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q.7 boron with atomic number 5 has two naturally occurring isotopes. calculate the percentage abundance of and from the following information.average atomic mass of boron isotopic mass of =10.0129 \mathrm{amu} isotopic mass of (ans: )

q.7 boron with atomic number 5 has two naturally occurring isotopes. calculate the percentage abundance of and from the following information.average atomic mass of boron isotopic mass of =10.0129 \mathrm{amu} isotopic mass of (ans: )

fill in the blanksthe unit of relative atomic mass isthe exact masses of isotopes can be determined byspectrograph.the phenomenon of isotopy was first discovered byempirical formula can be determined by combustion analysis for thosecompounds which have and in them.a limiting reagent is that 1 mole of glucose has of oxygen and of hydrogen. atoms molecules of . of at and pressure has stoichiometric calculations can be performed only when is obeyed.

fill in the blanksthe unit of relative atomic mass isthe exact masses of isotopes can be determined byspectrograph.the phenomenon of isotopy was first discovered byempirical formula can be determined by combustion analysis for thosecompounds which have and in them.a limiting reagent is that 1 mole of glucose has of oxygen and of hydrogen. atoms molecules of . of at and pressure has stoichiometric calculations can be performed only when is obeyed.

q.6 silver has atomic number 47 and has 16 known isotopes but two occur naturally i.e. ag-107 and . given the following mass spectrometric data calculate the average atomic mass of silver.\begin{tabular}{|l|c|c|}\hline isotopes & mass (\mathrm{amu}) & percentage abundance \\\hline { }^{107} \mathrm{ag} & 106.90509 & 51.84 \\ { }^{100} \mathrm{ag} & 108.90476 & 48.16 \\\hline\end{tabular}

q.6 silver has atomic number 47 and has 16 known isotopes but two occur naturally i.e. ag-107 and . given the following mass spectrometric data calculate the average atomic mass of silver.\begin{tabular}{|l|c|c|}\hline isotopes & mass (\mathrm{amu}) & percentage abundance \\\hline { }^{107} \mathrm{ag} & 106.90509 & 51.84 \\ { }^{100} \mathrm{ag} & 108.90476 & 48.16 \\\hline\end{tabular}

calculate the number of grams of and water produced when of are reacted with excess of . also calculate the number of molecules of water produced.

calculate the number of grams of and water produced when of are reacted with excess of . also calculate the number of molecules of water produced.

a sample of liquid consisting of carbon hydrogen and oxygen was subjected to combustion analysis. of the compound gave . determine the empirical formula of the compound.

a sample of liquid consisting of carbon hydrogen and oxygen was subjected to combustion analysis. of the compound gave . determine the empirical formula of the compound.

q.5(a) what are isotopes? how do you deduce the fractional atomic masses of elements from the relative isotopic abundance? give two examples in support of your answer.

q.5(a) what are isotopes? how do you deduce the fractional atomic masses of elements from the relative isotopic abundance? give two examples in support of your answer.