Complete the half-equation for this reaction so that you can determine the number of moles of electrons needed to reduce one mole of nitrobenzene.\n\n$\text{C}_6\text{H}_5\text{NO}_2 + \ldots e^- + \ldots \text{H}^+ \rightarrow \text{C}_6\text{H}_5\text{NH}_2 + \ldots \text{H}_2\text{O}$
The reducing agent usually employed is granulated tin together with concentrated hydrochloric acid. In the first stage, the reduction of nitrobenzene to phenylammonium chloride can be shown by the equation below.\n\nUse oxidation numbers or electrons transferred to balance this equation.\n\n$\ldots \text{C}_6\text{H}_5\text{NO}_2 + \ldots \text{HCl} + \ldots \text{Sn} \rightarrow \ldots \text{C}_6\text{H}_5\text{NH}_3\text{Cl} + \ldots \text{SnCl}_4 + \ldots \text{H}_2\text{O}$
If 5.0 g of nitrobenzene was reduced in this reaction and 4.2 g of phenylammonium chloride, $\text{C}_6\text{H}_5\text{NH}_3\text{Cl}$, was made, calculate the percentage yield.
Calculate the mass of phenylamine, $\text{C}_6\text{H}_5\text{NH}_2$, produced when 4.20 g of phenylammonium chloride reacts with an excess of $\text{NaOH(aq)}$.
Calculate the partition coefficient, $K_{\text{partition}}$, of phenylamine between dichloromethane and water using the data.
How does the basicity of phenylamine compare with that of ethylamine? Explain your answer.
State the reagents and conditions used in steps 1 and 2 in the synthesis of phenol from phenylamine.
In the box above, draw the structure of intermediate compound $E$.