Man-Made Climate Change in Your Kitchen!

We can simulate the atmosphere Dr. Romm fears with simple equipment, no million Dollar grant, advanced degrees, UN IPCC or EPA approval needed. Here’s how to create your own “climate change” experiment at home to prove climate change is a liberal myth!

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We do need: (1) two laboratory “stick” thermometers, (2) 650 ml of pure water, (3) 1/8th tsp. of baking soda, (4) a few drops of Distilled White Vinegar, (5) a medicine dropper (6) two 2.5 liter soda bottles that must be clear, not tinted and “2.5 liters” not the two or three liters. Most are 2.5 liters and sell for less than $2.00. And, you get to drink the soda!

Lab thermometers are $2.39 on Ebay, two for less than $10 with postage. Baking soda and White Distilled Vinegar are home pantry items. Medicine droppers are found in most homes or $1.00 each in a drug store. Medicine droppers produce 20 drops per milliliter, ml, per industry standards for use by pharmacists, physicians and patients to prepare and dispense medicine.

Thermometer accuracy is confirmed by putting them into a tall glass filled with ice and water. They should say 0° Celsius. Return any not showing that after two minutes in a glass filled with ice and water for ten minutes.

Plastic bottle caps are drilled by a Phillips screwdriver with a 1/4 inch shaft. Hold it an inch over a candle flame for 30 seconds. The handle insulates so you can hold it. Push the hot tip through the plastic cap in the center to leave a hole just large enough for a thermometer. Both thermometers are pushed into caps three inches while the plastic is soft. On cooling they will freeze into place, but can be removed by careful twisting, with your thumb and forefinger very near the cap applying gentle twisting with patience.

The volume of “2.5 liter” soda bottles is actually 2,725 ml. Use bottled or well water to avoid municipal water chlorine and fluorine. Put 325 ml, into each for a net air volume of 2400 ml over water. This simulates Earth’s air very well as 71% of the planet is covered by water, 14% is green putting almost as much water vapor into air as do the seas. Only 15% is barren.

2,400 ml is 1/10th “molar volume” of air at 20° Celsius, a common room temperature in the United States. “Molar” is from “mole,” a contraction of “molecular” meaning the volume of a gas with a mass of one molecular weight in grams. 28 grams of nitrogen, N2, for example, as each nitrogen is 14 atomic weight units and there are two of them in “N2.”

To determine how much baking soda and vinegar to use for creating a test atmosphere we use chemical relationships based on sums of relative weights of the elements in the compounds in a reaction to produce CO2.

Hydrogen, the lightest element, is defined as one atomic weight unit that has two atoms in each molecule so it has a “mole” weight of two grams and gas volume of 24,000 ml at 20 Celsius degrees. Gas volume is the same for 32 grams of oxygen, O2. 28 grams of nitrogen, N2, or 44 grams of CO2, carbon dioxide. Every gas has a “mole” volume of 24,000 ml at 20°C and each has the same number of molecules.

Air is a mixture of three principle gases and eight “trace” gases, meaning we know they are present, but they are of no consequence. CO2 is in that class having only 0.04% and to be of consequence in the atmosphere it must have more than one percent per the rules of the American Meteorological Society, the association of real climate scientists.

The only gas changing quantity in air is water vapor as it can exist as a solid, liquid or gas in the range of temperatures on Earth. When it condenses the volume shrinks by a factor of 1200. No other atmospheric gas does that. It absorbs energy from sunlight far better than any gas in air, seven times more than CO2 per molecule. Nitrogen and oxygen capture little infrared energy.

In our atmospheric simulator we add known quantities of CO2 to the present day 400 ppm with baking soda, NaHCO3, and White Distilled Vinegar, that is five percent acetic acid, CH3COOH, using the reaction:

NaHCO3 + CH3COOH —> CH3COONa + H2O + CO2g

84g 60g 82g 18g 44g

Sodium bicarbonate, NaHCO3, plus acetic acid, CH3COOH, combine to make sodium acetate, water and carbon dioxide gas, 44 g of CO2 is 24,000 ml, at 20°C, but we want a tiny amount. The task is getting it precisely.

Today air has 0.04% CO2 that is 9.60 ml per molar volume of air by 24,000 x 0.0004 = 9.60 ml or 0.960 ml/0.1 mole for our 1/10th molar volume bottle.

Where we want to add 510 ppm, or 510/1,000,000 = 0.00051 decimal parts of 2400 ml CO2 per 2400 x 0.00051 = 1.22 ml of CO2 we need only add that same number of moles of NaHCO3 and CH3COOH to make that much CO2 per the equation for the “2100” bottle.

0.00051 mole of NaHCO3 is 84 x 0.00051 = 0.0428g, an impossibly small quantity to weigh in a lab, but it is 60 x 0.00051 = 0.0306g of acetic acid which we can measure as it is in a 5% solution!

Baking soda, sodium bicarbonate weighs nine grams per teaspoon. Adding half a quarter teaspoon measure will be about one gram in solution which is 32 times more than we need, but we can control the amount of CO2 it nakes by limiting the acetic acid, White Distilled Vinegar.

White Distilled Vinegar is 5% acetic acid containing 50 grams per liter or (50g/60 g/mole) = 0.833 mole/liter or 0.000833 moles/ml or 0.000833 mole/ml/20 drop/ml = 0.0000417 mole/drop which would produce 0.0000417 moles of gas for each drop of household vinegar added to the solution of NaHCO3. This is the key to our accuracy.

Where we need 0.00051 mole of gas we can use 0.00051/0.0000417 = 12.2 drops of White Distilled Vinegar to get the acetic acid to make the 1.22 ml of CO2 we need to make the air of 2100 AD Dr. Romm fears. 12 drops will get us to within 98% of the target, installing them the day before the test to be sure everything has reacted.

In the morning the 2016 air has 400 ppm of CO2 and the 2100 AD has 959 ppm CO2. The test can be done outside, but we favor a south facing window sill as these bottles are easily tipped by an errant breeze and window glass passes infrared, IR, energy easily. When the sun is low very little IR comes through all the air with a low sun angle and little heating happens.

After 10 AM the sun angle is above 45 degrees and IR passes easily through less damp air which absorbs it. Be sure the thermometers are shaded from direct sun with aluminum foil “hats” so you are reading temperature of air in the flasks and not direct sunlight.

The best days for these experiments are those with clear air and no clouds as moist air and clouds absorb lots of IR. Avoid overcast or rainy days.

Make a chart to track temperatures hourly. You will see they rise through the noon hour, peak at 1:00 PM, flatten and decline as sunlight is passing through more air as it approaches the horizon.

Dr. Romm predicts air in the “2100 AD” bottle will heat very dramatically between 9:00 AM and noon and will be at, or over 37º C, but it does not happen! What does this mean?

Experiments like this do not lie, but let’s go one step further and take a cue from the real atmospheric scientists, meteorologists. They say “trace gases,” those with less than 1%,have no significance in the physics of air. What if we bring CO2 up to a level of significance, over 1%?

One percent CO2 is 10,000 ppm, ten times what Dr. Romm fears and where each drop of vinegar adds 575 ppm we need (10,000 – 975)/ 575 = 15.7 drops, call it 16. So we add 16 drops and wait overnight to be sure all has reacted and what do we see when we put it in the sunlight?

Instead of capturing heat turning the bottle into an oven the 10,000 ppm our greater than 1% CO2 bottle drops in temperature! Why should that be?

CO2 forces water vapor out of air changing it to water, per the Le Chatelier Principle which says: “When a system at equilibrium incurs a change of pressure, volume, concentration or temperature it counteracts that change to establish a new equilibrium.”

Where air has only two molecules heating it our Le Chatelier expression is:

[H2Og] x [CO2g] = Kt

[H2Ol]

The “[” brackets mean “moles/liter,” “g” is for gas or vapor, “l” is for liquid, “K” means “Constant” and “t” is temperature in degrees Kelvin which are degrees Celsius + 273. Water is the only participant that can change from gas to liquid; CO2 cannot and we can solve for water vapor to determine why the system behaves as it does. Revising the equation to solve for water vapor yields:

[H2Og] = _[H2Ol] x Kt_

[CO2]

Using the values of 0.03 moles of H2O water vapor, 0.0004 moles of CO2 and 55.5 mole/liter for liquid water, Kt = 2.1 x 10^-7 the equation shows the molarity of water vapor for 2016 air with 400 ppm CO2 is 0.04 mole and with 1% CO2 it is only 0.00117 mole H2O. This is a reduction in water vapor of 99.9% and H2O vapor is the primary IR heater of air! Therefore, increasing CO2 cools the atmosphere!