How many kilograms of perovskite are required to produce 5.00 kg of titanium? Perovskite = 29.4% Ca, 35.2% Ti, and 35.3% O

Consider the smelting of iron ore which consists of Fe2O3 and Fe3O4. If Fe is produced in the pig iron, and FeO is produced in the slag, what are the chemical equations involved?

When 1.848 g of finely divided magnesium is burned, 3.080 g of a white oxide is obtained. Determine the empirical formula of the oxide. At mass of Mg= 24g/mole and O= 16g/mole

Sodium hydrogen sulfate is used as a cleaning agent and as a flux (a substance that promotes the fusing of metals and prevents the formation of oxides). One of the ways in which sodium hydrogen sulfate is manufactured is by reacting sodium dichromate, Na2Cr2O7, with sulfuric acid. This process also forms water and chromium(VI) oxide, CrO3. Write a balanced equation for this reaction. (You do not need to include states.) How many kilograms of sodium dichromate, Na2Cr2O7, are necessary to produce 130.4 kg of sodium hydrogen sulfate? How many kilograms of chromium(VI) oxide are formed when 130.4 kg of sodium hydrogen sulfate is made? What is the minimum volume of 18.0 M H2SO4 solution necessary to react with 874.0 kg of sodium dichromate? What is the maximum mass of sodium hydrogen sulfate, NaHSO4, that can be formed from the reaction of 874.0 kg of sodium dichromate with 400.0 L of 18.0 M H2SO4?

What mass of Cu(IO3)2 can be formed from 0.650 g of CuSO4 · 5H2O? What mass of KIO3 is needed to convert the copper in 0.2750 g of CUSO4 - 5H2O to Cu(IO3)2?

Write the chemical equation for the word equation below. Each blank should be a different substance and the reaction does not need to be balanced. Molybdenum(IV) chromate reacts with lithium telluride to make molybdenum(IV) telluride and lithium chromate

What mass of ZNCI2 can be prepared from the rebction of 4.52 grams of zinc with 4.52 grams of HCl? Zn + 2HCI → ZNCI2 + H2 O 8.45 g O 9.42 g O 17.9 g O 7.94 g O 16.8 g

How many energy levels are there in the valence band of a single crystal of potassium with a mass of 6.05 mg

A sample of 0.2500 g of an antimony alloy is taken and converted into Sb2O4 by appropriate processes. Since the product brought to constant weight is 0.1305 g, calculate the percentage of antimony in the alloy (Sb = 121g / mol, 0 = 16 g / mol).

Consider the series of reactions to synthesize the alum (KAl(SO4 )2 · xH2O(s)) Assuming an excess of the other reagents, from one mole of aluminum Al (s), how many moles of alum will be produced?