A sample of a substance with the empirical formula XBr2 weighs 0.5000 g. When it is dissolved in water and all its bromine is converted to insoluble AgBr by addition of an excess of silver nitrate, the mass of the resulting AgBr is found to be 1.0198 g. The chemical reaction is XBr2 + 2 AgNO3 → 2 AgBr + X(NO3)2 (a) Calculate the molecular mass (that is, formula mass) of XBr2.(b) Calculate the atomic mass of X and give its name andsymbol.
A sample of a substance with the empirical formula XBr2 weighs 0.5000 g. When it is dissolved in water and all its bromine is converted to insoluble AgBr by addition of an excess of silver nitrate, the mass of the resulting AgBr is found to be 1.0198 g. The chemical reaction is XBr2 + 2 AgNO3 → 2 AgBr + X(NO3)2 (a) Calculate the molecular mass (that is, formula mass) of XBr2.(b) Calculate the atomic mass of X and give its name andsymbol.
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Chapter4: Chemical Reactions
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Problem 4.88QP: A 1.345-g sample of a compound of barium and oxygen was dissolved in hydrochloric acid to give a...
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A sample of a substance with the empirical formula XBr2 weighs 0.5000 g. When it is dissolved in water and all its bromine is converted to insoluble AgBr by addition of an excess of silver nitrate, the mass of the resulting AgBr is found to be 1.0198 g. The
XBr2 + 2 AgNO3 → 2 AgBr + X(NO3)2
(a) Calculate the molecular mass (that is, formula mass) of XBr2.
(b) Calculate the
symbol.
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