Write the equilibrium expressions for the following given reactions. a. Br2 + 2HI --------------> I2 + 2HBr b. 2NaHCO3(s) --------------------> Na2CO3(s) + CO2(g) + H2O(g) 1. Bromine monochloride (BrCl) decomposes to form bromine and chlorine: 2BrCl(g) -------> Br2(g) + Cl2(g) At a certain temperature, the equilibrium constant for the reaction is 11.1. A sample of pure BrCl is placed in a 1.0 L container and allowed to decompose. At equilibrium, the reaction mixture contains 4.0 mol Cl2. What are the equilibrium concentrations of Br2 and BrCl? 2. Iodine molecules react reversibly with iodide ions to produce triiodide ions. I2(aq) + I-(aq) ----------> I3(aq) If a liter of solution prepared from 1.00x10-3 mol of I2 and 1.00x10-3 mol of the strong KI contains 6.61x10-4 mol of iodine at eq., what is the eq. constant for the reaction? Establish an ICE chart.
Write the equilibrium expressions for the following given reactions.
a. Br2 + 2HI --------------> I2 + 2HBr
b. 2NaHCO3(s) --------------------> Na2CO3(s) + CO2(g) + H2O(g)
1. Bromine monochloride (BrCl) decomposes to form bromine and chlorine:
2BrCl(g) -------> Br2(g) + Cl2(g)
At a certain temperature, the equilibrium constant for the reaction is 11.1. A sample of pure BrCl is placed in a 1.0 L container and allowed to decompose. At equilibrium, the reaction mixture contains 4.0 mol Cl2. What are the equilibrium concentrations of Br2 and BrCl?
2. Iodine molecules react reversibly with iodide ions to produce triiodide ions.
I2(aq) + I-(aq) ----------> I3(aq)
If a liter of solution prepared from 1.00x10-3 mol of I2 and 1.00x10-3 mol of the strong KI contains 6.61x10-4 mol of iodine at eq., what is the eq. constant for the reaction? Establish an ICE chart.
Trending now
This is a popular solution!
Step by step
Solved in 2 steps
