Consider the following reaction,equilibrium concentrations,and equilibrium constant at a particular temperature.Determine the equilibrium pressure of H₂. D₂(g) + H₂(g) ⇌ 2 HD(g) K_p = 1.80
P(D₂) _eq = 1.1 × 10^-3atm P(HD) _eq = 2.7 × 10^-3 atm

Question

Quizplus · Accepted Answer

The equilibrium constant for the reaction, $K_p$, is given by the expression $[HD]^2 / ([D][H])$. Given $K_p = 1.80$, $P(D)_{eq} = 1.1 \times 10^{-3}$ atm, and $P(HD)_{eq} = 2.7 \times 10^{-3}$ atm, we can calculate the pressure of $H$ at equilibrium. However, the question asks for the equilibrium pressure of $HS_{1}^{1}B_{12}^{1}^{0}$, which is already provided as $1.1 \times 10^{-3}$ atm for $D$, which is a typo for the given species. The calculation for $H$ is not directly asked, but the equilibrium pressure for $D$ is correctly given, indicating a misunderstanding in the question's setup. The correct answer involves understanding the equilibrium constant and pressures given, but the provided data and question seem to have a mismatch in symbols used for chemical species.

Consider the Following Reaction,equilibrium Concentrations,and Equilibrium Constant at a Particular