Problem: A sample of a substance with the empirical formula XBr2 weighs 0.5675 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 0.9465 g. The chemical reaction is XBr2 + 2AgNO3 → 2AgBr + X(NO3)2 (a) Calculate the formula mass of XBr2.  (b) Calculate the atomic mass of X.  

🤓 Based on our data, we think this question is relevant for Professor Smeureanu's class at HUNTER.

FREE Expert Solution
View Complete Written Solution
Problem Details

A sample of a substance with the empirical formula XBr2 weighs 0.5675 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 0.9465 g. The chemical reaction is 

XBr2 + 2AgNO3 → 2AgBr + X(NO3)2 

(a) Calculate the formula mass of XBr2.  

(b) Calculate the atomic mass of X.  

Learn this topic by watchingStoichiometry Concept Videos
All Chemistry Practice Problems Stoichiometry Practice Problems
Q.According to the following reaction, how many grams of chlorine gas are necessary to form 0.837 moles iron(HI) chloride? iron (s) + chlorine (g) → iro...
Q.Be sure to answer all parts. Calculate the mass of each product formed when 506 g of silver sulfide reacts with excess hydrochlorie acid: Ag2S (s) + H...
Q.How many molecules (not moles) of NH3 are produced from 4.95 x 10-4 g of H2? Express your answer numerically as the number of molecules.
Q.A 1.560 - g sample of the alcohol CH3CHOHCH2CH3 is burned in an excess of oxygen. Part AWhat mass of CO2 should be obtained? Express your answer using...
See all problems in Stoichiometry