Chemical Reactions and Equations_LS_5

When Lead Nitrate reacts with potassium iodide, Yellow precipitate of ............. is formed

Reaction Taking

place is as follow:-KI(aq) + Pb(NO3)2(aq) → KNO3(aq) + PbI2(s)

• PbI₂

• KNO₃

• Pb(NO₃)₂

• PbIO₃

Name this compound:

KI

• potassium iodide

• potassium iodite

• iodine potasside

• potassium iodine

Give two characteristics of the chemical reaction which occurs on adding potassium iodide solution to lead nitrate solution. What is the first statement of the audio clip?

• Formation of yellow precipitate.

• The reaction color is changed from colorless to yellow.

• Reaction Taking

  place is as follow:-KI(aq) + Pb(NO3)2(aq) → KNO3(aq) + PbI2(s)

Give two characteristics of the chemical reaction which occurs on adding potassium iodide solution to lead nitrate solution. What is the second statement of the audio clip?

• Formation of yellow precipitate.

• The reaction color is changed from colorless to yellow.

• Reaction Taking

  place is as follow:-KI(aq) + Pb(NO3)2(aq) → KNO3(aq) + PbI2(s)

Give two characteristics of the chemical reaction which occurs on adding potassium iodide solution to lead nitrate solution. What is the third statement of the audio clip?

• Formation of yellow precipitate.

• The reaction color is changed from colorless to yellow.

• Reaction Taking

  place is as follow:-KI(aq) + Pb(NO3)2(aq) → KNO3(aq) + PbI2(s)

What is a chemical equation?

• Describes the number of elements in a compound.

• One or two letters that represent the elements on the periodic table.

• The number to the lower right of an element that shows the number of atoms bonded.

• A written description of a chemical reaction.

Chemical reactions

• create and destoy atoms

• only occurs outside living organisms

• occurs only in living organisms

• produce new substances

Chemical equations

• give directions for naming compounds

• describe only biological changes

• describe chemical reactions

• show how to write formulas

At the end of chemical reactions, what is the total mass of the reactants compared to the total mass of the products?

• the product is doubled
• the product is half the mass of the reactants
• the mass is the same
• the mass changes depending on the reaction

Magnesium can be burned in air to produce solid magnesium oxide.

• 2Mg(s) + O₂(g)→ 2MgO(s)
• Mg(s) + O(g) → MgO(s)
• 2Mg(s) + CO₂(g) → 2MgO(s) + C(s)
• 2Mg(s) + O₂(g) → Mg₂O₂(s)