Answer and Explain **Chemical Equilibrium and Concentration Calculation**Sulfur dioxide reacts with carbon dioxide to form an equilibrium with sulfur trioxide and carbon monoxide, all gases (see the reaction below). A mixture of 1.91 moles each of sulfur dioxide and carbon dioxide is placed in a 2.9-liter container and allowed to reach equilibrium. If the equilibrium constant, Kc, is 2.83 at this temperature, what is the concentration of sulfur trioxide at equilibrium?\[ \text{SO}_2 \, (g) + \text{CO}_2 \, (g) \rightleftharpoons \text{SO}_3 \, (g) + \text{CO} \, (g) \]**Solution Approach:**1. **Initial Moles and Concentrations**: - Initial moles of SO2 = 1.91 moles - Initial moles of CO2 = 1.91 moles - Volume of the container = 2.9 L Initial concentrations: \[ [\text{SO}_2]_0 = \frac{1.91 \, \text{moles}}{2.9 \, \text{L}} \] \[ [\text{CO}_2]_0 = \frac{1.91 \, \text{moles}}{2.9 \, \text{L}} \]2. **Setting Up the ICE Table**: - I (Initial): Concentrations before the reaction starts. - C (Change): Change in concentrations as the system moves to equilibrium. - E (Equilibrium): Concentrations when the system reaches equilibrium. | Species | Initial (M) | Change (M) | Equilibrium (M) | | ------------|-------------------------|------------|--------------------------| | SO2 | 0.659 | -x | 0.659 - x | | CO2 | 0.659 | -x | 0.659 - x | | SO3 | 0 | +x | x | | CO | 0 | +x | x |3. **Equilibrium Expression**: \[ K_c = \frac{[\text{SO}_3][\text{CO}]}{[\text{

Given that, an equilibrium reaction is SO2 g + CO2 g ⇌ SO3 g + CO g. Also, given that, the number of…

Sulfur dioxide reacts with carbon dioxide to form an equilibrium with sulfur trioxide and carbon monoxide, all gases (see the reaction below). A mixture of 1.91 mole each of sulfur dioxide and carbon dioxide is placed in an 2.9 L container and allowed to reach equilibrium. If the equilibrium constant, Kc, is 2.83 at this temperature, what is the concentration of sulfur trioxide at equilibrium? SO₂ (g) + CO₂ (g) = SO3 (g) + CO (g) Keep extra significant figures during the calculation and round your answer to 2 decimal places. This may not be the correct number of significant figures, but do it anyway.