Question

Sulfur reacts with oxygen to form sulfur trioxide, according to the following equation: 2S (g) + 3O2 (g) → 2SO3 (g) Calculate the value of the equilibrium constant at 310°C if an equilibrium mixture contains the following concentrations of reactants and products: [S2 (g)] = 0.059 mol/L; [O2 (g)] = 0.138 mol/L; [SO3] = 0.042 mol/L

Name: sulfur reacts with oxygen to form sulfur tri oxide according to the following equation 2s g 3o2 g 2so3 g calculate the value of the equilibrium constant at 310c if an equilibrium mixture con 48649
Uploaded: 2022-04-14T03:06:59-08:00
Duration: 1 min 7 s
Channel: Ronald Prasad
Description: sulfur reacts with oxygen to form sulfur tri oxide according to the following equation 2s g 3o2 g 2so3 g calculate the value of the equilibrium constant at 310c if an equilibrium mixture con 48649

          Sulfur reacts with oxygen to form sulfur trioxide, according to the following equation:
2S (g) + 3O2 (g) → 2SO3 (g)
Calculate the value of the equilibrium constant at 310°C if an equilibrium mixture contains the following concentrations of reactants and products:
[S2 (g)] = 0.059 mol/L; [O2 (g)] = 0.138 mol/L; [SO3] = 0.042 mol/L

Added by Kristen F.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Ronald Prasad

04/14/2022

Step 1

Step 1: Write the expression for the equilibrium constant (Kc) using the concentrations given in the question and the balanced chemical equation: \[ Kc = \left( \dfrac{[SO3]^2}{[S]^2[O2]^3} \right) \] Show more…

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Sulfur reacts with oxygen to form sulfur trioxide, according to the following equation: 2S (g) + 3O2 (g) → 2SO3 (g) Calculate the value of the equilibrium constant at 310°C if an equilibrium mixture contains the following concentrations of reactants and products: [S2 (g)] = 0.059 mol/L; [O2 (g)] = 0.138 mol/L; [SO3] = 0.042 mol/L