Zinc and Hydrochloric Acid Reactions

This video tutorial explains the reaction between zinc metal and aqueous hydrochloric acid. It covers predicting reaction products, balancing chemical equations, and writing net ionic equations. The video discusses the single replacement reaction where zinc displaces hydrogen, forming zinc chloride and hydrogen gas. It explains oxidation and reduction processes, emphasizing electron transfer. The activity series of metals is used to determine zinc's ability to displace hydrogen. Finally, the video demonstrates balancing the chemical equation and identifying spectator ions to write the net ionic equation.

What type of reaction occurs between zinc metal and hydrochloric acid?

• Single replacement reaction

• Decomposition reaction

• Synthesis reaction

• Double replacement reaction

What is the charge of a zinc ion in the reaction with hydrochloric acid?

• 1-

• 1+

• 2-

• 2+

What gas is produced when zinc reacts with hydrochloric acid?

• Oxygen

• Nitrogen

• Chlorine

• Hydrogen

In the reaction, what happens to zinc?

• It forms a precipitate

• It remains unchanged

• It is oxidized

• It is reduced

Which of the following metals cannot displace hydrogen from hydrochloric acid?

• Zinc

• Copper

• Magnesium

• Aluminum

What is the purpose of consulting the activity series of metals?

• To measure the temperature change in reactions

• To determine the solubility of metals

• To predict the color change in reactions

• To check if a metal can displace another in a reaction

What is the first step in balancing the chemical equation for the reaction?

• Balance the oxygen atoms

• Balance the chloride ions

• Balance the zinc atoms

• Balance the hydrogen atoms

What is the net ionic equation for the reaction between zinc and hydrochloric acid?

• Zn + Cl- → ZnCl2

• H+ + Cl- → HCl

• Zn + 2H+ → Zn2+ + H2

• Zn2+ + 2Cl- → ZnCl2

What are spectator ions in a chemical reaction?

• Ions that participate in the reaction

• Ions that form a precipitate

• Ions that change their oxidation state

• Ions that remain unchanged on both sides of the equation

Why are chloride ions considered spectator ions in this reaction?

• They do not change during the reaction

• They are oxidized

• They are reduced

• They form a solid precipitate