Synthesis of (NH4)2SnCl6 ( ammonium hexachlorostannate IV). Solution your not po

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your not posted the full qestion but i have the qeston You are making (NH4)2SnCl6 , so you will need 2x (NH4) and 1x SnCl4 . Hence the net balanced equation is, 2NH4 + SnCl4 ---> (NH4)2SnCl6 Molar Masses NH4 = 14 + 4*1 = 18 g/mol SnCl4 = 35.45*4 + 118.71 = 260.51 g/mol Density of these compounds NH4 = 1.5274 g/ml SnCl4 = 2.226 g/ml So you need to calculate first how much you used of each compound in grams NH4 = 1.5274 g/ml * 5 ml = 7.637g SnCl4 = 2.226 g/ml * 1.8 ml = 4.0068 Now You need to convert to moles of each compound you used NH4 = 7.637g / 18 g/mol = 0.424 moles Note: Since you need 2 moles per SnCl4, you should divide 0.424 by 2 when comparing the 2. In this case, it doesn't really matter, since SnCl4 will be the limiting reagent as I will explain further below. SnCl4 = 4.0068 / 260.51 g/mol = 0.0153 moles To find your limiting reagent, just compare the 2 amount of the react reactants you used in moles in the right proportions. Either way, you will notice that the SnCl4 is considerably be lower, so it is the limiting reagent. For instance if you are making a peanut butter and jelly sandwich and the NH4 is the jelly is the NH4 and the peanutbutter is SnCl4. If you have only 15.3 servings of peanut butter and 424 servings of jelly, you are limited by the number of sandwiches of your smallest reactant, in this case peanut butter or SnCl4. The theoretical yield is how much product you obtain if ALL of your limiting reagent reacts. Which means you should get 0.0153 moles of (NH4)2SnCl6 . Molar mass of your compound = 18 + 260.51 (just add your reactants together) = 278.51 g/mol You obtained 4.72 grams 4.72 grams / 278.51 g/mol = 0.01695 moles You should have obtained: 0.0153 moles Your percent yield: 0.01695 / 0.0153 = 1.107 or 110.7% Don't be alarmed, this is normal. QUiet frequently in chemistry, we obtain products with a lot of impurities, whether it is water/solvent that hasn't dried, or the formation of some side product or even from the weighing error of our initial products. Keep in mind, since you used only 1.8 ml, you can easily mistake an 0.1-0.2 ml of product which would end in the extra 10-20% of error at the end. This error is simply that your product isn't fully dried, the presence of impurity and/or even human error.

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