Stoichiometry Anyone good? 10pts!?
1. Thermite reaction produces great heat of the firebombing. The formula is: Fe2O3 + 2Al -> 2Fe + Al203. How grams of Fe2O3 on Al2O3 can be converted by the reaction of 47.1 g of Al? 2. A fire extinguisher depends carbonate Sodium acid (NaHCO3) the reaction with sulfuric acid (H2SO4) to produce CO2 that develops pressure water jet or foam. The equation for this is 2NaHCO3 + H2SO4 —> Na2SO4 + 2H2O + 2CO2. If the extinguisher is to hold 600 g of NaHCO3, how many grams of sulfur would be needed to react with all of it? Please explain the steps you take! Thank you very much!
1. The amount of the product determines how much you can do. Use the amount of Converting to moles, then that is the number of moles or grams (what you want, will only require one step grams more) of product that you can do based on the stoichiometry of the equation balanced. You can use the amount of product that can do with the amount given to reverse the amount of Fe2O3 that there must be used. Convert g Al g Al2O3:'ll molar mass of each: Al MW = 27 g / mol Al2O3 MW = 102 g / 47.1 g mol Al * (1 mol Al / 27 g of Al) * (1 mol Al2O3 / 2 mol Al) * (102 g Al2O3 / 1 mol Al2O3) = 89 g Al2O3. This is the amount of product you make using the American League. Then to find out how you had Fe2O3 only do the same only the other way around. The coefficients of the equation of balance are very important in the conversion of one species to another. 89 g Al2O3 * (1 mol Al2O3 / 102 g Al2O3) * (1 mol Fe2O3 / 1 mol Al2O3) * (160 g Fe2O3 / 1 mol Fe2O3) = 139.6, about 140 g of Fe2O3. 2. The question is how many moles of NaHCO3 that you have and then converted to moles of sulfuric acid using the equation. I will do the steps in more detail: NaHCO3 MW = 84 g / mol H2SO4 MW = 98 g / mol 600 g of NaHCO3 * (1 mol / 84 g) ga converts mol. Each time you remove a drive out to do the conversions, make sure the unit is trying to shed is the bottom (see how divided by 84?) and which will drive the top end unit. 600 g * (1 mol/84 g) NaHCO3 = 7.1 moles of NaHCO3 now to use all that for a reaction with sulfuric acid, you have to have 1 / 2 the amount of sulfuric acid, as per 2 NaHCO3 need H2SO4 1 according to the equation, in order to use the molar mass of sulfuric acid to convert moles to grams. First convert to moles NaHCO3 moles of H2SO4 using coefficients the equation: 7.1 moles NaHCO3 * (1 mol H2SO4 / 2 moles of NaHCO3) = 3.6 moles of H2SO4 then convert to grams: 3.6 moles of H2SO4 * (98 g H2SO4 / H2SO4 1 mol) = 350 g H2SO4 Hope this helps!
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