Our Next Lab:

Our Next Lab:

Relating Moles to

Coefficients of a

Chemical Reaction

Our Next Lab:Solid iron is added to a

solution of copper(II) sulfate, producing solid copper and a solution of iron(?) sulfate.

Our Next Lab:Solid iron is added to a

solution of copper(II) sulfate, producing solid copper and a solution of iron(?) sulfate.

What is the formula for copper(II) sulfate?

Our Next Lab:Solid iron is added to a

solution of copper(II) sulfate, producing solid copper and a solution of iron(?) sulfate.

What is the formula for copper(II) sulfate?

What is the formula for iron(II) sulfate?

Our Next Lab:Solid iron is added to a

solution of copper(II) sulfate, producing solid copper and a solution of iron(?) sulfate.

What is the formula for copper(II) sulfate?

What is the formula for iron(II) sulfate?

What is the formula for iron(III) sulfate?

Our Next Lab:Fe(s) + CuSO4(aq) →

FeSO4(aq) + Cu(s) or

Fe(s) + CuSO4(aq) → Fe2(SO4)3(aq) + Cu(s)

Our Next Lab:Fe(s) + CuSO4(aq) →

FeSO4(aq) + Cu(s) or

Fe(s) + CuSO4(aq) → Fe2(SO4)3(aq) + Cu(s)

What kind of reaction is this?

Our Next Lab:Fe(s) + CuSO4(aq) →

FeSO4(aq) + Cu(s) or

Fe(s) + CuSO4(aq) → Fe2(SO4)3(aq) + Cu(s)

synthesis, decomposition,

single replacement, double replacement,

or combustion?

Our Next Lab:Fe(s) + CuSO4(aq) →

FeSO4(aq) + Cu(s) or

Fe(s) + CuSO4(aq) → Fe2(SO4)3(aq) + Cu(s)

synthesis, decomposition,

single replacement, double replacement,

or combustion?

Our Next Lab:___Fe(s) + ___CuSO4(aq) →

___FeSO4(aq) + ___Cu(s) or

___Fe(s) + ___CuSO4(aq) → ___Fe2(SO4)3(aq) + ___Cu(s)

Are the equations balanced?

Our Next Lab:_1_Fe(s) + _1_CuSO4(aq) →

_1_FeSO4(aq) + _1_Cu(s) or

_2_Fe(s) + _3_CuSO4(aq) → _1_Fe2(SO4)3(aq) + _3_Cu(s)

Are the equations balanced?

Our Next Lab:_1_Fe(s) + _1_CuSO4(aq) →

_1_FeSO4(aq) + _1_Cu(s) or

_2_Fe(s) + _3_CuSO4(aq) → _1_Fe2(SO4)3(aq) + _3_Cu(s)

We will experimentally determine the correct formula for iron

sulfate.

Step 1:Mass a clean dry 100 ml.beaker.

Step 2:Mass a clean dry 100 ml.beaker.Measure 0.06 moles CuSO4 crystals and add to beaker.

Step 2:Mass a clean dry 100 ml.beaker.Measure 0.06 moles CuSO4 crystals and add to beaker.

How many grams is that?

Step 3:Mass a clean dry 100 ml.beaker.Measure 0.06 moles CuSO4 crystals and add to beaker.Measure 50.0 ml.H2O and add to beaker.

Step 4:Mass a clean dry 100 ml.beaker.Measure 0.06 moles CuSO4 crystals and add to beaker.Measure 50.0 ml.H2O and add to beaker.Heat gently to just below boiling.DO NOT ALLOW IT TO BOIL!!!

Step 5:Mass a clean dry 100 ml.beaker.Measure 0.06 moles CuSO4 crystals and add to beaker.Measure 50.0 ml.H2O and add to beaker.Heat gently to just below boiling.DO NOT ALLOW IT TO BOIL!!!Heat until crystals dissolve.

Step 6:While one partner is dissolving the crystals, another partner should measure out 0.04 moles of iron filings.

Step 6:While one partner is dissolving the crystals, another partner should measure out 0.04 moles of iron filings.

How many grams is that?

Step 7:While one partner is dissolving the crystals, another partner should measure out 0.04 moles of iron filings.Add the iron filings small amounts at a time to the copper sulfate solution, stirring constantly. Then let it sit for 10 minutes while the reaction proceeds. Record your observations.

Step 8:Decant the liquid into a 250 ml beaker. Do not disturb the solid at the bottom of the 100 ml beaker.

Step 9:Decant the liquid into a 250 ml beaker. Do not disturb the solid at the bottom of the 100 ml beaker.Add about 10 ml. water, stir to wash off the solid. Let it settle and then decant. Repeat.

Step 10:Decant the liquid into a 250 ml beaker. Do not disturb the solid at the bottom of the 100 ml beaker.Add about 10 ml. water, stir to wash off the solid. Let it settle and then decant. Repeat.Spread the solid out on the bottom of the beaker and leave to dry.

Step 11:The next day (or the next class period) mass the beaker and the dry copper metal.

Careful!Don’t let the liquid boil.Measure precisely.Decant carefully.Wash thoroughly.Check your calculations.