Fundamentals of Chemistry by R. Elsair

By R. Elsair

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6 Components of a mass spectrometer. 7 Detection As the magnetic field is gradually increased, the separated ions are detected and this signal sent to a data system where the m/e ratios are stored together with their relative abundance for presentation in the format of a spectrum. 8 Exercise - A naturally occurring sample of mercury produces this mass spectrum How many possible isotopes of mercury are there? Which isotope is most abundant? Estimate the RAM of naturally occurring mercury. Calculate the RAM accurately.

Equal concentration? A has same concentration as C; B has same concentration as D. • Equal number of moles of solute? B has same number of moles of solute as C. 4 Most useful unit of concentration - Molarity The number of moles is always more important than the mass (as the reaction equations tell us how many moles will react together, not the number of grams). So the usual units for concentration are moles per cubic decimetre (mol dm3). e. 1 Molar”). You may still find the equivalent term moles per litre (mol L-1) still used.

This gives the molar ratio of the elements present. Divide throughout by smallest number obtained to find the empirical formula. M. 1% O. M. of the compound is 90. Calculate the empirical and molecular formula. 2 Question Calculate the empirical formula of a compound which contains 63% Mn and 37% O. 7 Theoretical yield The yield is the amount of product made in a reaction. Theoretical yield is the amount of product that would be made if there were no experimental errors in the experiment. A chemical equation expresses the ratio of the number of moles of reactants and products (the stoichiometry of the equation).

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