<span>A base, an ionic molecule, and amphipathic </span>molecule
Answer:
please check image and explanation
Explanation:
First write the balance chemical reaction
CO(g)+2H2(g)⇌CH3OH(g)
To find out the equilibrium constant first need to find the concentration of each entities at equilibrium.
Rest all thing in the image
<u>Answer:</u> The solubility of nitrogen gas in the sample is ![5.6\times 10^{-4}mol/L](https://tex.z-dn.net/?f=5.6%5Ctimes%2010%5E%7B-4%7Dmol%2FL)
<u>Explanation:</u>
We are given:
Volume percent of nitrogen gas = 80 %
To calculate the molar solubility, we use the equation given by Henry's law, which is:
![C_{N_2}=K_H\times p_{N_2}](https://tex.z-dn.net/?f=C_%7BN_2%7D%3DK_H%5Ctimes%20p_%7BN_2%7D)
where,
= Henry's constant = ![7.0\times 10^{-4}mol/L.atm](https://tex.z-dn.net/?f=7.0%5Ctimes%2010%5E%7B-4%7Dmol%2FL.atm)
= partial pressure of nitrogen gas = 1.0 atm
Putting values in above equation, we get:
![C_{N_2}=7.0\times 10^{-4}mol/L.atm\times 1.0\\\\C_{N_2}=7.0\times 10^{-4}mol/L](https://tex.z-dn.net/?f=C_%7BN_2%7D%3D7.0%5Ctimes%2010%5E%7B-4%7Dmol%2FL.atm%5Ctimes%201.0%5C%5C%5C%5CC_%7BN_2%7D%3D7.0%5Ctimes%2010%5E%7B-4%7Dmol%2FL)
Solubility of nitrogen gas in the sample = ![\frac{80}{100}\times 7.0\times 10^{-4}mol/=5.6\times 10^{-4}mol/L](https://tex.z-dn.net/?f=%5Cfrac%7B80%7D%7B100%7D%5Ctimes%207.0%5Ctimes%2010%5E%7B-4%7Dmol%2F%3D5.6%5Ctimes%2010%5E%7B-4%7Dmol%2FL)
Hence, the solubility of nitrogen gas in the sample is ![5.6\times 10^{-4}mol/L](https://tex.z-dn.net/?f=5.6%5Ctimes%2010%5E%7B-4%7Dmol%2FL)
combustion reaction are always exothermic in nature...so heat liberated is one of way to identify it