This is a combination reaction, where a hydrocarbon reacts in the presence of oxygen to produce carbon dioxide and water.
Answer:
molecules have sufficient kinetic energy to overcome the intermolecular forces in the liquid
Explanation:
Answer:Partial pressure of the oxygen gas at equilibrium:
![p_{O_2}=3.8\times 10^{-5} atm](https://tex.z-dn.net/?f=p_%7BO_2%7D%3D3.8%5Ctimes%2010%5E%7B-5%7D%20atm)
Partial pressure of nitrogen monoxide gas at equilibrium:
![p_{NO}=7.6\times 10^{-5} atm](https://tex.z-dn.net/?f=p_%7BNO%7D%3D7.6%5Ctimes%2010%5E%7B-5%7D%20atm)
Explanation;
Initial Partial pressure of nitrogen dioxide gas
= p = 0.70 atm
The value of
for the reaction ![=4.48\times 10^{-13}](https://tex.z-dn.net/?f=%3D4.48%5Ctimes%2010%5E%7B-13%7D)
![2NO_2\rightleftharpoons 2NO+O_2](https://tex.z-dn.net/?f=2NO_2%5Crightleftharpoons%202NO%2BO_2)
Initially p
At eq'm p-2x 2x x
![K_p=\frac{[2x]^2[x]}{[p-2x]^2}](https://tex.z-dn.net/?f=K_p%3D%5Cfrac%7B%5B2x%5D%5E2%5Bx%5D%7D%7B%5Bp-2x%5D%5E2%7D)
![4.48\times 10^{-13}=\frac{4x^3}{[0.70-2x]^2}](https://tex.z-dn.net/?f=4.48%5Ctimes%2010%5E%7B-13%7D%3D%5Cfrac%7B4x%5E3%7D%7B%5B0.70-2x%5D%5E2%7D)
On solving for the x
![x=3.8\times 10^{-5} atm](https://tex.z-dn.net/?f=x%3D3.8%5Ctimes%2010%5E%7B-5%7D%20atm)
Partial pressure of the oxygen gas at equilibrium:
![p_{O_2}=x=3.8\times 10^{-5} atm](https://tex.z-dn.net/?f=p_%7BO_2%7D%3Dx%3D3.8%5Ctimes%2010%5E%7B-5%7D%20atm)
Partial pressure of nitrogen monoxide gas at equilibrium:
![p_{NO}=2x=2\times 3.8\times 10^{-5} atm=7.6\times 10^{-5} atm](https://tex.z-dn.net/?f=p_%7BNO%7D%3D2x%3D2%5Ctimes%203.8%5Ctimes%2010%5E%7B-5%7D%20atm%3D7.6%5Ctimes%2010%5E%7B-5%7D%20atm)
You count how much you won?
Gasoline will not dissolve in water because gasoline has more density then the water