The creation of shells by mollusk species is a fascinating process. By utilizing the Ca2+ in their food and aqueous environment, as well as some complex equilibrium processes, a hard calcium carbonate shell can be produced. One important equilibrium reaction in this complex process is as follows. HCO3−(aq)  H+(aq) + CO32−(aq)      K = 5.6 ✕ 10−11 If 0.33 mole of HCO3− is placed into 1.00 L of solution, what will be the equilibrium concentration (in M) of CO32−?

Consider the following fictional reaction: 2AB(aq) = 2A(aq) + B2(aq) K = 9.8 x 101 %3D If you start out with a 5.0 M solution of AB, A, and B2, what is the concentration of each species when the reaction reaches equilibrium. when solving this problem (more specifically, you are not allowed to put the algebra equation in your calculator to solve for x)

Suppose a 500. mL flask is filled with 0.10 mol of Br₂, 0.70 mol of OC12 and 0.40 mol of BrOC1. The following reaction becomes possible: Br₂(g) + OC1₂(g) ⇒ BrOC1 (g) + BrCl (g) The equilibrium constant K for this reaction is 7.81 at the temperature of the flask. Calculate the equilibrium molarity of BrOC1. Round your answer to two decimal places. M X S

Ammonia will decompose into nitrogen and hydrogen at high temperature. An industrial chemist studying this reaction fills a 75.0 L tank with 6.2 mol of ammonia gas, and when the mixture has come to equilibrium measures the amount of hydrogen gas to be 6.5 mol. Calculate the concentration equilibrium constant for the decomposition of ammonia at the final temperature of the mixture. Round your answer to 2 significant digits. K-0 C = ☐ x10 ×

I am confused because I am getting two possible answers one being 10. 6 and the other being 1.38

Write the equilibrium constant expression for the following reaction:  Fe3O4(s) + 4H2(g) to 3Fe(s) + 4H2O(g)

Calculating an equilibrium constant from a partial equilibrium composition Steam reforming of methane (CH4) produces "synthesis gas," a mixture of carbon monoxide gas and hydrogen gas, which is the starting point for many important industrial chemical syntheses. An industrial chemist studying this reaction fills a 75.0 L tank with 35. mol of methane gas and 16. mol of water vapor, and when the mixture has come to equilibrium measures the amount of hydrogen gas to be 43. mol. Calculate the concentration equilibrium constant for the steam reforming of methane at the final temperature of the mixture. Round your answer to 2 significant digits. K = [] с x10 X Ś ? olo 18 Ar

Ammonia is produced by the Haber process, in which nitrogen and hydrogen are reacted directly using an iron/iron oxide catalyst. For the reaction: N₂(g) + 3H₂(g) → 2NH3(g) AH -92.22 kJ/mol At 300 °C the equilibrium constant for the reaction is 4.34 x 10-³. a) Is this reaction endothermic or exothermic? b) What effect would the following changes have on the equilibrium position. Write forward, reverse or no change: • Add some more nitrogen gas • Increase the volume of the reaction vessel • Decrease the temperature • Remove some hydrogen gas

What is the correct equilibrium constant expression for the balanced reaction shown below? 2 HCl (g) + I2 (s)   2 HI (g) + Cl2 (g)

For the chemical equilibrium N₂ + 3H22NH3 what is the expression for the equilibrium constant? K=