Question

Suppose a 500. mL flask is filled with 1.3 mol of H,O, 1.6 mol of CO2 and 0.80 mol of H. This reaction becomes possible: CO(g) +H2O(g) + CO2(g) +H2 (8) 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 H,O. You can leave out the M symbol for molarity. со но со, initial F 1 x 6 ? change equilibrium equilibrium o O o

Answer 1

molarity of H2O = no of moles/volume in L

                         = 1.3/0.5   = 2.6M

molarity of CO2 = no of moles/volume in L

                          = 1.6/0.5   = 3.2M

molarity of H2 = no of moles/volume in L

                       = 0.8/0.5     = 1.6M

                CO(g)     +    H2O(g) ------------> CO2(g)   +    H2(g)

I                0                  2.6                           3.2           1.6

C               +x                 +x                 -x    -x

E +x 2.6+x 3.2-x 1.6-x