For the reaction 2 H,O(g) = 2H,(g) + 0,(g) the equilibrium concentrations were found to be [H,O] = 0.250 M, [H,] = 0.400M, and [O,] = 0.750M. What is the equilibrium constant for this reaction? K. = M

At a certain temperature, the equilibrium constant, ?c, for this reaction is 53.3. H2(g)+I2(g)↽−−⇀2HI(g)?c=53.3 At this temperature, 0.400 mol H2 and 0.400 mol I2 were placed in a 1.00 L container to react. What concentration of HI is present at equilibrium? [HI]= M   At a certain temperature, the equilibrium constant for the chemical reaction shown is 1.13×10−3. At equilibrium, the concentration of AB is 2.725 M, the concentration of BC is 2.225 M, and the concentration of AC is 0.220 M. Calculate the concentration of B at equilibrium. AB(aq)+BC(aq)↽−−⇀AC(aq)+2B(aq) [B]= M

A 0.066 mol sample of formaldehyde vapor, CH₂O, was placed in a heated 500 mL vessel and some of it decomposed. The reaction is CH,O(g) = At equilibrium, the CH₂O(g) concentration was 0.060 mol L-¹. Calculate the value of Kc for this reaction? Kc = H₂(g) H2(g) + CO(g) i

A gaseous reaction mixture contains 0.30 atm SO2, 0.16 atm Cl2 and 0.50 atm SO2C12 in a 2.0 L container. K=0.011 for the equilibrium system 1. SO,Cl, → so2 + Cl2 A) Is the system at equilibrium. If not what direction will the system move to reach equilibrium

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

At a given temperature, the equilibrium constant Kc for the following reaction is 0.110  2NO(g) + 2H2(g) <=>  N2(g) + 2H2O(g) What is the equilibrium constant for the following reaction? NO(g)+ H2(g) <=> 1/2N2(g) + H2O(g)

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.

Magnitude of the Equilibrium Constant 7 of 22 Review | Constants | Periodic Ta Part D For a reaction For the reaction aA + bB = cC + dD CO(g) + H2O(g) = H2(g) + CO2(g), K = 4.24 at 800 K the equilibrium constant K is defined as the ratio of products to reactants at equilibrium: what can be said about this reaction at this temperature? K [C]°D]* • View Available Hint(s) [A]*[B]* Because K represents the ratio of products to reactants, the magnitude of K is an indicator of the levels of products and reactants present when the reaction is at equilibrium. Some chemical reactions proceed almost fully to product, whereas other chemicals hardly react with each other at all, or react so as to have significant amounts of both reactants and products at equilibrium. O The equilibrium lies far to the right. O The reaction will proceed very slowly. O The reaction contains significant amounts of products and reactants at equilibrium. O The equilibrium lies far to the left.

The equilibrium expression for the the reaction:H2(g) + I2(g) <--> 2HI(g) would be: Given the reaction: A + B <--> C + DThe concentrations at equilibrium are [A] = 1 M, [B] = 1 M, [C] = 2 M, and [D] = 2 M. What is the value of the equilibrium constant (K)?

The diagrams represent the equilibrium mixture for the reaction X, (g) + Y(g) = X(g) + XY(g) at 300 K and 500 K. The X atoms are represented using red spheres, and the Y atoms are represented using blue spheres. Is the reaction exothermic or endothermic? exothermic cannot determine from the diagrams 300 K endothermic 500 K