Question

Chemical Reactions & Equations

System 1: Reaction of Sodium Metal with Water

Observations: solution start to produce vapor and eventually catches fire

Reaction Type:

Balanced Equation: (Na with H2O)

Reaction in words:

The hydrogen gas produced in the reaction can ignite in the presence of oxygen gas in the air. If you observed flames above, it was likely due to this reaction

Reaction Type:

Balanced Equation: (hydrogen gas with oxygen gas):

System 2: Combustion Reactions of Methane (CH4) and Cellulose (empirical formula=C6H10O5)

Procedure: Light a Bunsen burner flame. Observe. Light a wood splint (primarily cellulose fibers). Observe. Extinguish the flames. Complete the table below.

Observations: Flame increases in size in presence of wood splint

Balanced Equation: (combustion of methane)

Balanced Equation: (combustion of cellulose)

Reaction in words: (combustion of cellulose)

System 3: Magnesium in Hydrochloric Acid Procedure: Place ~ 3 mL of 1M HCl solution in a test tube. Drop a small strip of magnesium metal (1-2 cm) into the tube. Observe. Complete the table below.

Observations: starts to bubble and becomes warm. strip starts to dissolve

Reaction Type:

Balanced Equation:

Reaction in words:

System 4: Mixing aqueous solutions Procedure: Put 1-2 mL of 0.1M potassium iodide solution into each of two test tubes. Add 1-2 mL of lead (II) nitrate to one. Add 1-2 mL of zinc nitrate to the other. Observe. Complete the table below. Note that only one test tube is likely to have a reaction. After the observations are made, fill out the rest of the table for the reaction that takes place.

Observations: (for both test tubes): test tube with lead (ii) nitrate turned yellow. no change/reaction to zinc test tube

Reaction Type:

Balanced Equation:

Reaction in words:

Net Ionic Equation:

How might you have predicted which would have resulted in a chemical reaction? Are your observations consistent with that prediction?

System 5: Solutions and Metals Procedure: Put 2-3 mL of 0.1M copper (II) sulfate solution in a test tube. Drop a small strip of magnesium metal (1-2 cm) into the tube. Put 2-3 mL of 0.1M magnesium nitrate solution in a test tube. Add a small piece of copper metal. Observe both test tubes at 5 minutes and again at 10 minutes. Complete the table below. Note that only one test tube is likely to have a reaction. After the observations are made, fill out the rest of the table for the reaction that takes place.

Observations: (for both test tubes): magnesium test tube no change. copper test tube started to bubble and black solids piece were floating at 5mins sank to bottom at 10 mins.

Reaction Type:

Balanced Equation:

Reaction in words:

Net ionic equation:

How might you have predicted which would have resulted in a chemical reaction? Are your observations consistent with that prediction?

Answer 1