For the decomposition of ammonium chloride NH4cl(s) =>NH3(g)+Hcl (g) at 427degree centigrade , kp=4.8 calculate kc for this. Reaction
For the decomposition of ammonium chloride NH4cl(s) =>NH3(g)+Hcl (g) at 427degree centigrade , kp=4.8 calculate kc for this. Reaction
To calculate the equilibrium constant, Kc, for the given reaction, we need to relate Kp to Kc using the ideal gas law.
Here's how you can find Kc:
1. Start with the expression for Kp:
Kp = (P(NH3) * P(HCl)) / P(NH4Cl)
2. The expression for Kc can be obtained by replacing the partial pressures (P) with the molar concentrations (C) for gases:
Kc = (C(NH3) * C(HCl)) / C(NH4Cl)
3. The molar concentrations are related to the partial pressures using the ideal gas law:
P = nRT/V, where:
- n is the number of moles of the gas,
- R is the ideal gas constant (0.0821 L·atm/(mol·K)),
- T is the temperature in Kelvin (427°C = 700 K),
- V is the volume in liters.
4. Now, we need to determine the moles of each gas present at equilibrium. Since the balanced equation tells us that the ratio of moles is 1:1, we can assume x moles of NH3 and HCl have been produced, and x moles of NH4Cl have been consumed.
5. Calculate the molar concentration (C) for each gas using: C = n/V.
- For NH3 and HCl, the moles are x, and the volume can be any suitable value.
- For NH4Cl, the moles are x, and the volume can be any suitable value as well.
6. Substitute these molar concentrations into the Kc expression obtained in step 2, and you will have your answer.
Please note that in step 5, the volume you choose for calculation does not affect the value of Kc since it cancels out when dividing the concentrations. However, it should be consistent when comparing values of Kc for different reactions or comparing with other literature values.
Let's now calculate Kc.
Kp = Kc(RT)^delta n
Post your work if you get stuck.