Consider the following reaction at equilibrium. What will happen if so 2 is added to the reaction? 4 Fes 2n+ 110 2 2 Fe 20 3(1)+so 0

How long will it take for the concentration of A to decrease from 0.910 M to 0.387 for the reaction A → Products? (k = 0.153 M/s)

2) The following amounts of HI, H2, and I2 are introduced into a 10.00 L flask and are heated to 745 K.    mol of HI mol of H2 mol of I2 Case A 1.0 0.10 0.10 Case B 15.0 1.0 1.0 Case C 10.0 10.0 1.0 Case D 5.5 0.38 1.75 The equilibrium constant for the reaction 2HI (g) ↔ H2 (g) + I2 (g) is 0.0200 at 745 K.  In which cases will the concentration of HI increase as equilibrium is attained and in which cases will the concentration of HI decrease?

Given these initial concentrations: [SCN-] = 0.000644 M, [Fe3+] = 0.000505 M, and [Fe(SCN)2+] = 0.000 M, determine the value for K if the [Fe(SCN)2+] at equilibrium is 0.0000856 M.

At a certain temperature, the equilibrium constant for the chemical reaction shown is 6.46 × 10¬³. At equilibrium, the concentration of AB is 3.125 M, the concentration of BC is 1.425 M, and the concentration of AC is 0.210 M. Calculate the concentration of B at equilibrium. AB(aq) + BC(aq) = AC(aq) + 2 B(aq) [B] = M

How long will it take for the concentration of A to decrease from 0.910 M to 0.573 for the reaction A → Products? (k = 0.153 M/s)