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    zinc chloride can be prepared in the laboratory by the reaction between zinc oxide and hydrochloric acid . the equation is :

    ZnO + 2HCl = ZnCl2 + H20

    A 3.56g sample of pure zinc oxide was added to 0.0830 mol of hydrochloric acid. Calculate the maximum mass of anyhdrous zinc chloride that could be obtained from the products of this reaction .
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    I would use the equation Mass= Mr x Mole. Find out the number of moles of zinc oxide using this equation.
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    Find the limiting reagent. Convert grams into moles for zinc chloride.
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    The Rfm of ZnCl2 = 136.4
    as there is a molar ratio of 2:1 of HCL and ZnCl2 and there are 0.083 moles of HCl, there are 0.0415 moles of ZnCl2
    Mass= RFM x Moles = 136.4 x 0.0415 = 5.6606 g of Anhydrous Zinc Chloride.
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    (Original post by ArcaneMists)
    Find the limiting reagent. Convert grams into moles for zinc chloride.
    (Original post by ASHLEYTMK)
    The Rfm of ZnCl2 = 136.4
    as there is a molar ratio of 2:1 of HCL and ZnCl2 and there are 0.083 moles of HCl, there are 0.0415 moles of ZnCl2
    Mass= RFM x Moles = 136.4 x 0.0415 = 5.6606 g of Anhydrous Zinc Chloride.
    oh ok thanks guys
 
 
 
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