The Mole Concept
Akopọ
A balance in a school laboratory can tell you that a strip of magnesium weighs 0.1 g. What it cannot tell you, and what a chemist actually wants to know, is how much magnesium that is in the sense a chemical equation cares about. Equations are recipes written in amounts: two of these react with one of those. Balances are built to read grams. Somewhere between those two facts there has to be a translator, and the mole is it.
This lesson introduces the one unit that lets a laboratory balance speak the language of a chemical equation. You will learn the single sentence the specification uses to define a mole, see why the relative formula mass on a periodic table turns into a weighable quantity the moment you write g after it, and practise moving in both directions between a mass in grams and an amount in moles. By the end you will be able to look at 9.0 g of water and 22 g of carbon dioxide and say, without hesitation, that the two samples hold exactly the same amount of substance.
Awọn Afojusun
- The relative formula mass of a substance, in grams, is known as one mole of that substance. Students should be able to use the relative formula mass of a substance to calculate the number of moles in a given mass of that substance and vice versa
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Ìdánwò Ẹ̀kọ́
Oriire fun ipari ẹkọ lori The Mole Concept. Ni bayi ti o ti ṣawari naa awọn imọran bọtini ati awọn imọran, o to akoko lati fi imọ rẹ si idanwo. Ẹka yii nfunni ni ọpọlọpọ awọn adaṣe awọn ibeere ti a ṣe lati fun oye rẹ lokun ati ṣe iranlọwọ fun ọ lati ṣe iwọn oye ohun elo naa.
Iwọ yoo pade adalu awọn iru ibeere, pẹlu awọn ibeere olumulo pupọ, awọn ibeere idahun kukuru, ati awọn ibeere iwe kikọ. Gbogbo ibeere kọọkan ni a ṣe pẹlu iṣaro lati ṣe ayẹwo awọn ẹya oriṣiriṣi ti imọ rẹ ati awọn ogbon ironu pataki.
Lo ise abala yii gege bi anfaani lati mu oye re lori koko-ọrọ naa lagbara ati lati ṣe idanimọ eyikeyi agbegbe ti o le nilo afikun ikẹkọ. Maṣe jẹ ki awọn italaya eyikeyi ti o ba pade da ọ lójú; dipo, wo wọn gẹgẹ bi awọn anfaani fun idagbasoke ati ilọsiwaju.
- The relative formula mass of magnesium oxide, MgO, is 40. What is the mass of one mole of magnesium oxide? A. 0.40 g B. 4.0 g C. 40 g D. 400 g Answer: C
- The relative formula mass of copper sulfate, CuSO4, is 159.5. What is the mass of 0.20 moles of copper sulfate? A. 3.19 g B. 31.9 g C. 79.75 g D. 319 g Answer: B
- A sample of sodium has a mass of 4.6 g. The relative atomic mass of sodium is 23. How many moles of sodium are in the sample? A. 0.20 mol B. 0.50 mol C. 2.0 mol D. 5.0 mol Answer: A
- 0.25 moles of a compound has a mass of 10 g. What is the relative formula mass of the compound? A. 2.5 B. 10 C. 40 D. 250 Answer: C
- Four samples each have a mass of 8.0 g. Which sample contains the greatest amount of substance in moles? Relative formula masses: H2O = 18, Mg = 24, MgO = 40, CO2 = 44. A. water, H2O B. magnesium, Mg C. magnesium oxide, MgO D. carbon dioxide, CO2 Answer: A
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Ṣe o fẹ ṣe adaṣe awọn ibeere idanwo adaṣe nipa The Mole Concept? Ṣe igbasilẹ ohun elo Green Bridge CBT lati wọle si awọn ibeere idanwo adaṣe ati awọn ayẹwo adaṣe kikun fun koko-ọrọ yii.
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