Calcium chloride is produced as the product of a chemical reaction.
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What is the formula of calcium chloride?
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What is the percentage mass of each of the elements in a molecule of
calcium chloride?
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If the sample contains \(\text{5}\) \(\text{g}\) of calcium chloride,
what is the mass of calcium in the sample?
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How many moles of calcium chloride are in the sample?
Solution not yet available
\(\text{13}\) \(\text{g}\) of zinc combines with \(\text{6,4}\) \(\text{g}\) of
sulphur.
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What is the empirical formula of zinc sulphide?
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What mass of zinc sulphide will be produced?
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What is the percentage mass of each of the elements in zinc sulphide?
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The molar mass of zinc sulphide is found to be \(\text{97,44}\)
\(\text{g·mol$^{-1}$}\). Determine the molecular formula of
zinc sulphide.
Solution not yet available
A calcium mineral consisted of \(\text{29,4}\%\) calcium, \(\text{23,5}\%\)
sulphur and \(\text{47,1}\%\) oxygen by mass. Calculate the empirical formula
of the mineral.
Solution not yet available
A chlorinated hydrocarbon compound was analysed and found to consist of
\(\text{24,24}\%\) carbon, \(\text{4,04}\%\) hydrogen and \(\text{71,72}\%\)
chlorine. From another experiment the molecular mass was found to be
\(\text{99}\) \(\text{g·mol$^{-1}$}\). Deduce the empirical and molecular
formula.
Solution not yet available
Magnesium sulphate has the formula \(\text{MgSO}_{4}.\text{nH}_{2}\text{O}\). A
sample containing \(\text{5,0}\) \(\text{g}\) of magnesium sulphate was heated
until all the water had evaporated. The final mass was found to be
\(\text{2,6}\) \(\text{g}\). How many water molecules were in the original
sample?
Solution not yet available