Mg(s) + HCl(aq) −→ MgCl2(aq) + H2(g). What mass of HCl is consumed by the reaction of 2.28 mol of magnesium?
Answer in units of g

166 g HCl

General Formulas and Concepts:

Math

Pre-Algebra

Order of Operations: BPEMDAS

BracketsParenthesisExponentsMultiplicationDivisionAdditionSubtractionLeft to Right

Chemistry

Stoichiometry

Reading a Periodic TableBalancing EquationsUsing Dimensional AnalysisExplanation:

Step 1: Define

[RxN - Unbalanced] Mg (s) + HCl (aq) → MgCl₂ (aq) + H₂ (g)

[RxN - Balanced] Mg (s) + 2HCl (aq) → MgCl₂ (aq) + H₂ (g)

[Given] 2.28 mol Mg (s)

Step 2: Identify Conversions

[RxN] 1 mol Mg = 2 mol HCl

Molar Mass of H - 1.01 g/mol

Molar Mass of Cl - 35.45 g/mol

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

Step 3: Stoichiometry

Set up:                               Multiply:                            

Step 4: Check

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

166.258 g HCl ≈ 166 g HCl

Heat is involved in chemical change in two ways; chemical changes either result in heat being added to or removed from an object, and chemical changes require a certain amount of heat before they can take place.

Hbr dissociates to form h+ and br-ca(oh)2 dissociates to form ca2+ and 2oh-the h+ and oh- react to form waterassuming the reactants are dissolved in water, the net reaction is h+ + oh- —> h2oif you’re asked to show all components of the reaction, the complete reaction is 2hbr + ca(oh)2 —> cabr2 + 2h2o