Diets that severely restrict carbohydrate intake often result in ketosis for the dieter.
Explain why this occurs by selecting the correct answer.
| A. When carbohydrates are restricted, the body metabolizes fats for energy, resulting in a quantity of acetyl-CoA that can't be metabolized in the citric acid cycle due to the reduced quantity of acetate, which is used in gluconeogenesis, The body, instead, uses ketosis for energy, and ketogenesis results. |
|
B. When carbohydrates are restricted, the body metabolizes fats for energy, resulting in a quantity of acetyl- CoA that can't be metabolized in the citric acid cycle due to the reduced quantity of oxaloacetate, which is used in gluconeogenesis, The body, instead, uses ketogenesis for energy, and ketosis results. |
| C. When carbohydrates are restricted, the body metabolizes proteins for energy, resulting in a quantity of acetyl-SCoA that can't be metabolized in the citric acid cycle due to the reduced quantity of oxaloacetate, which is used in gluconeogenesis, The body, instead, uses ketogenesis for energy, and ketosis results. |
In: Chemistry
When he received the Nobel Prize in chemistry in
1960, Willard Libby gave a lecture about radioactive dating to the
king of Sweden and assembled guests in Stockholm.
a) It was suspected that cosmic rays from space hit the
Earth. What evidence confirmed this hypothesis?
b) What did Libby have to assume to reach the
conclusion that the expected specific radioactivity of living
matter would be 2.0/8.5 disintegrations per second per gram of C?
What evidence was there to confirm his conclusion?
c) Libby concluded that we humans are in steady
state with respect to our own concentrations of carbon-14 while
alive but not after death. How did he justify this
conclusion?
d) On what basis did Libby conclude that humans are
radioactive? What evidence did he collect to test his
conclusion?
And here is the link provided for answering this question: http://www.nobelprize.org/nobel_prizes/chemistry/laureates/1960/libby-lecture.pdf
In: Chemistry
A 100.0 −mL buffer solution is 0.110 M in NH3 and 0.125 M in NH4Br.
A. If the same volume of the buffer were 0.260 M in NH3 and 0.395 M in NH4Br, what mass of HCl could be handled before the pH fell below 9.00?
B. What mass of HCl could this buffer neutralize before the pH fell below 9.00?
In: Chemistry
Why does the primary structure impact all levels of protein structure? What is unique about the peptide bond that directly impacts protein structure? What intermolecular forces stabilize protein structure? Consider protein denaturation, what environmental forces can cause a protein to lose its structure? What types of interactions are they disrupting? Many proteins require chaperones to properly fold. How do chaperones help proteins fold? What potential problems might arise from a misfolded protein? (An example from the text may be useful but is not required.)
In: Chemistry
In a buffer solution prepared from 10 mL of 3.0 M benzoic acid (HC6H5CO2) added to 20 mL of a 2.0 M sodium benzoate (NaC6H5CO2) and diluted to a total volume of 200mL- Calculate each of the following:
a. The original pH of the buffer solution
b. The pH upon addition of 8.0 mL of 2.0 M NaOH to part a
c. The pH upon addition of 30.0 mL of 2.0 M HCl to part a
In: Chemistry
In a buffer solution prepared from 10 mL of 3.0 M Pyridine (C5H5N) added to 20 mL of 2.0 M Pyridine Hydrochloride (C5H5NHCl) and diluted to a total volume of 200 mL- Calculate each of the following:
a. The original pH of the buffer solution
b. The pH upon addition of 25.0 mL of 2.0 M NaOH to part a
c. The pH upon addition of 10.0 mL of 2.0 M HCl to part b
In: Chemistry
1. For KNO3 the heat of solution is 23.8 kJ/mol and the lattice energy is -685.0 kJ/mol. Calculate the heat of hydration.
2. 60.3 g of zinc sulfate [ZnSO4], is added to 160. g of water. Will the salt dissolve completely and, if so, will the solution be saturated or unsaturated? The solubility of ZnSO4 is 3.57 m.
3. What volume of water, in mL, is needed to dissolve 2.2 mg of hydrogen gas when the partial pressure of hydrogen above the water is 2.2 atm at 25 °C? The Henry's constant for hydrogen gas in water at 25 °C is 7.8×10-4 M/atm.
PLEASE ANSWER ALL 3 QUESTIONS.
In: Chemistry
Answer the following and express your answer using two significant figures.
Calculate the final concentration of each of the following diluted solutions.
A) 3.5 L of a 4.0 M HNO3 solution is added to water so that the
final volume is 8.0 L .
B) Water is added to 0.15 L of a 6.0 M KOH solution to make 2.0 L of a diluted KOH solution.
C) A 35.0 mL sample of 8.0 % (m/v) NaOH is diluted with water so that the final volume is 200.0 mL .
D) A 6.0 mL sample of 50.0 % (m/v) acetic acid (HC2H3O2) solution is added to water to give a final volume of 25 mL .
In: Chemistry
A sample that contains only BaCO3 and MnCO3 weighs 0.8192 g. When it is dissolved in excess acid, 0.2420 g of carbon dioxide is liberated. What percentage of BaCO3 did the sample contain? Assume all the carbon originally present is converted to carbon dioxide.
In: Chemistry
You prepare a solution by dissolving 50.4g sucrose (C12H22O11) in
0.332 kg of water. The final volume of the solution is 355 mL.
Calculate the concentration of the solution in each unit.
1 mole C12H22O11 = 342.296 g sucrose
(a) Molarity
(b) Molality
(c) Percent by mass
(d) Mole fraction
In: Chemistry
Calculate the mass and volume of 150 mmol of benzaldehyde, and the theoretical yields of benzoin, benzil, and benzilic acid expected from that much benzaldehyde. I'm pretty sure that you use 2 mol of benzaldehyde per 1 mol of the other compounds, but you might want to check to make sure.
Please calculate the theoretical yield in grams. Thank you very much.
In: Chemistry
I don't understand this at all so the more detailed explaination would be amazing, thanks!
part B: How many grams of NH3 can be produced from 3.34 mol of N2 and excess H2.
Express your answer numerically in grams.
Part C: How many grams of H2 are needed to produce 13.73 g of NH3?
Express your answer numerically in grams.
Part D: How many molecules (not moles) of NH3 are produced from 3.50×10−4 g of H2?
Express your answer numerically as the number of molecules.
In: Chemistry
a sample of water collected in the field had a pH of 6.8. by the time the water sample reached the laboratory for analysis the pH had increased to 7.5. give a possible explanation for this sample change.
In: Chemistry
Answer the following and express your answer using two significant figures. Calculate the grams of solute needed to prepare each of the following solutions.
A) 1.6 L of a 4.5 M NaOH solution
B) 7.0 L of a 0.20 M CaCl2 solution
C) 180 mL of a 3.50 M NaNO3 solution
In: Chemistry
9. Calculate the freezing point and boiling point of the
following aqueous solutions, assuming
complete dissociation:
(a) 10.5 g FeCl3 in 1.50
In: Chemistry