Question

a at a certain temperature, the value of the equilibrium constant for this reaction is 9.00. at this temperature 0.100mol a and 0.100mol z are placed in a container of volume 1.00 dm³ and allowed to come to equilibrium. calculate the number of moles of x present at equilibrium.

Answer 1

The question involves using the ICE table method and the given equilibrium constant to calculate the number of moles of compound X at equilibrium in a chemical reaction.

Step-by-step explanation:

The question concerns the calculation of the number of moles of compound X present at equilibrium, when a certain amount of reactants A and Z are placed in a container at a specific volume and allowed to reach equilibrium. The equilibrium constant value is given, and the ICE table method (Initial, Change, Equilibrium) is suggested for solving the problem. It is crucial to consider the mole ratio in these types of reactions to properly calculate the changes in concentrations or moles of the substances involved.

To address the problem, one would need to know the balanced chemical equation, which has not been provided. However, assuming the student provided the reaction, the steps would involve setting up an ICE table with the initial mole amounts, determining changes (x) as the reaction goes to equilibrium, and solving for x using the equilibrium constant and the stoichiometry of the reaction.

An important point to consider is to make an assumption about the small extent of reaction if the equilibrium constant suggests as much, to simplify calculations. Otherwise, solving a quadratic equation might be necessary if the extent of reaction is significant.

Answer 2

To calculate the number of moles of x present at equilibrium, use the equilibrium constant and set up the equilibrium expression. Simplify and solve the equation to find the value of x. The number of moles of x at equilibrium is approximately 0.0875 mol.

Step-by-step explanation:

To calculate the number of moles of x present at equilibrium, we first need to determine the initial concentrations of A, B, and Z. Since we have 0.100 mol of A and 0.100 mol of Z in a 1.00 dm³ container, their initial concentrations are both 0.100 M. Using the equation A <=> B + Z, the equilibrium constant (K) is given as 9.00. We can set up the equilibrium expression as [B][Z]/[A] = 9.00.

Let's assume that x mol of A is converted to B and Z at equilibrium. This means that the final concentration of A will be 0.100 - x mol/L and the final concentrations of B and Z will be x mol/L each. Substituting these values into the equilibrium expression, we have (x)(x)/(0.100 - x) = 9.00. Simplifying the equation and solving for x, we find that x ≈ 0.0875. Therefore, at equilibrium, the number of moles of x present is approximately 0.0875 mol.