As Transitions Measuring Amount of Substance Enthalpy Changes
AS TRANSITION COURSE
SUMMER 2012
PART 1: MEASURING AMOUNT OF SUBSTANCE
MASS VOLUME MOLAR MASS AVOGADRO
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CONCENTRATION ATOM ION MOLECULE
COURSE OUTLINE
OCR Chemistry A
Unit 1 – Autumn Term 2012
• Atoms and Electron Structure
• Moles, Equations and Acids
• Structure and Bonding
• Redox, Group 2 and Group 7
Unit 1 Exam – January 2013 – 1 hour – 90 UMS – 30% of total
Unit 2 – Spring Term 2013
• Basic Concepts in Organic Chemistry
• Alkanes and Alkenes
• Haloalkanes and Alcohols
• Enthalpy Changes
• Rates and Equilibrium
• Modern Analytical Techniques
• Chemistry of the Air
• Sustainability
Unit 2 Exam – May 2013 – 1 hr 45 mins – 150 UMS – 50% of total
Unit 3 – Autumn Term 2012 and Spring Term 2013
Internal Assessments – 60 UMS – 20% of total
MEASUREMENTS IN CHEMISTRY
Mass
Convert the following into grams:
a) 0.25 kg
b) 15 kg
c) 100 tonnes
d) 2 tonnes
Volume
Convert the following into dm3:
a) 100 cm3
b) 25 cm3
c) 50 m3
d) 50000 cm3
Tip – always use standard form for very large and very small numbers!
What is a mole?
Atoms and molecules are very small – far too small to count individually!
It is important to know how much of something we have, but we count particles in MOLES because you get simpler numbers
1 mole = 6.02 x 1023 particles
(6.02 x 1023 is known as Avogadro’s number)
a) If you have 2.5 x 1021 atoms of magnesium, how many moles do you have?
b) If you have 0.25 moles of carbon dioxide, how many molecules do you have?
How can you work out how many moles you have?
a) From a measurement of MASS:
You can find the number of moles of a substance if you are given its mass and you know its molar mass:
number of moles = mass/molar mass
SUMMER 2012
PART 1: MEASURING AMOUNT OF SUBSTANCE
MASS VOLUME MOLAR MASS AVOGADRO
[pic]
CONCENTRATION ATOM ION MOLECULE
COURSE OUTLINE
OCR Chemistry A
Unit 1 – Autumn Term 2012
• Atoms and Electron Structure
• Moles, Equations and Acids
• Structure and Bonding
• Redox, Group 2 and Group 7
Unit 1 Exam – January 2013 – 1 hour – 90 UMS – 30% of total
Unit 2 – Spring Term 2013
• Basic Concepts in Organic Chemistry
• Alkanes and Alkenes
• Haloalkanes and Alcohols
• Enthalpy Changes
• Rates and Equilibrium
• Modern Analytical Techniques
• Chemistry of the Air
• Sustainability
Unit 2 Exam – May 2013 – 1 hr 45 mins – 150 UMS – 50% of total
Unit 3 – Autumn Term 2012 and Spring Term 2013
Internal Assessments – 60 UMS – 20% of total
MEASUREMENTS IN CHEMISTRY
Mass
Convert the following into grams:
a) 0.25 kg
b) 15 kg
c) 100 tonnes
d) 2 tonnes
Volume
Convert the following into dm3:
a) 100 cm3
b) 25 cm3
c) 50 m3
d) 50000 cm3
Tip – always use standard form for very large and very small numbers!
What is a mole?
Atoms and molecules are very small – far too small to count individually!
It is important to know how much of something we have, but we count particles in MOLES because you get simpler numbers
1 mole = 6.02 x 1023 particles
(6.02 x 1023 is known as Avogadro’s number)
a) If you have 2.5 x 1021 atoms of magnesium, how many moles do you have?
b) If you have 0.25 moles of carbon dioxide, how many molecules do you have?
How can you work out how many moles you have?
a) From a measurement of MASS:
You can find the number of moles of a substance if you are given its mass and you know its molar mass:
number of moles = mass/molar mass