16. Chemical Equilibrium
ICE Charts
36PRACTICE PROBLEM
The reaction of hydrogen (H2) and iodine (I2) produces hydrogen iodide (HI) according to the following equation:
H2(g) + I2(s) ⇌ 2 HI(g)
An equilibrium mixture contains the following concentrations/amounts of the reactants and products in a 1.00 L container: H2 = 0.234 mol, HI = 0.348 mol and I2 = 10.0 g.
If an additional 0.0700 moles of H2 are added to the reaction mixture, how many moles of HI are produced when the equilibrium is reestablished?
The reaction of hydrogen (H2) and iodine (I2) produces hydrogen iodide (HI) according to the following equation:
H2(g) + I2(s) ⇌ 2 HI(g)
An equilibrium mixture contains the following concentrations/amounts of the reactants and products in a 1.00 L container: H2 = 0.234 mol, HI = 0.348 mol and I2 = 10.0 g.
If an additional 0.0700 moles of H2 are added to the reaction mixture, how many moles of HI are produced when the equilibrium is reestablished?