CHEM 112 Lecture Notes - Lecture 9: Limiting Reagent, Reagent
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I"(cid:448)e lea(cid:396)(cid:374)ed a (cid:448)e(cid:396)y si(cid:373)ple (cid:373)ethod fo(cid:396) li(cid:373)iti(cid:374)g (cid:396)eage(cid:374)t (cid:395)uestio(cid:374)s (cid:449)hi(cid:272)h (cid:449)ill (cid:271)e very easy for you to remember. Just like the empirical formula method, we use a table to hold all our information. The reaction of 167 g fe2o3 with 85. 8 g co produces 72. 3 g fe. Determine the limiting reactant, theoretical yield, and percent yield. The thing to remember with limiting reagents is that the reactants always determine the products so you always use the masses and information of the reactants to find the amount of product. The first thing you need to do is rewrite the equation and write the information you are given in the question above the respective substances. Do this so you can see the n=m/m equation clearer. Fe2o3 (s) + 3co (g) 2fe (s) + 3co2 (g) n= 0. 9537 mol 3. 0632 mol. We"ll (cid:374)o(cid:449) (cid:272)o(cid:374)st(cid:396)u(cid:272)t a ta(cid:271)le to put all ou(cid:396) i(cid:374)fo(cid:396)(cid:373)atio(cid:374) i(cid:374):
