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9 June, 13:12

If 1.0g of rubidium and 1.0 g of bromine are reacted what will be left in measurable amounts in the reaction

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  1. 9 June, 15:17
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    0.0639 g of Br₂ will be left

    Explanation:

    The balance chemical equation for given synthesis reaction is,

    2 Rb + Br₂ → 2 RbBr

    Step 1: Calculate Moles of each reactant for given masses as;

    Moles of Rb = 1 g : 85.46 g/mol

    Moles of Rb = 0.0117 moles

    Similarly,

    Moles of Br₂ = 1 g : 159.80 g/mol

    Moles of Br₂ = 0.00625 moles

    Step 2: Find reactant in Excess as:

    According to equation,

    2 moles of Rb reacted with = 1 mole of Br₂

    So,

    0.0117 moles of Rb will react with = X moles of Br₂

    Solving for X,

    X = 0.0117 mol * 1 mol / 2 mol

    X = 0.00585 mol of Br₂

    While, as calculated above we are provided with 0.00625 moles of Br₂. Therefore, Br₂ is in excess and the excess amount is calculated as,

    = Given Moles - Consumed Moles

    = 0.00625 moles - 0.00585 moles

    = 0.0004 moles

    Step 3: Calculate mass of excess Br₂ as:

    Mass = Moles * M. Mass

    Mass = 0.0004 mol * 159.80

    Mass = 0.0639 g of Br₂

    Note: Speaking broadly, there will be 1.93 g of RbBr along with 0.0639 g of Br₂ because RbBr is being produced and is available along with unreacted Br₂.
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