To calculate the yield of p-nitroaniline, we need to follow these steps:1. Determine the limiting reactant.2. Calculate the theoretical yield.3. Apply the reaction conditions to estimate the actual yield.First, let's write the balanced chemical equation for the reaction:C6H7N + HNO3 C6H6N2O2 + H2OAniline C6H7N reacts with nitric acid HNO3 to form p-nitroaniline C6H6N2O2 and water H2O .Step 1: Determine the limiting reactantMolar mass of aniline C6H7N = 6 x 12.01 + 7 x 1.01 + 14.01 = 93.13 g/molMoles of aniline = mass / molar mass = 10 g / 93.13 g/mol = 0.107 molMolar mass of nitric acid HNO3 = 1.01 + 14.01 + 3 x 16.00 = 63.02 g/molSince we have a 70% nitric acid solution, the mass of nitric acid in 10 mL is:Mass of nitric acid = 10 mL x 1.42 g/mL density of 70% HNO3 x 0.7 = 9.94 gMoles of nitric acid = mass / molar mass = 9.94 g / 63.02 g/mol = 0.158 molThe stoichiometry of the reaction is 1:1, so we need an equal amount of moles of both reactants. Since we have fewer moles of aniline 0.107 mol than nitric acid 0.158 mol , aniline is the limiting reactant.Step 2: Calculate the theoretical yieldMolar mass of p-nitroaniline C6H6N2O2 = 6 x 12.01 + 6 x 1.01 + 2 x 14.01 + 2 x 16.00 = 138.12 g/molTheoretical yield of p-nitroaniline = moles of limiting reactant x molar mass of product = 0.107 mol x 138.12 g/mol = 14.78 gStep 3: Apply the reaction conditions to estimate the actual yieldThe actual yield depends on the reaction conditions, such as temperature, pressure, and time. Since we are given only the reaction time 1 hour , we cannot accurately estimate the actual yield without more information about the reaction conditions and the efficiency of the reaction.However, if we assume that the reaction goes to completion 100% yield under the given conditions, the actual yield of p-nitroaniline would be equal to the theoretical yield, which is 14.78 g.