Kp for the reaction is 1.47 at 727°S CO2(g) + C(s) 2CO(g) Calculate Kc at this temperature
Answered above.
To calculate Kc at a given temperature, we need to use the relationship between Kp and Kc for a gaseous equilibrium reaction.
The general equation to relate Kp and Kc is as follows:
Kp = Kc(RT)^(∆n)
Where:
Kp is the equilibrium constant in terms of partial pressures
Kc is the equilibrium constant in terms of molar concentrations
R is the gas constant
T is the temperature in Kelvin
∆n is the difference in the number of moles between products and reactants
In the given reaction, we have
CO2(g) + C(s) ⇌ 2CO(g)
To find ∆n, we need to compare the sum of the moles of the products to the sum of the moles of the reactants. In this case, since there are 2 moles of CO on the product side and only 1 mole of CO2, the difference in moles is ∆n = 2 - 1 = 1.
Given
Kp = 1.47
T = 727°C = 1000 K (since °C + 273 = K)
Now, we can calculate Kc using the equation:
Kc = Kp / (RT)^(∆n)
Plugging in the values we have:
Kc = 1.47 / (R * 1000)^(1)
The last missing piece is the value of the gas constant, R. The value of R depends on the units you are using. For example, if you are using L and atm, then R = 0.0821 L·atm/(mol·K).
Once you have the value of R, substitute it into the equation to calculate Kc.
Note: Make sure the units are consistent throughout the calculations.