美国高考SATII化学专题分析——Limiting Reagents

来源：51SAT整理 作者： 时间：2008-12-03 Tag：SAT考试 美国大学 SAT成绩 点击：

SAT是Scholastic Aptitude Test的缩写，是申请几乎所有美国大学必须参加的考试。通常，希望继续接受高等教育的高中生需要参加SAT考试，并且SAT考试得分是获取奖学金的重要标准之一。大部分美国大学要求SAT考试作为录取的条件并根据SAT得分授予奖学金。

Have you ever noticed that hot dogs are sold in packages of 10, while the buns come in packages of eight? In this scenario, the buns are the limiting reactant in the sense that they limit the hot dog preparation to eight. The limiting reactant or reagent is the one that is consumed first in the chemical reaction, and its consumption halts the progress of the forward reaction.

When answering questions about limiting reagents on the exam, your first step should always be to convert all the masses you were given into moles. You should set up your table as you did before, only now you’ll have two amounts and thus two numbers of moles to get you started.

Let’s look at a specific question, involving the Haber process. Basically, this is the process of making ammonia from the reaction of nitrogen and hydrogen gases. The reaction is shown below:

Molar mass	(28.02)	(2.02)	(17.04)
Balanced equation	N₂ +	3H₂	2NH₃
No. of moles
Amount

Suppose you have a total of 25.0 kg of nitrogen to react with a total of 5.00 kg of hydrogen. What mass of ammonia can be produced? Which reactant is the limiting reactant? What is the mass of the reactant that’s in excess? Insert the masses in the correct rows and find the number of moles of both.

Molar mass	(28.02)	(2.02)	(17.04)
Balanced equation	N₂ +	3H₂	2NH₃
No. of moles	892 mol	2475 mol
Amount	25,000 g	5000 g

Start with nitrogen. You have 892 moles of it available, and in order for the nitrogen to react completely with hydrogen, you’d need 3(892 mol) = 2676 moles of hydrogen, which you don’t have. Therefore, hydrogen is the limiting reagent. Now let’s answer the other parts of the question. The mass of ammonia that can be produced is limited by the amount of hydrogen, so do your calculations based on the number of moles of hydrogen available. Your chart should look like the one below:

Molar mass	(14.02)	(2.02)	(17.04)
Balanced equation	N₂ +	3H₂	2NH₃
No. of moles	825 mol used	2475 mol used	therefore 1650 mol produced
Amount	892 mol 23,117 g used 25,000g	5000 g	1650 mol (17.04) = 28,116 g produced

更多详细资料请参见：http://bbs.51sat.com/

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