Alaboratory manual gave precise instructions for carrying out the reaction described by the chemical equation, c2h6o + o2 c2h4o2 + h2o. it stated that if you bubble oxygen gas through a solution containing the reactant for 24 hours then the yield of c2h4o2 would be 7.50% of the theoretical amount. if you desire to produce 700. grams of the c2h4o2 in a single batch, how many kg of c2h6o should you begin with?

Astudent is given a sample of a blue copper sulfate hydrate. he weighs the sample in a dry covered porcelain crucible and got a mass of 23.875 g for the crucible, lid, and sample. the mass of the empty crucible and lid was found earlier to be 22.652 g. he then heats the crucible to expel the water of hydration, keeping the crucible at red heat for 10 minutes with the lid slightly ajar. on colling, he finds the mass of crucible, lid, and contents to be 23.403 g. the sample was changed in the process to very light clue anhydrous cuso4. if there are again 100.0 g of hydrate, how many grams of cuso4 are in it? how many moles of cuso4? (hint: molar mass of cuso4 = 159.6 g / mole. what per cent of the hydrate is cuso4? you may convert the mass of cuso4 to moles.)