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PlsHelpMeh3401
21.01.2020 •
Chemistry
Ferrophosphorus (fe2p) reacts with pyrite (fes2) producing iron(ii) sulfide and a compound that is 27.87% p and 72.13% s by mass and has a molar mass of 444.56 g/mol.
a. determine the empirical and molecular formulas of this compound.
b. empirical formula: molecular formula:
c. write a balanced chemical equation for this reaction. do not include phases.
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Ответ:
The molecular formula of the compound =![P_4S_{10}](/tpl/images/0463/4499/9e919.png)
The empirical formula of the compound =![P_2S_{5}](/tpl/images/0463/4499/4f9b9.png)
The balanced chemical equation for this reaction:
Explanation:
Compound that is 27.87% P and 72.13% S by mass and has a molar mass of 444.56 g/mol.
Molar mass of compound = 444.56 g/mol
Number of phosphorus atom = x
Number of sulfur atom = y
Atomic mass of phosphorus 31 g/mol
Atomic mass of sulfur = 32 g/mol
Percentage of element in compound :
Phosphorus :
x = 4
Sulfur :
y = 10
The molecular formula of the compound =![P_4S_{10}](/tpl/images/0463/4499/9e919.png)
Empirical formula is the simplest chemical formula which depicts the whole number of atoms of each element present in the compound.
The empirical formula of the compound =![P_2S_{5}](/tpl/images/0463/4499/4f9b9.png)
The balanced chemical equation for this reaction:
Ответ:
what kinda school u go to lolll