Question

Given the equilibrium constant values:

N2 + 1/2O2 >>> N2O ; kc = 2.7 * 10^-18

N2O4>>>>2NO2 kc=4.6*10^-3

1/2N2 + O2>>>NO2 kc = 4.1 * 10^-9

What is a value of Kc for this reaction?

2N2O + 3O2 >>> 2N2O4

i got 2.72 * 10^17, and got it wrong. i reversed the first by taking the reciprocal, and reversed the 2nd one, times 2 by the last one. added them, square rooted and then doubled. what did i do wrong
equation 1 x 2 and reverse. (1/K<sub>1</sub><sup>2</sup>)
equation 2 x 2 and reverse. (1/K<sub>2</sub><sup>2</sup>)
equation 3 x 4 as written. (K<sub>3</sub><sup>4</sup> )

K<sub>c</sub> = (1/K<sub>1</sub><sup>2</sup>)*(1/K<sub>2</sub><sup>2</sup>)*(K<sub>3</sub><sup>4</sup>) = ??

Check my work. Make sure the equations you have added together gets the equation you want at the end. I think this will do it. I've tried to write superscripts and subscripts but if I missed one of the "turn ons or turn offs" it will be messed up. I'll correct it if it appears to be too difficult to decipher.
High school teacher

Related Questions

Which of the following statements are incorrect? 1) Gases are not included in the equilibrium const... write the equilibrium-constant expression and calculate the value of the equilibrium constant for ea... What is constant about the equilibrium constant? A. The reversibility of the reaction at equil... Calculate the equilibrium constant 2SO2(g]+O2(g]⇌2SO3(g] given equilibrium constant of SO2,O2,SO3...