Given the equation 2Si(s) + 2Cl2(g) –> 2SiCl2(g) + 687 kJ, how much heat is produced when 106 g of Cl2 react?

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Given the equation 2Si(s) + 2Cl2(g) –> 2SiCl2(g) + 687 kJ, how much heat is produced when 106 g of Cl2 react?

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Delwyn 1 week 2021-07-22T23:23:22+00:00 1 Answers 3 views 0

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    2021-07-22T23:24:33+00:00

    Answer:

    514 kJ

    General Formulas and Concepts:

    Atomic Structure

    • Reading a Periodic Table
    • Elements
    • Compounds
    • Moles

    Stoichiometry

    • Analyzing Reactions rxn
    • Using Dimensional Analysis

    Explanation:

    Step 1: Define

    Identify

    [Given] rxn (balanced): 2Si (s) + 2Cl₂ → 2SiCl₂ (g) + 687 kJ

    [Given] 106 g Cl₂

    [Solve] kJ heat

    Step 2: Identify Conversions

    [rxn] 2 mol Cl₂ → 687 kJ

    [PT] Molar Mass of Cl: 35.45 g/mol

    Molar Mass of Cl₂: 2(35.45) = 70.9 g/mol

    Step 3: Stoichiometry

    1. [DA] Set up:                                                                                                       \displaystyle 106 \ g \ Cl_2(\frac{1 \ mol \ Cl_2}{70.9 \ g \ Cl_2})(\frac{687 \ kJ}{2 \ mol \ Cl_2})
    2. [DA] Divide/Multiply [Cancel out units]:                                                           \displaystyle 513.554 \ kJ

    Step 4: Check

    Follow sig fig rules and round. We are given 3 sig figs.

    513.554 kJ ≈ 514 kJ

    Topic: AP Chemistry

    Unit: Thermochemistry

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