At 319K the decomposition of dinitrogen tetroxide occurs with the following Kp:
2NO2(g)<>2NO(g)+O2(g) Kp=.700
What is the value of Kc for this reaction?
Kp = Kc(RT)n(prod)-n(react)
Substitute and solve for Kc. I have estimated the answer at about 0.03. Post your work if you get stuck.
Kp = Kc (RT) (exponent = (2+1)-2)
0.700 = Kc (R * 319)
not sure what R is or how to figure it out????
To find the value of Kc for the given reaction, we need to relate Kp and Kc using the equation:
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 ideal gas constant (0.0821 L·atm/(mol·K))
T is the temperature in Kelvin
∆n is the change in moles of gas molecules for the balanced equation (products minus reactants)
In the given reaction, we can determine the change in moles of gas molecules by comparing the coefficients of the products and reactants:
∆n = (2 + 1) - (2) = 3 - 2 = 1
Since the value of ∆n is 1, we don't have to consider it in the equation relating Kp and Kc. Therefore, the equation simplifies to:
Kp = Kc(RT)
Rearranging the equation:
Kc = Kp / (RT)
Now, we can substitute the given values into the equation:
Kp = 0.700
R = 0.0821 L·atm/(mol·K)
T = 319 K
Kc = 0.700 / (0.0821 L·atm/(mol·K) * 319 K)
Calculating the value of Kc:
Kc = 0.700 / 26.2439
Kc ≈ 0.0266
Therefore, the value of Kc for the given reaction is approximately 0.0266.