Combined Science Double Award - 9204 OxfordAQA

Use Of Amount Of Substance In Relation To Masses Of Pure

Muhtasari

A white crystalline solid arrives in a laboratory with nothing written on the jar. Nobody knows what it is. Within an hour an analyst can hand back its formula, and the only instrument that really mattered was a balance. That is a strange claim on the face of it: a balance reports masses, and a formula is a statement about how many atoms of each kind are locked together. Getting from one to the other is the single most useful piece of arithmetic in the whole of chemistry, and it is what this lesson is about.

You will start by learning to add up a formula, turning a string of symbols and subscripts into one number that stands for the mass of the whole unit. From there you will work out what fraction of a compound is the element you actually care about, which is how a food label turns into a sodium figure and how a mining company decides whether an ore is worth digging. Then comes the reverse trip, and it is the best part: given nothing but masses measured on a bench, you will reconstruct the formula of a substance you have never met, then sharpen that formula until it names one compound and one compound only. Both of the first two skills are worth marks on both tiers of the chemistry paper, and the third carries the single longest calculation on it.

Malengo

  1. The relative formula mass (Mr) of a compound is the sum of the relative atomic masses of the atoms in the numbers shown in the formula. Students are expected to use relative atomic masses in the calculations specified in the subject content. Students should be able to calculate the relative formula mass (Mr) of a compound from its formula.
  2. The percentage by mass of an element in a compound can be calculated from the relative atomic mass of the element in the formula and the relative formula mass of the compound.
  3. The empirical formula of a compound can be calculated from the masses or percentages of the elements in a compound. Students should be able to calculate empirical formulae and molecular formulae.

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Maelezo ya Somo

Suppose you are handed a sample of a compound built from just two elements, and you are told its mass and how much of that mass is each element. Nothing else. No spectrometer, no reference book, no helpful colleague. It sounds like far too little information to name the substance, and for most of the history of chemistry people agreed with you. The breakthrough came from realising that atoms of different elements have fixed, comparable masses, so a mass on a balance is a disguised count of atoms. Undo the disguise and the formula falls out.

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Tathmini ya Somo

Hongera kwa kukamilisha somo la Use Of Amount Of Substance In Relation To Masses Of Pure. Sasa kwa kuwa umechunguza dhana na mawazo muhimu, ni wakati wa kuweka ujuzi wako kwa mtihani. Sehemu hii inatoa mazoezi mbalimbali maswali yaliyoundwa ili kuimarisha uelewaji wako na kukusaidia kupima ufahamu wako wa nyenzo.

Utakutana na mchanganyiko wa aina mbalimbali za maswali, ikiwemo maswali ya kuchagua jibu sahihi, maswali ya majibu mafupi, na maswali ya insha. Kila swali limebuniwa kwa umakini ili kupima vipengele tofauti vya maarifa yako na ujuzi wa kufikiri kwa makini.

Tumia sehemu hii ya tathmini kama fursa ya kuimarisha uelewa wako wa mada na kubaini maeneo yoyote ambapo unaweza kuhitaji kusoma zaidi. Usikatishwe tamaa na changamoto zozote utakazokutana nazo; badala yake, zitazame kama fursa za kukua na kuboresha.

  1. What is the relative formula mass of sodium hydrogencarbonate, NaHCO3? Relative atomic masses: H = 1, C = 12, O = 16, Na = 23. A. 52 B. 68 C. 84 D. 100 Answer: C
  2. What is the percentage by mass of oxygen in water, H2O? Relative atomic masses: H = 1, O = 16. A. 11.1 B. 16.0 C. 50.0 D. 88.9 Answer: D
  3. A compound contains 1.4 g of nitrogen and 0.3 g of hydrogen. What is its empirical formula? Relative atomic masses: H = 1, N = 14. A. NH B. NH2 C. NH3 D. N3H Answer: C
  4. Which of these is the empirical formula of glucose, C6H12O6? A. CHO B. CH2O C. C2H4O2 D. C3H6O3 Answer: B
  5. A compound has the empirical formula CH2 and a relative formula mass of 70. What is its molecular formula? Relative atomic masses: H = 1, C = 12. A. C2H4 B. C3H6 C. C4H8 D. C5H10 Answer: D

Fanyia kazi maswali haya kwenye programu

Fanyia kazi maswali haya kwenye programu

Vitabu Vinavyopendekezwa

OxfordAQA International GCSE Chemistry (9202)
OxfordAQA International GCSE Chemistry (9202)
Manukuu: Student Book
Mchapishaji: Oxford University Press
Mwaka: 2016
ISBN: 978-0-19-837589-0
Maelezo: The endorsed student book for the 9202 specification, covering the full subject content with required practicals and exam guidance.
OxfordAQA International GCSE Combined Sciences Chemistry (9204)
OxfordAQA International GCSE Combined Sciences Chemistry (9204)
Manukuu: Student Book
Mchapishaji: Oxford University Press
Mwaka: 2017
ISBN: 978-0-19-842308-9
Maelezo: The chemistry half of the Combined Science series. A lighter parallel treatment of the same content, useful for a second explanation.

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