標題:
發問:
The formula for hydrated iron(II) sulphate is FeSO4．xH2O.On strong heating, 20.1g of the sulphate produces 9.1g of water.What is the value of x? (Relative atomic masses: H=1 O=16 S=32.1 Fe=56)
最佳解答:
FeSO4．xH2O → FeSO4 + xH2O no. of mole of FeSO4．xH2O used = 20.1/(56+32.1+16*4+x(2+16))=20.1/(152.1+18x) no. of mole of H2O produced = 9.1/(2+16) = 9.1/18 from the equation, mole ratio of FeSO4．xH2O : H2O = 1 : x so (20.1/(152.1+18x))/(9.1/18) = 1/x x = 6.99 (3 sig. fig.) = 7 so x = 7
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Reacting mass發問:
The formula for hydrated iron(II) sulphate is FeSO4．xH2O.On strong heating, 20.1g of the sulphate produces 9.1g of water.What is the value of x? (Relative atomic masses: H=1 O=16 S=32.1 Fe=56)
最佳解答:
FeSO4．xH2O → FeSO4 + xH2O no. of mole of FeSO4．xH2O used = 20.1/(56+32.1+16*4+x(2+16))=20.1/(152.1+18x) no. of mole of H2O produced = 9.1/(2+16) = 9.1/18 from the equation, mole ratio of FeSO4．xH2O : H2O = 1 : x so (20.1/(152.1+18x))/(9.1/18) = 1/x x = 6.99 (3 sig. fig.) = 7 so x = 7
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