Amount of a Substance
Quiz yourself by thinking what should be in
each of the black spaces below before clicking
on it to display the answer.
Help!
|
|
||||
|---|---|---|---|---|---|
| Relative Atomic Mass | The weighted Average of a mass of an atom of an element, taking into account its naturally occurring isotopes, relative to 1/12th the mass of Carbon-12.
🗑
|
||||
| Relative Atomic Mass Formula = | Ar = (Average mass of an atom of an element) / (1/12 of mass of atom of Carbon-12)
🗑
|
||||
| Relative Molecular Mass | The relative molecular mass of a molecule is the mass of that molecule relative the mass of an atom of Carbon-12. Add the Ar of the Atoms in the molecule.
🗑
|
||||
| Relative Molecular Mass Formula = | Mr = (Average Mass of a Molecule) / (1/12th mass of an atom of Carbon-12).
🗑
|
||||
| Avagardo Constant: | The Number of molecules in 12 grams of Carbon-12. 6.022 x10^3
🗑
|
||||
| Number of Moles = | Mass of what you have / Mass of 1 mole (Mr).
🗑
|
||||
| Pressure = | Force / Area
🗑
|
||||
| Describe the effects on pressure for the following variables: Temp, Volume, Number of Moles: | Temp: increasing temp increases pressure, the inverse is true. Volume: Increasing Volume decreases pressure, inverse also true. No of Moles, Increasing the no of moles increases pressure, inverse true.
🗑
|
||||
| Ideal Gas Constant: | PV=nRT (Pressure x Vol = No of Moles x Constant x Temp).
🗑
|
||||
| Units of the Ideal Gas Constant | Vol = M^3, Temp = Kelvin (K), Pressure = Pa, R = J K-1 Mol-1.
🗑
|
||||
| Empirical Formula: | A formula showing the simplest whole number ratio of atoms of each element in a compound.
🗑
|
||||
| Molecular Formula: | A formula showing the actual number of each atom in a compound.
🗑
|
||||
| What method is used to find Empirical Formula? | Combustion Analysis. Compound is burnt in Oxygen and then the products by mass are analysed.
🗑
|
||||
| How to Calculate Empirical Formula: | Workout Number of moles of each element, divide all numbers by lowest amount, find ratio.
🗑
|
||||
| Moles in a Solution: | (Concentration (M) x Volume (V)) / 1000
🗑
|
||||
| Concentration = | Number of moles / Volume
🗑
|
||||
| When can we use the ideal gas equation? | To calculate the amount of gas produced in a Reaction
🗑
|
||||
| How can we find concentration, experimentally? | Using a Titration. So long as we know the concentration of the acid and equation between them.
🗑
|
||||
| Write a common Ionic equation: | H+ + OH- ---> H20
🗑
|
||||
| Titration explain the steps: | Fill burette with Acid (known concentration), measure out Alkali with Pipette and add to Flask with indicator, slowly add in acid until neutral, repeat until 2 results are the same.
🗑
|
||||
| Atom Economy (percentage): | (Mass of desired produce / Amount of reactants) x 100
🗑
|
||||
| Reaction Yield (%): | (Mass (or moles) of desired product / theoretical maximum amount of desired product) x 100
🗑
|
Review the information in the table. When you are ready to quiz yourself you can hide individual columns or the entire table. Then you can click on the empty cells to reveal the answer. Try to recall what will be displayed before clicking the empty cell.
To hide a column, click on the column name.
To hide the entire table, click on the "Hide All" button.
You may also shuffle the rows of the table by clicking on the "Shuffle" button.
Or sort by any of the columns using the down arrow next to any column heading.
If you know all the data on any row, you can temporarily remove it by tapping the trash can to the right of the row.
To hide a column, click on the column name.
To hide the entire table, click on the "Hide All" button.
You may also shuffle the rows of the table by clicking on the "Shuffle" button.
Or sort by any of the columns using the down arrow next to any column heading.
If you know all the data on any row, you can temporarily remove it by tapping the trash can to the right of the row.
Embed Code - If you would like this activity on your web page, copy the script below and paste it into your web page.
Normal Size Small Size show me how
Normal Size Small Size show me how
Created by:
mjwilson1988
Popular Chemistry sets