A chemist has a sample of an unknown metal. When the chemist reacts this metal with Cl2, the water soluble compound MCl2 is produced. The reaction continues until the Cl2 is consumed. In order to identify the unknown metal, the chemist isolates the MCl2 that is produced. The chemist records the mass measurements of all chemicals throughout the reaction in the data table below. Mass of Empty Beaker 123.41 g Mass of Beaker and Unknown Metal Solid 138.31 g Mass of Beaker, Unknown Metal Solid, and Cl2, before the reaction has occured 141.31 g Mass of MCl2 only, after the reaction has occurred 8.82 g a) Given the metal is in excess, calculate the number of moles of Cl2 that reacted. b) Calculate the molar mass of the unknown metal.
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A chemist has a sample of an unknown metal. When the chemist reacts this metal with Cl2, the water soluble compound MCl2 is produced. The reaction continues until the Cl2 is consumed.
In order to identify the unknown metal, the chemist isolates the MCl2 that is produced. The chemist records the mass measurements of all chemicals throughout the reaction in the data table below.
| Mass of Empty Beaker | 123.41 g |
| Mass of Beaker and Unknown Metal Solid | 138.31 g |
| Mass of Beaker, Unknown Metal Solid, and Cl2, before the reaction has occured | 141.31 g |
| Mass of MCl2 only, after the reaction has occurred | 8.82 g |
a) Given the metal is in excess, calculate the number of moles of Cl2 that reacted.
b) Calculate the molar mass of the unknown metal.
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