CLASS X SEMESTER 2 SMKN 7 BANDUNG Mole Concept CLASS X SEMESTER 2 SMKN 7 BANDUNG

Isi dengan Judul Halaman Terkait Standard Competency Comprehends mole concept Basic competency Explains mole concept Applies Law Gay Lussac and Law Avogadro The aim of the lesson Student understands and solvent of description of proton, neutron and electron based on relative charge and his(its relative mass Hal.: 2 Isi dengan Judul Halaman Terkait

Isi dengan Judul Halaman Terkait Solvent student of description of mass and charge in atom Solvent student of description of contribution of proton and neutron at atomic nucleus based on atomic number and mass number Solvent student of deduction number of protons, neutron and electron which there is in atom and ion from atomic number and mass number given Student can differentiate isotope based on neutron amounts differs in the Solvent student of deduction of atom electronic configuration Hal.: 3 Isi dengan Judul Halaman Terkait

Comprehends mole concept Law Gay-Lussac ( Volume Comparison Law) Express that comparison of gas volume involving in a chemical reaction ( either reactant and also matter result of reaction) be integer and simple Comparison law of this volume applies at reaction of gas which formation of its(the molecule is simple Hal.: 4 Isi dengan Judul Halaman Terkait

Isi dengan Judul Halaman Terkait Law Avogadro Be a chemistry fundamental law expressing that in the situation the same temperature and pressure, gas having the same volume consisted of number of the same molecules Hal.: 5 Isi dengan Judul Halaman Terkait

Isi dengan Judul Halaman Terkait Mole Concept Molecule Formula and Empiric formula Chemistry formula is statement of chemical composition from a compound applies symbols to express its(the compiler atom types Example; water chemistry formula H2O Water compiler elements is Hydrogen ( H) and oxygen ( O) Hal.: 6 Isi dengan Judul Halaman Terkait

Isi dengan Judul Halaman Terkait Empiric formula a molecule is formula which more modestly is compared to its(the molecule formula Molecule formula seen equal to empiric formula but its(the index number only loads information of comparison from interconnected elements one another and is not atoms that is actually Example; ethane molecule formula is C2H6 indicating that comparison of carbon atoms and hydrogen is 1 compares 3 so that its(the empiric formula is CH3 Water molecule formula equal to its(the empiric formula is H2O Hal.: 7 Isi dengan Judul Halaman Terkait

Isi dengan Judul Halaman Terkait Relative Atom Mass The standard of atomic mass unit is based on the mass of carbon -12 (C-12) isotope 1 amu = 1/12 x mass of C-12 atom or mass of C-12 atom = 12 amu where 1 amu = 1,66 x 10-27 kg Ar X = Mx 1/12 MC-12 Ar X = the relative atomic mass of x element M x = the average mass per atom of x element MC-12 = the mass of a carbon-12 atom Hal.: 8 Isi dengan Judul Halaman Terkait

Isi dengan Judul Halaman Terkait Relative Molecule Mass Mr xy = M xy 1/12 MC-12 Where; Mr xy = the relative molecule mass of xy M xy = the average mass of xy molecule MC-12 = the mass of a carbon-12 atom Hal.: 9 Isi dengan Judul Halaman Terkait

Isi dengan Judul Halaman Terkait Mole Concept The mole number of a substance can be determined by the equation as follows; n = mA (for atom) Ar n = mM (for molecule or compound) Mr n = the number substance mole (mol) mA= atomic mass (gram) mM= molecule or compound mass (gram) Ar= the relative atomic mass of element (gram/mol) Mr= the relative molecule mass of compound or molecule (gram/mol) Hal.: 10 Isi dengan Judul Halaman Terkait

The Relation of Mole and Particles Number N = n x 6,02 x 1023 particle n : the number of mole of the substance (mol) N : the number of particle of substance Molar Mass of Substances Mm= m n Mm : molar mass of substance (gram/mol) m : mass of substance (gram) n : the number substance mole (mol) Hal.: 11 Isi dengan Judul Halaman Terkait

Isi dengan Judul Halaman Terkait Molar Volume of Substance Vm = V n Vm : molar volume of substance (l/mol) V : volume of substance (liter) V = n x 22,4 liter/mol Hal.: 12 Isi dengan Judul Halaman Terkait

Isi dengan Judul Halaman Terkait Equation of Ideal Gas Pv = n.R.T or V = n.R.T P v : gas volume (liter) n : number of gas moles (mol) R : gas constant (0,082 L atm/mole.k) T : absolute temperature (k) P : gas pressure (atm) Hal.: 13 Isi dengan Judul Halaman Terkait

Isi dengan Judul Halaman Terkait For situation of referring gas in the situation other gas V = n V gas1 V gas2 n1 : number of gas moles 1 (mol) n2 : number of gas moles 2 (mol) V1 : gas volume 1 (liter) V2 : gas volume 2 (liter) Hal.: 14 Isi dengan Judul Halaman Terkait

Isi dengan Judul Halaman Terkait Molarities M = n V M : molarities of solution (mol/L or M) n : number of mole of the solute (mol) V : volume of solution (liter) Hal.: 15 Isi dengan Judul Halaman Terkait

Isi dengan Judul Halaman Terkait From all description upper to be inferential “ number of moles was central terminal from all Stoichiometry traffic line “ MASS MOLE NUMBER OF (gram) PARTICLES GASS VOLUME STP ( liter ) Hal.: 16 Isi dengan Judul Halaman Terkait

Isi dengan Judul Halaman Terkait THANK YOU Hal.: 17 Isi dengan Judul Halaman Terkait