# Chemistry Unit 3.1.2

Ideal Gas, Moles and Equations

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• CHEMISTRY
• MOLES
• MOLES= MASS/RELATIVE FORMULA MASS
• 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
• 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
• 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
• BALANCING EQUATIONS
• TO BALANCE AN EQUATION YOU HAVE TO BALANCE THE METALS THEN THE HYDROGEN THEN THE NONMETALS THEN CARBON THEN OXYGEN