Chemistry /Edexcel A Level Chemistry: 5: Formulae, Equations and Amounts of Substance Part 2
Edexcel A Level Chemistry: 5: Formulae, Equations and Amounts of Substance Part 2
This deck covers key concepts related to formulae, equations, and amounts of substances in chemistry, including gas laws, concentration calculations, and yield measurements.
What is the molar volume of a gas?
The volume of 1mol of the gas under stated conditions. At room temperature and atmospheric pressure the molar volume of all gases is 24dm-3mol-1
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Key Terms
Term
Definition
What is the molar volume of a gas?
The volume of 1mol of the gas under stated conditions. At room temperature and atmospheric pressure the molar volume of all gases is 24dm-3mol-1
What is room temperature?
16°C
What is atmospheric pressure?
100kPa
Volume of gas (cm3) =
Amount of gas (mol) x molar volume (cm3 mol-1)
How would you calculate the amounts of reactants and products?
Write a balanced equation
Write down the amounts in moles of the relevant reactants and products in the equation
The volume of gas, under a given temperature and pressure depends only on…
…the amount of gas, not the type of gas
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Term | Definition |
---|---|
What is the molar volume of a gas? | The volume of 1mol of the gas under stated conditions. At room temperature and atmospheric pressure the molar volume of all gases is 24dm-3mol-1 |
What is room temperature? | 16°C |
What is atmospheric pressure? | 100kPa |
Volume of gas (cm3) = | Amount of gas (mol) x molar volume (cm3 mol-1) |
How would you calculate the amounts of reactants and products? |
|
The volume of gas, under a given temperature and pressure depends only on… | …the amount of gas, not the type of gas |
Concentration (g/dm-3) = | Mass of solute (g) / volume of solution (dm-3) |
Concentration (mol/dm-3) = | Amount of solute (mol) / volume of solution (dm3) |
What is the concentration of a solution? | How much solute is dissolved in a certain volume |
What is a titration? | A volumetric analysis technique for finding the concentrations of solutions and for investigating the amounts of chemicals involved in reactions |
What is a standard solution? | A solution with an accurately known concentration |
What is a primary standard? | A chemical which can be weighed out accurately to make up a standard solution |
The method for preparing a standard solution is only appropriate with a chemical that is… | is very pure |
does not gain or lose mass when in the air | has a relatively high molar mass so that weighing errors are minimised |
What was the ideal gas equation used for? | Measuring the molar masses of gases before mass spectrometry |
What is the ideal gas equation accurate enough to determine? | The molecular formula of elements and compounds |
What does the ideal gas equation show? | That at a fixed temperature and pressure the volume of a gas depends only on the amount of moles. |
How do you calculate the masses of reactants and products? | Write a balanced equation |
What is an uncertainty? | The amount of error your measurements might have? |
For any piece of equipment, what will the uncertainty be? | Half the smallest increment of measure in either direction |
What should be done if different measurements are being combined? | Their uncertainties should be combined |
How would you calculate percentage uncertainty? | Uncertainty/reading x 100 |
How can uncertainty be reduced? | By using the most precise equipment possible and the largest measurements |
What is theoretical yield? | The maximum that you could get |
How would you calculate theoretical yield? | Using the moles of reactants and products |
How would you calculate percentage yield? | Actual yield/theoretical yield x 100 |
What is atom economy? | A measure of how efficient the reaction is |
How would you calculate atom economy? | Molar mass of desired product/combined molar masses of all products x 100 |