Chemistry
Chemistry
Problem
The gas-phase equilibrium 2 NOBr(g) ⇌ 2 NO(g) + Br₂(g) is studied at 300 K, where Kc = 1.8 × 10⁻². A 2.50 L rigid flask at this temperature initially contains 0.200 mol NOBr and 0.0600 mol NO; no Br₂ is present. After sealing, the system is allowed to reach equilibrium. (a) Taking y as the number of moles of NOBr that decompose after sealing, express the equilibrium molarities of NOBr, NO, and Br₂ in terms of y. (b) Derive the single algebraic equation in y that results from substituting your expressions from part (a) into the equilibrium-constant expression. (c) Solve for y and determine the equilibrium molarity of each species. (d) Calculate the total pressure (in atm) in the flask at equilibrium, assuming ideal-gas behavior.Intuitive explanation
This is an equilibrium problem where you need to track how concentrations shift as the system reaches its balance point. Start by converting moles to initial concentrations, then use an ICE table to account for how much NOBr decomposes (or NO recombines) to satisfy . The key insight is recognizing the direction of shift: compare the reaction quotient to to see whether the system must shift forward or backward to reach equilibrium.
Intuitive explanation
This is an equilibrium problem where you need to track how concentrations shift as the system reaches its balance point. Start by converting moles to initial concentrations, then use an ICE table to account for how much NOBr decomposes (or NO recombines) to satisfy . The key insight is recognizing the direction of shift: compare the reaction quotient to to see whether the system must shift forward or backward to reach equilibrium.