1. Solid Calcium carbonate (MgCO3) decomposes at high temperatures to form solid Magnesium oxide and Carbon dioxide gas. a) Write a balanced chemical equation for this reaction b) If we start off with 660g of MgCO3, How many moles is this? c) How many moles of Carbon dioxide could be formed ? d) What mass of Carbon dioxide would be formed? e) What mass of Magnesium Carbonate would be needed to decompose to produce 5Kg of Magnesium oxide ?

onsider the balanced chemical equation :math>4Al(s)+3O2(g)2Al2O3(s). at mole ratio would you use to calculate how many moles of oxygen gas would be needed to react completely with a given number of moles of aluminum metal? What mole ratio would you use to calculate the number of moles of product that would be expected if a given number of moles of aluminum metal reacts completely?

Calculate the amounts of reactants needed in a chemical reaction to produce a specified amount of product.

Many cereals are made with high moisture content so that the cereal can be formed into various shapes before it is dried. A cereal product containing 58% H2O by mass is produced at the rate of 1000. kg/h. What mass of water must be evaporated per hour if the final product contains only 20.% water?

What is the theoretical yield for a reaction, and how does this quantity depend on the limiting reactant?

A possible practical way to eliminate oxides of nitrogen(such as NO2 ) from automobile exhaust gases uses cyanuricacid, C3N3(OH)3 . When heated to the relatively lowtemperature of 625°F, cyanuric acid converts to gaseousisocyanic acid (HNCO). Isocyanic acid reacts with NO2 inthe exhaust to form nitrogen, carbon dioxide, and water,all of which are normal constituents of the air. (a) Write balanced equations for these two reactions. (b) If the process described earlier became practical, howmuch cyanuric acid (in kilograms) would be requiredto absorb the 1.71010kgNO2 generated annuallyin auto exhaust in the United States?