Question
Asked Mar 8, 2019
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Assuming an efficiency of 38.20%, calculate the actual yield of magnesium nitrate formed from 135.4 g of magnesium and excess copper(II) nitrate?

 

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Expert Answer

Step 1

Balance the chemical equation for the reaction is as follows:

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Step 2

Every 1 mole of magnesium metal that takes part in the reaction consumes 1 moleof copper (II) nitrate and produces 1 mole of aqueous magnesium nitrate.

Convert the mass of magnesium to moles by using the element's molar mass

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Step 3

Theoretical yield can be calcu...

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