The initial concentration for the compounds involved in the reaction displayed were determined to be [BrI(g)] = 0.3220 mol/L, [Br2(g)] = 0.3287 mol/L, [I2(g)] = 0.004086 mol/L. Calculate the value of the equilibrium constant (Kc) at 423.0 K if the equilibrium concentration of Br2(g) was 0.3273 mol/L.
K = C + 273
Equi constant:
Kc = (BrI)(I2)/(Br2)^2
To calculate the equilibrium constant (Kc), we need to use the given initial concentrations of the compounds involved and the equilibrium concentration of Br2. Follow these steps:
Step 1: Write the balanced chemical equation for the reaction. From the given information, it seems like the reaction involves the formation of Br2 from BrI and I2. Suppose the balanced equation is:
BrI(g) + I2(g) ⇌ Br2(g)
Step 2: Write the expression for Kc using the balanced equation. In this case, the equilibrium constant expression would be:
Kc = [Br2(g)] / ([BrI(g)] * [I2(g)])
(Keep in mind that the equilibrium constant expression is determined by the stoichiometry of the balanced equation.)
Step 3: Substitute the given equilibrium concentration of Br2 into the equation from step 2. We have [Br2(g)] = 0.3273 mol/L.
Step 4: Substitute the given initial concentrations into the equation from step 2. We have [BrI(g)] = 0.3220 mol/L, [I2(g)] = 0.004086 mol/L.
Step 5: Calculate the equilibrium constant (Kc) using the values from steps 3 and 4. Plug in the respective values into the equation from step 2 and perform the calculation.
Kc = (0.3273) / (0.3220 * 0.004086)
Step 6: Calculate the value of Kc using a calculator or software. The final value will be the equilibrium constant (Kc) at 423.0 K.
Note: Make sure to convert any temperature values to Kelvin (K) if necessary, as indicated in the given equation K = C + 273.
This method can generally be used to calculate the equilibrium constant (Kc) for any given reaction, provided you know the initial concentrations and the equilibrium concentration of the species involved.