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one reaction that produces hydrogen gas can be represented by the unbalanced chemical equation Mg(s)+HCI(aq) -> MgCI(aq)+H2(g). What is the mass of HCI is consumed by the reaction of 3.25 mol of magnesium?

User Rmbaughman
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1 Answer

8 votes

Answer:

128 g HCl

General Formulas and Concepts:

Math

Pre-Algebra

Order of Operations: BPEMDAS

  1. Brackets
  2. Parenthesis
  3. Exponents
  4. Multiplication
  5. Division
  6. Addition
  7. Subtraction
  • Left to Right

Chemistry

Atomic Structure

  • Reading a Periodic Table

Stoichiometry

  • Reaction Mole Ratios
  • Using Dimensional Analysis

Step-by-step explanation:

Step 1: Define

[RxN - Unbalanced] Mg (s) + HCl (aq) → MgCl (aq) + H₂ (g)

[RxN - Balanced] 2Mg (s) + 2HCl (aq) → 2MgCl (aq) + H₂ (g)

[Given] 3.25 mol Mg

[Solve] x g HCl

Step 2: Identify Conversions

[RxN] 2 mol Mg → 2 mol HCl

[PT] Molar Mass of H - 1.01 g/mol

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

Molar Mass of HCl - 1.01 + 35.45 = 36.46 g/mol

Step 3: Stoich

  1. [S - DA] Set up:
    \displaystyle 3.25 \ mol \ Mg((2 \ mol \ HCl)/(2 \ mol \ Mg))((36.46 \ g \ HCl)/(1 \ mol \ HCl))
  2. [S - DA] Multiply/Divide [Cancel out units]:
    \displaystyle 127.61 \ g \ HCl

Step 4: Check

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

127.61 g HCl ≈ 128 g HCl

User Gabriel Esteban
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