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kevin86604
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Mind Map on Topic 1 Quantitative Chemsitry, created by kevin86604 on 05/21/2014.

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kevin86604
Created by kevin86604 almost 11 years ago
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Topic 1QuantitativeChemsitry1.1 The mole concept and Avogadro's constant1.2 Formulas1.3 Chemical Equations1.4 Mass and gaseous Volume relationships in chemical reactions1.5 SolutionsMeasurements and uniteskg, s, K, m3, Pa or Nm-2g, min, ĖšC cm3,atmAmount ofsubstanceElementAtomsCompoundMolesMolecular FormulaRelative molecular massAvogadro's constant6.02 x 10^23 mol-1The number of particles permoleNumber of moles(n) =Mass/Molar massA mole is the amount of asubstnace which contains thesame number of chemical speciesas there are atoms in exactly 12gof the isotope carbon-12ExampleCalculate the amount of water, H20, that contains 1.80x 10^24moleculesSolutionn = N/L n= 1.80x 10-24/6.02x10^23n= 2.99 molEmperical formulaMolecular formulaBalancing equationsLimiting reactantTheoretical yieldPercentage yieldThe limiting reactant is thereactant that determines thetheoretical yield of productTheoreticall yield is the mass oramount of product producedaccording to the chemical equationexperimentalyield/theoretical yieldx 100STP= 273K and 101.3 kPa (1atm)For gas: Number of moles(n)= Volume (V) / MolarVolumeThe ideal gas equationPV=nRTEquation: CH3+O2 -> CO2 + H2OBalanced Equation: CH4+2O2 -> CO2+2H2OIt gives the ratio of the atoms of different elements in a compound.Shows the actual number of atoms of each element present in a moleculeConcentrationExample: A solution of sodium hydroxide has aconcentration of 8.00g dm-3. What is itsconcentration in mol dm-3n=m/M M=2.99+1.01+16.00 =40.00g n=8.00/40.00= 0.200[NaOH] = n/V = 0.200/1.00 = 0.200mol dm-3n=n/VDouble click this nodeto edit the textClick and drag this buttonto create a new node