<li><p>Molten iron and carbon monoxide are produced in a blast furnace by the reaction of iron (III) oxide and coke (carbon). If 25.0 kg of pure Fe2O3 are used, how many moles of iron can be produced?</p></li>
<li><p>Ammonia gas produced as a by-product in an industrial reaction can be reacted with sulfuric acid in order that the gas does not escape into the atmopshere. The product, ammonium sulfate, can be used as a fertilizer. Determine how many kilograms of acid are required to produce 1000.0 kg of (NH4)2SO4.</p></li>
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<li><p>simple stoichiometry. once you get your shiz into moles you're pimpin. convert the mass of iron oxide into moles by multiplying by the molar mass of iron oxide. think ratios of the coefficients now. well, looks like you need to write out the balanced equation. once u got that, multiply the value of the moles u got earlier by the (coefficient of iron/ coefficient of iron oxide) to get moles of iron. </p></li>
<li><p>same shiz here. actually always write out the balanced equation first for stoichimetry problems to get a good picture of what u need to solve for. then take the mass of (NH4)2SO4 and convert to moles. do the mole ratios to find moles of acid then multiply that by molar mass (g/mol) to get grams. </p></li>
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