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Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
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Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch. 17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds

Solution: Consider the reaction between Mg(s) and HCl(aq) to produce aqueous magnesium chloride and hydrogen gas. What volume of hydrogen at STP will be produced when 12.15 g of magnesium reacts with an excess

Solution: Consider the reaction between Mg(s) and HCl(aq) to produce aqueous magnesium chloride and hydrogen gas. What volume of hydrogen at STP will be produced when 12.15 g of magnesium reacts with an excess

Problem

Consider the reaction between Mg(s) and HCl(aq) to produce aqueous magnesium chloride and hydrogen gas. What volume of hydrogen at STP will be produced when 12.15 g of magnesium reacts with an excess of hydrochloric acid?

A. 1.00 L

B. 2.00 L

C. 5.6 L

D. 11.2 L

E. 22.4 L

Solution

We will calculate the amount of hydrogen gas (H2(g)) produced from Mg(s). The limiting reactant is Mg(s) since HCl(aq) is in excess.

Let’s first write the balanced reaction equation:

Reactants:

Mg(s)
HCl(aq)

Products:

aqueous magnesium chloride

▪ magnesium → group 2A → +2 charge → Mg2+ 
▪ chloride → group 7A → -1 charge → Cl- 
*criss cross the charges of Mg2+ and Cl- and that would be the subscript of each ion
▪ aqueous magnesium chloride → MgCl2(aq)

hydrogen gas → diatomic hydrogen gas → H2(g)

View the complete written solution...