Chemistry Unit 3.1.2

Ideal Gas, Moles and Equations

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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
    • 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

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