When the 0.10 M solution of HClO2 is allowed to come to equilibrium, what percent of the acid molecules are ionized?

Suppose a 250. mL flask is filled with 1.2 mol of H₂ and 0.90 mol of HI. This reaction becomes possible: H₂(g) +1₂(g) → 2HI(g) Complete the table below, so that it lists the initial molarity of each compound, the change in molarity of each compound due to the reaction, and the equilibrium molarity of each compound after the reaction has come to equilibrium. Use x to stand for the unknown change in the molarity of I2. You can leave out the M symbol for molarity. H₂ 1₂ HI initial 1.2 0 ? change X equilibrium

Enter your answer in the provided box. The equilibrium constant K, for the equation 2H,(g) + CO(g) =CH;OH(g) is 23 at a certain temperature. If there are 1.81 x 102 moles of H, and 2.31 x 10-3 moles of CH3OH at equilibrium in a 6.75-L flask, what is the concentration of CO? M

Write the equilibrium constant expression, K, for the following reaction: (If either the numerator or denominator is blank, please enter 1.) COC12 (g) CO(g) + Cl₂ (g) K =

Label the following statements as true or false.True False When Q < Kc, the reaction shifts to the left to reduce stress on the system. True False When a system is at equilibrium, the reactants and the products of the reaction will be equal in concentration. True False When a system is at equilibrium, the reaction rate of the forward reaction is less than to the reaction rate of the reverse reaction. True False When Q > Kc, the reaction shifts to the right to reduce stress on the system. True False For a reversible reaction, the ΔH of the forward reaction is equal in magnitude but opposite in sign to the ΔH of the reverse reaction. True False If Kc=5 for the reaction A + B <--> AB, then AB <--> A + B has a Kc=0.2

Can you help me every step by step with number 3 part A,  part B, part C, part D? Can you explain it to me?

Mass, Volume and Keq An equilibrium mixture, at 712°C in a 1972-mL container, involving the chemical system N2(g) + 3H2(g) — 2NH3(g) is found to contain 1.26 g of №₂, 0.227 g of H₂, and 9.76×10-³ g of NH3. Calculate the equilibrium constant (Keq expressed in terms of the molar concentrations) at the given temperature. (No units required.) 0.0148

Write the concentration equilibrium constant expression for this reaction. CH;CO,C,Hg(aq)+H,O(1)→CH,CO,H(aq)+C,H,OH(aq)

4. Write an equilibrium equation, keq for the following reactions: a. N2 (g) + 3H2 (g) → 2NH3 (g) b. H2 (g) + I2 (g) → 2HI (g)

Nitrogen dioxide is one of the many oxides of nitrogen (often collectively called "NOx") that are of interest to atmospheric chemistry. It can react with itself to form another form of NOx, dinitrogen tetroxide. A chemical engineer studying this reaction fills a 125 L tank with 47. mol of nitrogen dioxide gas. When the mixture has come to equilibrium he determines that it contains 22. mol of nitrogen dioxide gas. The engineer then adds another 16. mol of nitrogen dioxide, and allows the mixture to come to equilibrium again. Calculate the moles of dinitrogen tetroxide after equilibrium is reached the second time. Round your answer to 2 significant digits. ||mol x10