You place 3.00 mol of pure SO3 in an 8.00-L. flask at 1150 K. At equilibrium, 0.58 mol of O2 has

step 1 Let's first solve for our values here. We're going to start. We're told we have S .O3 that's pla

You place 3.00 mol of pure SO3 in an 8.00-L. flask at 1150...

You place 3.00 mol of pure $\mathrm{SO}_{3}$ in an $8.00-\mathrm{L}$. flask at $1150 \mathrm{K}$. At equilibrium, 0.58 mol of $\mathrm{O}_{2}$ has been formed. Calculate $K$ for the reaction at $1150 \mathrm{K}$ $$ 2 \mathrm{SO}_{3}(\mathrm{g}) \rightleftarrows 2 \mathrm{SO}_{2}(\mathrm{g})+\mathrm{O}_{2}(\mathrm{g}) $$

You place 3.00 mol of pure $\mathrm{SO}_{3}$ in an $8.00-\mathrm{L}$. flask at $1150 \mathrm{K}$. At equilibrium, 0.58 mol of $\mathrm{O}_{2}$ has been formed. Calculate $K$ for the reaction at $1150 \mathrm{K}$
$$
2 \mathrm{SO}_{3}(\mathrm{g}) \rightleftarrows 2 \mathrm{SO}_{2}(\mathrm{g})+\mathrm{O}_{2}(\mathrm{g})
$$

Key Concepts

Chemical Equilibrium

Chemical equilibrium is the state in a reversible reaction where the rate of the forward reaction equals the rate of the reverse reaction. At this point, despite ongoing reactions, the concentrations of reactants and products remain constant over time. This concept is central to understanding how systems achieve balance and how conditions such as temperature and pressure influence the final composition of a reaction mixture.

Equilibrium Constant (K)

The equilibrium constant (K) is a dimensionless number that expresses the ratio of the concentrations of products to reactants, each raised to the power of their stoichiometric coefficients, when a chemical reaction has reached equilibrium. This value provides insight into the extent to which a reaction proceeds, indicating whether the equilibrium favors the formation of products or reactants.

Stoichiometry

Stoichiometry involves the quantitative relationships between the amounts of reactants and products in a chemical reaction as dictated by the balanced chemical equation. It allows the determination of how a change in the amount of one species affects the others and is essential for setting up relationships used in equilibrium calculations.

ICE Table Method

The ICE table (Initial, Change, Equilibrium) is a systematic method used to track the concentrations or pressures of the chemical species involved in a reaction as it proceeds towards equilibrium. It organizes the initial conditions, the changes during the reaction, and the equilibrium state, making it easier to set up the relationships needed to solve equilibrium problems.

Concentration Calculation

Concentration, expressed usually in molarity, is calculated by dividing the number of moles of a substance by the volume of the solution in liters. Accurate conversion from moles to molarity is important in equilibrium problems because the equilibrium constant expression is typically written in terms of concentrations, ensuring consistency in calculations.

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