Suppose a flask is filled with of , of and of . The following reaction becomes possible: The equilibrium constant for this reaction is at the temperature of the flask. Calculate the equilibrium molarity of H2O. Round your answer to two decimal places.

1.02M

Explanation:

The first thing to do is to write out the balanced chemical reaction out.

Therefore, the chemical equation for the chemical reaction is given below as:

CO + H₂O <> CO₂ + H₂.

The molarity of CO = 1.8/O.25 = 7.2M, the molarity of H2O = 0.5 × 4 = 2 m and the molarity of CO2 is 1.6 × 4 =6.4 M.

Therefore at equilibrium we have that the molarity of CO = (7.2 - x)M, the molarity of CO2 at equilibrium = (6.4 + x)M, the molarity of Hydrogen at equilibrium = x M and the molarity of H2O  at equilibrium = ( 2 - x) M.

Hence, the equilibrium constant is given as, Kc = 0.152 = [CO2][H2]/[CO][H2O].

The equilibrium constant = 0.152 = [6.4 + x][x]/[7.2 - x][2 - x].

Solving for the quadratic equation gives the value of x as equals to= 0.981.

Therefore, the equilibrium molarity of H2O = 2 - 0.981 = 1.019 = 1.02M

your answer is a. the enthalpy of formation for a pure element in its standard state is always positive.