO] that will be present at equilibrium. (4.1)