Hydrogen iodide is formed according to the gas-phase reaction A 1.00 L reaction…
CHEMISTRY · Multi-part · A Level · Chemistry · Chemical equilibria (Le Chatelier’s principle and Kc) · Chemical equilibria (Le Chatelier’s principle and Kc)
Problem
Hydrogen iodide is formed according to the gas-phase reaction
H2(g)+I2(g)⇌2HI(g)
A 1.00 L reaction vessel at 448 °C initially contains 0.800 mol of H2(g) and 0.500 mol of I2(g). After equilibrium is established, the vessel is found to contain 0.620 mol of HI(g).
(a) Show, using stoichiometric reasoning, whether H2(g) or I2(g) is the limiting reactant in the forward reaction under the initial conditions.
(b) Calculate the equilibrium amounts (in moles) of all three species present in the vessel.
(c) Determine the numerical value of Kc for the reaction at 448 °C.
(d) Compute the percentage of the limiting reactant that has been consumed when equilibrium is reached and interpret what this implies about the position of equilibrium.