To calculate the theoretical yield of 2,4-dinitrophenol, we first need to determine the balanced chemical equation for the reaction. For simplicity, let's assume the reaction is as follows:Phenol C6H5OH + 2 HNO3 2,4-Dinitrophenol C6H3 NO2 2OH + H2ONext, we need to find the molar mass of phenol and 2,4-dinitrophenol:Phenol C6H5OH : 6 * 12.01 + 6 * 1.01 + 16.00 = 94.11 g/mol2,4-Dinitrophenol C6H3 NO2 2OH : 6 * 12.01 + 3 * 1.01 + 2 * 14.01 + 2 * 16.00 + 16.00 = 184.11 g/molNow, we can calculate the moles of phenol used:moles of phenol = mass of phenol / molar mass of phenolmoles of phenol = 10 g / 94.11 g/mol = 0.106 molAccording to the balanced equation, 1 mole of phenol produces 1 mole of 2,4-dinitrophenol. Therefore, the theoretical yield of 2,4-dinitrophenol is:moles of 2,4-dinitrophenol = 0.106 molmass of 2,4-dinitrophenol = moles of 2,4-dinitrophenol * molar mass of 2,4-dinitrophenolmass of 2,4-dinitrophenol = 0.106 mol * 184.11 g/mol = 19.52 gHowever, the problem states that the yield is 85%. To find the actual yield, we multiply the theoretical yield by the percentage yield:actual yield = theoretical yield * percentage yieldactual yield = 19.52 g * 0.85 = 16.59 gSo, the theoretical yield of 2,4-dinitrophenol is 19.52 g, and the actual yield obtained is 16.59 g.