The balanced equation for the oxidation of 2-methyl-1-propanol C4H10O to form 2-methyl-1-propanal C4H8O using potassium dichromate K2Cr2O7 as the oxidizing agent in the presence of sulfuric acid H2SO4 is as follows:C4H10O + K2Cr2O7 + 4H2SO4 C4H8O + Cr2 SO4 3 + K2SO4 + 7H2ONow, let's calculate the mass of potassium dichromate required to oxidize 5.6 g of 2-methyl-1-propanol.First, we need to find the moles of 2-methyl-1-propanol:Moles of 2-methyl-1-propanol = mass / molar massMolar mass of 2-methyl-1-propanol C4H10O = 4 12.01 + 10 1.01 + 16.00 = 74.14 g/molMoles of 2-methyl-1-propanol = 5.6 g / 74.14 g/mol = 0.0755 molesFrom the balanced equation, we can see that 1 mole of 2-methyl-1-propanol reacts with 1 mole of potassium dichromate. Therefore, 0.0755 moles of 2-methyl-1-propanol will react with 0.0755 moles of potassium dichromate.Now, let's find the mass of potassium dichromate:Molar mass of potassium dichromate K2Cr2O7 = 2 39.10 + 2 51.99 + 7 16.00 = 294.18 g/molMass of potassium dichromate = moles molar massMass of potassium dichromate = 0.0755 moles 294.18 g/mol = 22.21 gSo, 22.21 g of potassium dichromate is required to oxidize 5.6 g of 2-methyl-1-propanol.