This chemistry question involves key chemical concepts and calculations. The detailed solution below walks through each step, from identifying the reaction type to computing the final answer.
ScanSolve AI Answer
Step 1: Understand the concept of the equilibrium constant (K_c) and its relation to reactant and product concentrations. The equilibrium constant (K_c) indicates the extent to which a reaction proceeds to completion. If K_c is very large (K_c 1), the equilibrium lies far to the right, meaning products are heavily favored, and the concentration of reactants at equilibrium will be very small. If K_c is very small (K_c 1), the equilibrium lies far to the left, meaning reactants are heavily favored, and the concentration of products at equilibrium will be very small. If K_c is neither very large nor very small, then both reactants and products will be present in appreciable* (significant and measurable) concentrations at equilibrium. Step 2: Determine the range of K_c for appreciable concentrations. In general chemistry, a common rule of thumb is that if the equilibrium constant K_c is between 10^-3 and 10^3, then both reactants and products will be present in appreciable concentrations at equilibrium. Outside this range, one set of species (either reactants or products) will be present in very low concentrations. Step 3: Compare with the given options. The options are: a) 10^-4 to 10^4 b) 10^-3 to 10^3 c) 10^3 to 10^6 d) 10^-5 to 10^3 Based on the established chemical principle, the range 10^-3 to 10^3 corresponds to the condition where appreciable concentrations of both reactants and products are present. The final answer is b) 10^-3 to 10^3.