Chemistry Unit 3.1.2
Ideal Gas, Moles and Equations
- Created by: Edible_Kitten
- Created on: 24-09-14 08:41
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- CHEMISTRY
- MOLES
- MOLES= MASS/RELATIVE FORMULA MASS
- AVAGADROS CONSTANT= 6.02x10^23
- MASS= MOLES X RELATIVE FORMULA MASS
- RELATIVE FORMULA MASS= MASS/MOLES
- IDEAL GAS EQUATION
- PV=nRT
- P=PRESSURE
- V=VOLUME
- n=NUMBER OF MOLES
- T= TEMPERATURE IN KELVIN
- Untitled
- R= GAS CONSTANT
- 8.31j per k per mole
- R= GAS CONSTANT
- PV=nRT
- DEFINITIONS
- MOLECULAR FORMULA- THE AMOUNT OF ATOMS IN THE MOLECULE
- RELATIVE MOLECULAR MASS- THE MASS OF A MOLECULE IN RELATIN TO 1/12 OF CARBON 12
- ATOMIC NUMBER- THE NUMBER OF PROTON AND ELECTRON IN THE ATOM
- MOLE- A UNIT OF MESUREMENT OF 6.02x10^23 OF SOMETHING
- EMPIRICAL FORMULA- THE SIMPLIST RATIO OF ATOMS IN A MOLECULE
- RELATIVE ATOMIC MASS- THE MASS OF AN ATOM IN RELATION TO 1/12 CARBON 12
- EQUATIONS AND FORMULAE
- EMPIRICAL FORMULAE
- WRITE IN A TABLE THE ELEMENT SYMBOLS, AMOUNTS (THE IS DICTATED IN THE QUESTION) AND THE Mr
- DIVIDE THE AMOUNT BY THE Mr
- THEN MULTIPLY BY THE SMALLEST
- NOW YOU HAVE THE EMPIRICAL FORMULA
- IF THE QUESTION ASKS FOR YOU TO CALCULATE THE MOLECULAR FORMULA FROM THAT THEN CALCULATE THE Mr OF THE EMPIRICAL FORMULA
- NOW MULTIPLY THE EMPIRICALS Mr TO GET THE MOLECULAR MASS AND THEN DO THE SAME WITH THE ATOMS
- IF THE QUESTION ASKS FOR YOU TO CALCULATE THE MOLECULAR FORMULA FROM THAT THEN CALCULATE THE Mr OF THE EMPIRICAL FORMULA
- NOW YOU HAVE THE EMPIRICAL FORMULA
- THEN MULTIPLY BY THE SMALLEST
- DIVIDE THE AMOUNT BY THE Mr
- WRITE IN A TABLE THE ELEMENT SYMBOLS, AMOUNTS (THE IS DICTATED IN THE QUESTION) AND THE Mr
- MOLECULAR FORMULAE
- NOW YOU HAVE THE MOLECULAR MASS
- NOW MULTIPLY THE EMPIRICALS Mr TO GET THE MOLECULAR MASS AND THEN DO THE SAME WITH THE ATOMS
- NOW YOU HAVE THE MOLECULAR MASS
- BALANCING EQUATIONS
- TO BALANCE AN EQUATION YOU HAVE TO BALANCE THE METALS THEN THE HYDROGEN THEN THE NONMETALS THEN CARBON THEN OXYGEN
- EMPIRICAL FORMULAE
- MOLES
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