# Kp for the reaction is 1.47 at 727°S CO2(g) + C(s) 2CO(g) Calculate Kc at this temperature

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## 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.