AQA Chemistry A-level 3.1.2 Amount of Substance Notes PDF
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These detailed notes cover the AQA Chemistry A-level topic 3.1.2: Amount of Substance. Topics include relative atomic/molecular mass, moles, Avogadro's constant, ideal gas equation, empirical/molecular formulas, and equations.
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AQA Chemistry A-level 3.1.2: Amount of Substance Detailed Notes This work by PMT Education is licensed under https://bit.ly/pmt-cc https://bit.ly/pmt-edu-cc CC BY-NC-ND 4.0...
AQA Chemistry A-level 3.1.2: Amount of Substance Detailed Notes This work by PMT Education is licensed under https://bit.ly/pmt-cc https://bit.ly/pmt-edu-cc CC BY-NC-ND 4.0 https://bit.ly/pmt-cc https://bit.ly/pmt-edu https://bit.ly/pmt-cc 3.1.2.1 - Mr and Ar Relative atomic mass (Ar) is defined as: The mean mass of an atom of an element, divided by one twelfth of the mean mass of an atom of the carbon-12 isotope. Relative molecular mass (Mr) is defined as: The mean mass of a molecule of a compound, divided by one twelfth of the mean mass of an atom of the carbon-12 isotope. For ionic compounds, is it known as relative formula mass. 3.1.2.2 - Moles and the Avogadro Constant The mole is a unit of measurement for substances. It always contains the same number of particles. This number is the Avogadro Constant (L) and allows the number of particles present in a sample of a substance with known mass to be found: (n = moles) (L = Avogadro constant) The mole is a very important unit of measurement in many calculations: (where concentration is in moldm-3) https://bit.ly/pmt-cc https://bit.ly/pmt-edu https://bit.ly/pmt-cc 3.1.2.3 - Ideal Gas Equation When under standard conditions, gases and volatile liquids follow certain trends: pressure is proportional to temperature volume is proportional to temperature pressure and volume are inversely proportional These relationships can be combined to give the ideal gas equation: In order to use this equation, the variables must be in the correct standard units: p = pressure in Pascals V = volume in m3 T = temperature in Kelvin n = moles m = mass in grams R is the ideal gas constant, equal to 8.31 JK-1mol-1. 3.1.2.4 - Empirical and Molecular Formula Empirical formula is the simplest whole number ratio of atoms of each element in a compound. It is found using molar ratios of each element. (see model answer) Molecular formula is the true number of each atom in the molecule. It can be determined using the Mr of the empirical formula and the true Mr of the molecule. This gives a multiplier value which can be used to scale up the empirical formula. (see model answer) https://bit.ly/pmt-cc https://bit.ly/pmt-edu https://bit.ly/pmt-cc 3.1.2.5 - Equations and Calculations Chemical equations must be balanced before they can be used in calculations. This is because the reacting ratios must be correct. It can then be used to calculate reacting masses, percentage yield and atom economy. Percentage Yield Atom Economy In industrial chemical processes it is desirable to have a high atom economy for a reaction. This means there is little or no waste product, only the desired product. Therefore it means the process is more economically viable for industrial scale manufacture. Having a high atom economy is also beneficial for the environment as it uses less natural resources and therefore often uses less energy. https://bit.ly/pmt-cc https://bit.ly/pmt-edu https://bit.ly/pmt-cc
