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11 Nov 2019

I need to convert carbs into grams in a food item (Hot Cheetos 15g) and then convert grams into molecules (180 g for glucose). I used Avogadroâs number (6.022x10^23) to get 5.02x10^24. NOW I need to convert molecules of glucose into a chain of glucose. Where one molecule of glucose is 1.5nm long. And then convert that nm chain into km. How would I convert this?

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4 Apr 2019

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Kendrick Taylor looks over the WAIS drill That, at least, is the theory. But temperature can be exchanged between the poles through other channels, including the atmosphere, which moves heat faster than ocean currents do, says Bo Vinther, a postdoc at the Un versity of Copenhagen, who has worked on coring projects in Greenland and Antarctica. Ifpalaeoclimatologists see long lags between temperature changes at the poles when they stack the WAIS cores up against those from Greenland, that evidence would suggest a lead role for the ocean in the bipolar seesaw. But a shorter lag would suggest a more prominent role for theatmosphere. The CO2 record will help to answer this ques tion, too: CO2 from deep in the ocean, where arge masses of organic matter have decom. posed, has a different isotopic signature from terrestrial or atmospheric CO2. Heavier CO n the WAIS record would suggest that ocean. irculation bringing up deep water was largely responsible for the bipolar seesaw. With about a kilometre of ice left to pull up, Taylor is hopeful that the core will be complete by the end of the next drilling season. But the final metres can be the toughest to dig up because the drill's descent grows longer with each segment ofextracted core. "We can get it all done next season ifevery thing goes perfectly," he says. "But this is Antarctica. Every day is a surprise Chaz Firestone Mischler, J. A etai. Glob, Biogeochem, Cycles 23, GB4024 2009 22. Bluni & Brook, E. Science 291, 09-112 (2001 3. EPICA Community Members Nature 444,195-198 (2006) For more images from the camp, VeansoG. see go nature.com Altered microbe makes biofuel In a bid to overcome the drawbacks ames Liao, a metabolic engineer and of existing biofuels, researchers have synthetic biologist at the University of engineered a bacterium that can convert California, Los Angeles a form of raw plant biomass directly into LS9's calculations, performed with the clean, road-ready diesel. help of the Argonne National Laboratory So far, biofuels have largely been limited in Illinois, show that the biodiesel that it is to ethanol, which is harder to transport preparing to market reduces greenhouse than petrol and is made from crop plants gas emissions by 85% compared with such as maize (corn) and sugarcane, standard diesel. That calculation is based putting vehicles in competition with on using Brazilian sugarcane, which is hungry mouths. In this week's Nature a much more efficient feedstock than researchers from the University of maize LS9 says that the shift from sugars California, Berkeley, and the biotech firm to biomass as a feedstock would reduce LS9 of South San Francisco, California, greenhouse gases even further. among others describe apotential solution The company has been working to modified Escherichia coli bacterium that convert sugars into tailored molecules for can make biodiesel directly from sugar several years, says co-author Stephen del omponent The process has Cardayre, LS9's vice-president for research and development. hemicellulose, of plant fibre (see page 559 a lot of promise The method can be tailored However, their university to produce ahost of high for actually being collaborators went two steps value chemicals, including further, eliminating the need for commercialized molecules that mimic additives and then folding in the standard petrol, and could be expanded to ability to use hemicellulose asafeedstock. work on tougher cellulosicmaterials, the This a representation of the type researchers say. of efforts that are going to move us to The work identifies a potentially cost biomass," he says. effective way of converting grass orcrop The researchers basically amplified waste directly into fuel, filling gas tanks and then short-circuited E coli's internal without raising global food prices or machinery for producing large fatty-acid increasing hunger and deforestation i molecules, enabling them to convert far-flung locales. Moreover, the process precursor molecules directly into fuels is much more climate friendly than and other chemicals. The team then facturing ethanol from maize, and inserted genes from other bacteria to manu produces higher-energy fuels that are produce enzymes able to break down interchangeable with current petroleum hemicellulose. In all, the authors report products. The next step is to scale the more than a dozen genetic modifications process up and adapt it to cellulose, which The results could buoy LS9, says Mark makes up the bulk of plant material Bunger, a research director at business "It's a nice milestone in the field of consultancy Lux Research in San Francisco. biofuels, and it has a lot of promise for Like its competitors, including Amyris actually being commer rcialized," says of Emeryville, California, and South San Francisco-based S LS9 struggled for funding in 2008 and early 2009 because of the drop in oil prices and the economic downturn, Bunger says. But LS9 made it through, securing US$25 million in new funding from various sources, including a strategic partnership with oil giant Chevron last September. The company plans to open a commercial-scale demonstration plant later this year. eff Tollefso Switchgrass could be made into diesel cleanly and quickly.

I need help writing a purpose for a chemistry experiment. I feel I was always do a great job, but my professor always disagrees and Iâm out of ideas. The professor wants us to summarize the introduction, and summarize what you will do in each section of the experiment and state how this work will support the goal of this experiment being longer than 1/2 a page. Please, please help me right a better purpose for the experiment below. Thanks.

Experiment 9 Molecular Weight Determination of a Pure Substance Using the Ideal Gas Equation.

Introduction:

The purpose of this experiment is to determine the molecular weight of a volatile, essentially non-polar liquid. An excess amount of pure unknown volatile liquid will be placed into a flask, whose volume will also be determined. The flask will be placed into a hot water bath, whose temperature corresponds to the temperature of the gas in the flask. The liquid will evaporate, driving out the air while the excess liquid evaporates. The pressure of the gas in the flask will correspond to the atmospheric pressure. After the excess unknown liquid has been allowed to evaporate, the flask will be stoppered, cooled, and weighed to determine the grams of the unknown liquid that will be present at the temperature of the water bath as a gas. In this experiment the ideal gas equation will be used PV = nRT = (g/M)RT where R = 0.0821 L*atm/mol*K, T = temperature in K, P = pressure in atm, V = volume in liters, n = moles of gas, g = grams of gas, and M = molecular weight of gas (in units of g/mole). Solving for the molecular weight, M: M = gRT/ PV.

If the molecular weight of a gas is to be determined, the m, T, P, and V must be determined experimentally in the lab. Even though the ideal gas equation is only an approximation of the behavior of gases, molecular weights can still be obtained within 5% of the correct values, as long as volatile non-polar compounds or compounds with only slight amount of polarity are used. For example, C, H, compounds as CH₄ are essentially non-polar, whereas compounds as H₂O are highly polar. Hence, the ideal gas equation would not be a good approximation for describing the behavior of gaseous water.

Procedure:

At the very beginning of the period get a one-liter beaker. Put about 800 mL (your instructor will tell you the exact amount needed) of tap water into the one-liter beaker. Put the one-liter beaker with water onto the hot plate. Set the heat setting of the hot plate to the maximum value. The water in the beaker should be boiling very lightly prior to doing the actual experiment. Therefore, after the water starts boiling in the hot water bath, it may be necessary to cut the heat setting back from highest value. This will take some time. While the water is heating, get the rest of the things needed for this experiment. The setup is shown in figure 1. Record the barometric pressure (in torr to one decimal place). Obtain the rest of the setup consisting of a 250 ml flask, properly prepared rubber stopper with glass tube and aluminum foil, a no-hole rubber stopper, thermometer, and glass stirring rod.

Make sure the 250 mL Florence (or Erlenmeyer) flask is dried (if it is not dry, rinse with 5 mL of acetone, pour off the acetone into the waste bottle in the hood, and then clamp the 250 mL Florence flask onto the ring stand in the inverted position to allow the last traces of acetone to drain out and evaporate. Place the dry no-hole stopper on the flask and weight the flask with the rubber stopper on the balance to 3 decimal places. Record this weight for the weight of the flask plus rubber stopper and moist air. Place 5 mL with a graduated cylinder of unknown liquid into the flask. Place the one-hole rubber stopper, with tube and aluminum foil in the flask. This one-hole stopper, which contains a glass tube that sticks out on the top by 3 mm and is flush with the bottom of the stopper, is covered with aluminum foil with a hole punched into the bottom where the glass tube is. This one-hole rubber stopper is already prepared for you. Push it down firmly into the flask. Remove it. Do this 2-3 times to smooth out the aluminum foil so that the stopper will go down into the flask as much as possible. Then push the stopper down so that it fits snugly but not too tightly to allow it to be removed while the flask is hot. Clamp the flask about the top lip of the Florence flask. That is, the center of the clamp goes about the rim of the flask. Push the flask as far down into the water bath as possible while holding the end of the clamp with your other hand. It is important to be sure that the water in the water bath is always at least 5 mm above there the bottom of the stopper is in the flask. More water may have to be added as some of the water evaporates during the duration of this experiment. (A beaker with hot water (extra) should be present in the hood. One or two of these beakers of hot water should be enough for everyone.) If the water level is not kept to its proper height, the liquid will condense in the upper part of the flask and the excess liquid will never be removed. Be sure that the aluminum foil on top makes a protective wind breaker for the short glass tube sticking out of the rubber stopper so that condensation does not occur there also. As the liquid evaporates from the flask, mix the water in the water bath occasionally and check to see that the temperature remains constant. Record the temperature value of the water bath as the temperature of the gas in the flask for the temperature of the gas would have equilibrated to the temperature of the water bath. After all the liquid has evaporated (takes 2-5 mins for the liquid to evaporate.) from the flask (check carefully that all of the liquid has evaporated-since observing when all the liquid has been evaporated maybe difficult, you should carefully shake slightly the clamp holding the Florence flask to observe the movement of the unknown liquid and when it has disappeared) and none is condensed on the surface walls; (if condensation occurs, be sure all precautions mentioned above are taken) then (these next several steps are to be done quick) remove the rubber stopper with the glass tubing and aluminum foil without excessive shaking. There could be a condensed liquid droplet or two in the glass tube that is not visible. The droplets could drop back into the flask and cause a false high reading for the measured weight of gas in the flask. Immediately replace the rubber stopper (with the glass tube and aluminum foil) with the no-hole stopper, which was used when the flask was originally weighed. This step must be performed quickly to prevent the unknown gas vapors from escaping and being replaced by moist air. Place the no-hole rubber stopper in the Florence flask firmly. Remove the flask from the bath and again check to be sure that the no-hole rubber stopper is firmly in place. Cool the flask by running tap water over the flask for 30-60 seconds. If the stopper is not fitted firmly, air will enter the flask as the liquid inside the flask condenses. As the gas cools and changes to the liquid state, a partial vacuum is created inside the flask. Hence, air will enter the flask if the rubber stopper is not fitted firmly. Completely dry the flask and weigh it on the balance to three decimal places. Record the weight of flask plus stopper and unknown gas.

Repeat this entire procedure a second time and record the date. After, second trial, completely fill the flask with distilled water. Place the no-hole rubber stopper in the flask allowing the excess water to overflow. Wipe the outside completely dry. Then measure the volume of the water in the flask by pouring water into a graduated cylinder. Record this volume.

Below, is a completed lab. After completing this lab, I was asked the following question:

What changes would you make, if any, if you did this lab again?

I'm having a hard time thinking of what I would do different. Please help!

Observations & Questions for Part 1

Record your observations and your time and temperature data in tables. Use one table for the pure water and one table for the salt solution.

Data Table 1: Pure Water and Salt Solution
Seconds	Distilled H20 Room temp	Distilled H20 Ice bath	Saltwater Room temp	Saltwater Ice bath
0	23	23	17	23
30	23	10	20	7
60	23	4	22	1
90	22.5	1	22	0
120	22.5	0	22	0
150		0	22	-1
180		-1	22	-1
210		-1	22	-2
240		-2		-2
270		-1		-2
300		-1		-2
330		-1		-2
360		-1
390		0
420		0
450		0
480		0
510		0
540
570
600
630
660

Make two graphs of your data. On one graph plot the data from the pure water. On the other graph plot the data from the salt solution. On both plot temperature on the y-axis and time on the x-axis.

A. Record the freezing point of the pure water and the freezing point of the salt solution.

Freezing point of salt Sol: -2 degree Celsius

Freezing point of pure H2O: 0 degree Celsius

B. How do these two freezing points compare?

The freezing point of salt water is lower than the freezing

point of fresh water. Salt in the water lowers the freezing point

of water.

C. What are some practical applications of freezing point depression, boiling point elevation, and vapor pressure lowering?

Some practical applications of freezing point depression

are antifreeze in a radiator and salt on the road used to melt

ice in the winter. Some practical applications of boiling point

elevation are a sealed container and possibly a pressure cooker.

Some practical applications of vapor pressure lowering are freeze

drying and steam engines.

Questions - Part 2

To what biological structure is the dialysis bag comparable? How is it similar? How is it different?

The plasma membrane is comparable to the dialysis bag.

The similarity between them is that they are both semipermeable.

The difference is the dialysis bag acts as a permeable membrane,

however, purely based on its pore size, the small molecules are

able to get through but the bigger molecules are unable to. The

plasma membrane is a more complex system that uses both active

and passive transport to allow the molecule to move through.

In biological systems if a cell is placed into a salt solution in which the salt concentration in the solution is lower than in the cell, the solution is said to be hypotonic. Water will move from the solution into the cell, causing lysis of the cell. In other words, the cell will expand to the point where it bursts. On the other hand, if a cell is placed into a salt solution in which the salt concentration in the solution is higher than in the cell, the solution is said to be hypertonic. In this case, water will move from the cell into the solution, causing cellular death through crenation or cellular shrinkage. In your experiment is the Karo

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