[\/et_pb_text][\/et_pb_column][\/et_pb_row][et_pb_row _builder_version=”4.16″ custom_padding=”27px|0px|0|0px|false|false” global_colors_info=”{}”][et_pb_column type=”4_4″ _builder_version=”4.16″ custom_padding=”|||” global_colors_info=”{}” custom_padding__hover=”|||”][et_pb_text _builder_version=”4.16″ global_colors_info=”{}”]<\/p>\n
Bad Drink, Good Blast…<\/strong><\/span><\/h4>\nMethanol is a toxic alcohol, capable of blinding and killing those who consume it…\u00a0 hence, a BAD drink!<\/span><\/p>\nThe combustion of gaseous methanol results in the production of carbon dioxide, steam and fire!\u00a0 The expansion of the heated gases produces a characteristic “whoosh”…\u00a0 the GOOD blast!<\/span><\/p>\n2CH3<\/sub>OH(g) + 3O2<\/sub>(g) \u2192 2CO2<\/sub>(g) + 4H2<\/sub>O(g)<\/span><\/p>\nYears ago, while performing a chemistry show to celebrate the opening of the 400 building, the exhaust from this demonstration managed to knock out a ceiling tile and completely destroy a separate demonstration!<\/span><\/p>\nClick here to see the demonstration…<\/span><\/span><\/a><\/span><\/p>\n[\/et_pb_text][et_pb_text _builder_version=”4.23″ global_colors_info=”{}”]<\/p>\n
Carbide Cannon…<\/strong><\/span><\/h4>\nCalcium carbide will react with water to produce acetylene gas…<\/span><\/p>\nCaC2<\/sub>(s) + 2H2<\/sub>O(l)\u00a0\u00a0 \u2192 Ca(OH)2<\/sub>(s) + C2<\/sub>H2<\/sub>(g)<\/span><\/p>\nAcetylene gas forms explosive mixtures in air for pretty much all concentrations…<\/span><\/p>\n2C2<\/sub>H2<\/sub>(g) + 5O2<\/sub>(g)\u00a0\u00a0 \u2192\u00a0\u00a0 4CO2<\/sub>(g) + 2H2<\/sub>O(g)<\/span><\/p>\nAnd this is the basis for the carbide cannon!<\/span><\/p>\nCalcium carbide is mixed with water within a PVC tube, with the acetylene gas produced trapped by the placement of a small cup. A piezoelectric ignitor is then used to ignite the acetylene gas\u2026 producing a small bang and flash!<\/span><\/p>\nI used to perform this demonstration outside \u2013 of course, things change. A few years back I had the pleasure of seeing a half-dozen Campus Safety officers run around the building shortly after the ignition of the acetylene. They were less than pleased with the demonstration, and asked that I refrain from performing without prior notice\u2026<\/span><\/p>\nWhere\u2019s the fun in that?<\/span><\/p>\nClick here to see the demonstration…<\/span><\/span><\/a><\/span><\/p>\n[\/et_pb_text][\/et_pb_column][\/et_pb_row][et_pb_row _builder_version=”4.16″ global_colors_info=”{}”][et_pb_column type=”4_4″ _builder_version=”4.16″ custom_padding=”|||” global_colors_info=”{}” custom_padding__hover=”|||”][et_pb_text _builder_version=”4.16″ global_colors_info=”{}”]<\/p>\n
Combustible Bubbles…<\/strong><\/span><\/h4>\nNatural gas can be thought of as a mixture of combustible hydrocarbons and mercaptans (the smelly compounds!).\u00a0 As natural gas is primarily methane, we can write the chemical equation for this combustion process as…<\/span><\/p>\nCH4<\/sub>(g) + 2O2<\/sub>(g)\u00a0\u00a0 \u2192 \u00a0 CO2<\/sub>(g) + 2H2<\/sub>O(g)<\/span><\/p>\nBubbles are produced upon flowing natural gas into a soap solution.\u00a0 Imagine scooping a handful of these combustible bubbles from a beaker… and then exposing the bubbles to a flame:<\/span><\/p>\n![\"\"](\"https:\/\/staff.fullcoll.edu\/gdadson\/wp-content\/uploads\/sites\/68\/2020\/08\/Bubbles-300x122.jpg\")
<\/span><\/p>\nThat’s right!\u00a0 You have a cool demonstration that results in the complete loss of hair on your hand…<\/span><\/p>\n[\/et_pb_text][\/et_pb_column][\/et_pb_row][et_pb_row _builder_version=”4.16″ custom_padding=”27px|0px|0|0px|false|false” global_colors_info=”{}”][et_pb_column type=”4_4″ _builder_version=”4.16″ custom_padding=”|||” global_colors_info=”{}” custom_padding__hover=”|||”][et_pb_text _builder_version=”4.16″ global_colors_info=”{}”]<\/p>\n
Mighty Magnesium…<\/strong><\/span><\/h4>\nThe combustion of magnesium is a sight to behold! The incredible temperature of the reaction (in excess of 3000 degree Celsius) results in a bright white flame\u2026<\/span><\/p>\n\u00a02Mg(s) + O2<\/sub>(g)\u00a0\u00a0 \u2192\u00a0\u00a0 2MgO(s)<\/span><\/p>\nA fair amount of smoke (magnesium oxide) is also generated. I suppose this was the reason for the fire (smoke) alarm that resulted in an evacuation of two relatively large science complexes in my second year at Fullerton College.<\/span><\/p>\nYou have to wonder how it was I kept my job!<\/span><\/p>\n<\/strong>Click here to see the demonstration…<\/span><\/a><\/span><\/p>\n[\/et_pb_text][\/et_pb_column][\/et_pb_row][et_pb_row _builder_version=”4.16″ custom_padding=”27px|0px|0|0px|false|false” global_colors_info=”{}”][et_pb_column type=”4_4″ _builder_version=”4.16″ custom_padding=”|||” global_colors_info=”{}” custom_padding__hover=”|||”][et_pb_text _builder_version=”4.16″ global_colors_info=”{}”]<\/p>\n
oh sNap!<\/strong><\/span><\/h4>\nAh yes, the reaction of sodium metal with water can be incredibly exciting!<\/span><\/p>\nAs the sodium metal reacts with water, hydrogen gas is produced. The heat of the reaction ignites the hydrogen gas and, for a moment, the metal appears to be burning in water.<\/span><\/p>\n2Na(s) + 2H2<\/sub>O(l)\u00a0\u00a0 \u2192\u00a0\u00a0 2NaOH(aq) + H2<\/sub>(g)<\/span><\/p>\nIn actuality, the metal is melting as the hydrogen burns, eventually resulting in the production of enough hydrogen to generate a small explosion.<\/span><\/p>\n2H2<\/sub>(g) + O2<\/sub>(g)\u00a0\u00a0 \u2192\u00a0\u00a0 2H2<\/sub>O(g)<\/span><\/p>\nFor those that are curious, the formation of a pink solution is due to the presence of phenolphthalein indicator. The basic conditions created by the formation of (sodium) hydroxide change the solution from colorless to pink\u2026 <\/span>Good times, eh?<\/span><\/span><\/p>\n<\/span><\/span><\/p>\nClick here to see the demonstration…<\/span><\/a><\/span><\/p>\n[\/et_pb_text][\/et_pb_column][\/et_pb_row][et_pb_row _builder_version=”4.16″ custom_padding=”27px|0px|0|0px|false|false” global_colors_info=”{}”][et_pb_column type=”4_4″ _builder_version=”4.16″ custom_padding=”|||” global_colors_info=”{}” custom_padding__hover=”|||”][et_pb_text _builder_version=”4.23″ hover_enabled=”0″ global_colors_info=”{}” sticky_enabled=”0″]<\/p>\n
Thermite…<\/strong><\/h4>\nWhat can I write that could possibly add to the thrill of preparing molten iron? Right?<\/span><\/p>\nHere we have the reaction between iron(III) oxide and powdered aluminum. A piece of magnesium ribbon is used as a fuse\u2026 the burning magnesium initiates the reaction, which results in the release of significant amounts of energy (heat). The products of this reaction include molten iron, which falls from the terra cotta pot into a bucket of sand.<\/span><\/p>\nFe2<\/sub>O3<\/sub>(s) + 2Al(s)\u00a0\u00a0 \u2192\u00a0\u00a0 2Fe(l) + Al2<\/sub>O3<\/sub>(s)<\/span><\/p>\nBefore you make the mistake of thinking that this reaction is limited to the “classroom”, it was used to weld the railroad rails for the transcontinental railroad!<\/span><\/p>\nI should add that this reaction is still used to this day to weld railroad rails\u2026<\/span><\/p>\n![\"\"](\"https:\/\/staff.fullcoll.edu\/gdadson\/wp-content\/uploads\/sites\/68\/2020\/07\/redox-in-action.png\")
<\/span><\/p>\nIt\u2019s amazing what you can be paid to do these days. Right?<\/span><\/p>\nClick here to see the demonstration..<\/span>.<\/span><\/span><\/a><\/p>\n[\/et_pb_text][\/et_pb_column][\/et_pb_row][et_pb_row _builder_version=”4.23″ _module_preset=”default” global_colors_info=”{}”][et_pb_column type=”4_4″ _builder_version=”4.23″ _module_preset=”default” global_colors_info=”{}”][et_pb_text _builder_version=”4.23″ _module_preset=”default” global_colors_info=”{}”]<\/p>\n
Cellulose Nitrate\u2026<\/strong><\/span><\/h4>\nCall it nitrocellulose, cellulose nitrate, flash cotton, or just guncotton… Me? I call it a good time! Cellulose nitrate was definitely on my bucket list for demonstrations since first witnessing it many years ago at the University of Utah… and, again, at CSU Fullerton. The production of cellulose nitrate is straightforward and should be performed by all chemists at some point in their career.<\/span><\/p>\nWith sulfuric acid as a catalyst…<\/span><\/p>\n3HNO3<\/sub>\u00a0+ C6<\/sub>H7<\/sub>(OH)3<\/sub>O2<\/sub> \u2192<\/span>\u00a0C6<\/sub>H7<\/sub>(ONO2<\/sub>)3<\/sub>O2<\/sub> + 3H2<\/sub>O<\/span><\/p>\n
The combustion of gaseous methanol results in the production of carbon dioxide, steam and fire!\u00a0 The expansion of the heated gases produces a characteristic “whoosh”…\u00a0 the GOOD blast!<\/span><\/p>\n 2CH3<\/sub>OH(g) + 3O2<\/sub>(g) \u2192 2CO2<\/sub>(g) + 4H2<\/sub>O(g)<\/span><\/p>\n Years ago, while performing a chemistry show to celebrate the opening of the 400 building, the exhaust from this demonstration managed to knock out a ceiling tile and completely destroy a separate demonstration!<\/span><\/p>\n Click here to see the demonstration…<\/span><\/span><\/a><\/span><\/p>\n [\/et_pb_text][et_pb_text _builder_version=”4.23″ global_colors_info=”{}”]<\/p>\n Calcium carbide will react with water to produce acetylene gas…<\/span><\/p>\n CaC2<\/sub>(s) + 2H2<\/sub>O(l)\u00a0\u00a0 \u2192 Ca(OH)2<\/sub>(s) + C2<\/sub>H2<\/sub>(g)<\/span><\/p>\n Acetylene gas forms explosive mixtures in air for pretty much all concentrations…<\/span><\/p>\n 2C2<\/sub>H2<\/sub>(g) + 5O2<\/sub>(g)\u00a0\u00a0 \u2192\u00a0\u00a0 4CO2<\/sub>(g) + 2H2<\/sub>O(g)<\/span><\/p>\n And this is the basis for the carbide cannon!<\/span><\/p>\n Calcium carbide is mixed with water within a PVC tube, with the acetylene gas produced trapped by the placement of a small cup. A piezoelectric ignitor is then used to ignite the acetylene gas\u2026 producing a small bang and flash!<\/span><\/p>\n I used to perform this demonstration outside \u2013 of course, things change. A few years back I had the pleasure of seeing a half-dozen Campus Safety officers run around the building shortly after the ignition of the acetylene. They were less than pleased with the demonstration, and asked that I refrain from performing without prior notice\u2026<\/span><\/p>\n Where\u2019s the fun in that?<\/span><\/p>\n Click here to see the demonstration…<\/span><\/span><\/a><\/span><\/p>\n [\/et_pb_text][\/et_pb_column][\/et_pb_row][et_pb_row _builder_version=”4.16″ global_colors_info=”{}”][et_pb_column type=”4_4″ _builder_version=”4.16″ custom_padding=”|||” global_colors_info=”{}” custom_padding__hover=”|||”][et_pb_text _builder_version=”4.16″ global_colors_info=”{}”]<\/p>\n Natural gas can be thought of as a mixture of combustible hydrocarbons and mercaptans (the smelly compounds!).\u00a0 As natural gas is primarily methane, we can write the chemical equation for this combustion process as…<\/span><\/p>\n CH4<\/sub>(g) + 2O2<\/sub>(g)\u00a0\u00a0 \u2192 \u00a0 CO2<\/sub>(g) + 2H2<\/sub>O(g)<\/span><\/p>\n Bubbles are produced upon flowing natural gas into a soap solution.\u00a0 Imagine scooping a handful of these combustible bubbles from a beaker… and then exposing the bubbles to a flame:<\/span><\/p>\n That’s right!\u00a0 You have a cool demonstration that results in the complete loss of hair on your hand…<\/span><\/p>\n [\/et_pb_text][\/et_pb_column][\/et_pb_row][et_pb_row _builder_version=”4.16″ custom_padding=”27px|0px|0|0px|false|false” global_colors_info=”{}”][et_pb_column type=”4_4″ _builder_version=”4.16″ custom_padding=”|||” global_colors_info=”{}” custom_padding__hover=”|||”][et_pb_text _builder_version=”4.16″ global_colors_info=”{}”]<\/p>\n The combustion of magnesium is a sight to behold! The incredible temperature of the reaction (in excess of 3000 degree Celsius) results in a bright white flame\u2026<\/span><\/p>\n \u00a02Mg(s) + O2<\/sub>(g)\u00a0\u00a0 \u2192\u00a0\u00a0 2MgO(s)<\/span><\/p>\n A fair amount of smoke (magnesium oxide) is also generated. I suppose this was the reason for the fire (smoke) alarm that resulted in an evacuation of two relatively large science complexes in my second year at Fullerton College.<\/span><\/p>\n You have to wonder how it was I kept my job!<\/span><\/p>\n <\/strong>Click here to see the demonstration…<\/span><\/a><\/span><\/p>\n [\/et_pb_text][\/et_pb_column][\/et_pb_row][et_pb_row _builder_version=”4.16″ custom_padding=”27px|0px|0|0px|false|false” global_colors_info=”{}”][et_pb_column type=”4_4″ _builder_version=”4.16″ custom_padding=”|||” global_colors_info=”{}” custom_padding__hover=”|||”][et_pb_text _builder_version=”4.16″ global_colors_info=”{}”]<\/p>\n Ah yes, the reaction of sodium metal with water can be incredibly exciting!<\/span><\/p>\n As the sodium metal reacts with water, hydrogen gas is produced. The heat of the reaction ignites the hydrogen gas and, for a moment, the metal appears to be burning in water.<\/span><\/p>\n 2Na(s) + 2H2<\/sub>O(l)\u00a0\u00a0 \u2192\u00a0\u00a0 2NaOH(aq) + H2<\/sub>(g)<\/span><\/p>\n In actuality, the metal is melting as the hydrogen burns, eventually resulting in the production of enough hydrogen to generate a small explosion.<\/span><\/p>\n 2H2<\/sub>(g) + O2<\/sub>(g)\u00a0\u00a0 \u2192\u00a0\u00a0 2H2<\/sub>O(g)<\/span><\/p>\n For those that are curious, the formation of a pink solution is due to the presence of phenolphthalein indicator. The basic conditions created by the formation of (sodium) hydroxide change the solution from colorless to pink\u2026 <\/span>Good times, eh?<\/span><\/span><\/p>\n <\/span><\/span><\/p>\n Click here to see the demonstration…<\/span><\/a><\/span><\/p>\n [\/et_pb_text][\/et_pb_column][\/et_pb_row][et_pb_row _builder_version=”4.16″ custom_padding=”27px|0px|0|0px|false|false” global_colors_info=”{}”][et_pb_column type=”4_4″ _builder_version=”4.16″ custom_padding=”|||” global_colors_info=”{}” custom_padding__hover=”|||”][et_pb_text _builder_version=”4.23″ hover_enabled=”0″ global_colors_info=”{}” sticky_enabled=”0″]<\/p>\n What can I write that could possibly add to the thrill of preparing molten iron? Right?<\/span><\/p>\n Here we have the reaction between iron(III) oxide and powdered aluminum. A piece of magnesium ribbon is used as a fuse\u2026 the burning magnesium initiates the reaction, which results in the release of significant amounts of energy (heat). The products of this reaction include molten iron, which falls from the terra cotta pot into a bucket of sand.<\/span><\/p>\n Fe2<\/sub>O3<\/sub>(s) + 2Al(s)\u00a0\u00a0 \u2192\u00a0\u00a0 2Fe(l) + Al2<\/sub>O3<\/sub>(s)<\/span><\/p>\n Before you make the mistake of thinking that this reaction is limited to the “classroom”, it was used to weld the railroad rails for the transcontinental railroad!<\/span><\/p>\n I should add that this reaction is still used to this day to weld railroad rails\u2026<\/span><\/p>\n It\u2019s amazing what you can be paid to do these days. Right?<\/span><\/p>\n Click here to see the demonstration..<\/span>.<\/span><\/span><\/a><\/p>\n [\/et_pb_text][\/et_pb_column][\/et_pb_row][et_pb_row _builder_version=”4.23″ _module_preset=”default” global_colors_info=”{}”][et_pb_column type=”4_4″ _builder_version=”4.23″ _module_preset=”default” global_colors_info=”{}”][et_pb_text _builder_version=”4.23″ _module_preset=”default” global_colors_info=”{}”]<\/p>\n Call it nitrocellulose, cellulose nitrate, flash cotton, or just guncotton… Me? I call it a good time! Cellulose nitrate was definitely on my bucket list for demonstrations since first witnessing it many years ago at the University of Utah… and, again, at CSU Fullerton. The production of cellulose nitrate is straightforward and should be performed by all chemists at some point in their career.<\/span><\/p>\n With sulfuric acid as a catalyst…<\/span><\/p>\n 3HNO3<\/sub>\u00a0+ C6<\/sub>H7<\/sub>(OH)3<\/sub>O2<\/sub> \u2192<\/span>\u00a0C6<\/sub>H7<\/sub>(ONO2<\/sub>)3<\/sub>O2<\/sub> + 3H2<\/sub>O<\/span><\/p>\nCarbide Cannon…<\/strong><\/span><\/h4>\n
Combustible Bubbles…<\/strong><\/span><\/h4>\n
<\/span><\/p>\nMighty Magnesium…<\/strong><\/span><\/h4>\n
oh sNap!<\/strong><\/span><\/h4>\n
Thermite…<\/strong><\/h4>\n
<\/span><\/p>\nCellulose Nitrate\u2026<\/strong><\/span><\/h4>\n
![\"\"](\"https:\/\/staff.fullcoll.edu\/gdadson\/wp-content\/uploads\/sites\/68\/2024\/05\/Nitrocellulose.jpg\")
<\/p>\n![\"\"](\"https:\/\/staff.fullcoll.edu\/gdadson\/wp-content\/uploads\/sites\/68\/2024\/05\/Silver-Tree.jpg\")
<\/p>\n![\"\"](\"https:\/\/staff.fullcoll.edu\/gdadson\/wp-content\/uploads\/sites\/68\/2024\/05\/Silver-Bars.jpg\")
<\/span><\/p>\n