False, our tongue and nose work together
<u>Answer:</u> The value of
for the chemical equation is ![8.341\times 10^{-5}](https://tex.z-dn.net/?f=8.341%5Ctimes%2010%5E%7B-5%7D)
<u>Explanation:</u>
For the given chemical equation:
![N_2(g)+O_2(g)\rightarrow 2NO(g)](https://tex.z-dn.net/?f=N_2%28g%29%2BO_2%28g%29%5Crightarrow%202NO%28g%29)
To calculate the
for given value of Gibbs free energy, we use the relation:
![\Delta G=-RT\ln K_p](https://tex.z-dn.net/?f=%5CDelta%20G%3D-RT%5Cln%20K_p)
where,
= Gibbs free energy = 78 kJ/mol = 78000 J/mol (Conversion factor: 1kJ = 1000J)
R = Gas constant = ![8.314J/K mol](https://tex.z-dn.net/?f=8.314J%2FK%20mol)
T = temperature = 1000 K
= equilibrium constant in terms of partial pressure = ?
Putting values in above equation, we get:
![78000J/mol=-(8.314J/Kmol)\times 1000K\times \ln K_p\\\\Kp=8.341\times 10^{-5}](https://tex.z-dn.net/?f=78000J%2Fmol%3D-%288.314J%2FKmol%29%5Ctimes%201000K%5Ctimes%20%5Cln%20K_p%5C%5C%5C%5CKp%3D8.341%5Ctimes%2010%5E%7B-5%7D)
Hence, the value of
for the chemical equation is ![8.341\times 10^{-5}](https://tex.z-dn.net/?f=8.341%5Ctimes%2010%5E%7B-5%7D)