In 1906 harden and young, in a series of classic studies on the fermentation of glucose to ethanol and co2 by extracts of brewer's yeast, made the following observations.

(a) inorganic phosphate was essential to fermentation; when the supply of phosphate was exhausted, fermentation ceased before all the glucose was used.
(b) during fermentation under these conditions, ethanol, co2, and a sugar phosphate accumulated.
(c) when arsenate was substituted for phosphate, no sugar phosphate acumulated, but the fermentation proceeded until all the glucose was converted to ethanol and co2.

answer the following questions.

1. which enzyme of glycolysis requires inorganic phosphate and therefore stops when no phosphate is available?
(a) glyceraldehyde 3-phosphate dehydrogenase
(b) phosphoglycerate mutase
(c) phosphofructokinase-1
(d) phosphoglycerate kinase

2. what sugar phosphate accumulates under these conditions?
(a) glucose 1,6-biphosphate
(b) glucose 1-phosphate
(c) fructose 1-phosphate
(d) fructose 1,6-biphosphate

3. arsenate substitution for phosphate generated an acyl arsenate compound that immediately degraded. what glycolysis intermediate was a product of the spontaneous degradation of this acyl arsenate?
(a) glycerol 3-phosphate
(b) 3-phosphoglycerate
(c) dihydroxyacetone phosphate
(d) glyceraldehyde 3-phosphate

Match the following items. 1. high-intensity bundle of energy being emitted from some decaying nuclei gamma ray 2. particle radiating from the nucleus of some atoms beta particle 3. negative particle identical to an electron but radiating from a decaying nucleus alpha particle

Ionic compounds are made of ions, and yet the overall charge of an ionic compound is neutral. why?

Experiment: effect of solution concentration on reaction rate you have learned that as the concentration of reactants increases, there will most likely be a greater number of collisions, and hence increase the rate of a reaction. in this experiment, you will see a demonstration of this, with a twist. there will be three reactions going on in this experiment. objectives determine how solution concentration can affect the rate of a reaction. the first reaction will be a reaction of the iodide ion (i-1) with hydrogen peroxide (h2o2) in an acidic solution. this reaction produces a slightly orange solution. in our experiment, we will add some orange food coloring to make this solution more orange. 2 h+ (aq) + 2 i- (aq) + h2o2 (aq) ⟶ i2 (aq) + 2 h2o (l) the next reaction will be between the iodine and starch i2 + starch ⟶ i2-starch complex (blue-black) so, when starch is added to the iodine solution made from the first reaction, the solution will turn black immediately, so it is difficult to find the rate of reaction. in order to be able to time this reaction, you will slow it down with another reaction. adding ascorbic acid will react with the iodine, reducing the concentration of the iodine available to react with the starch. c6h8o6 (aq) + i2 (aq) ⟶ 2i- (aq) + c6h6o6 (aq) + 2 h+ (aq) when the ascorbic acid is used up, the remaining iodine molecules can react with the starch and form the black color. the more ascorbic acid you add, the slower the reaction to form the iodine-starch complex will be. use your data and observations to complete the assignment. analysis and conclusions submit your data and the answers to these questions in the essay box below. what was your hypothesis? plot your data as drops of ascorbic acid vs. time. as the concentration of ascorbic acid was increased, did the rate of the formation of the iodine-starch complex increase or decrease? explain your answer in terms of the chemical reactions involved. was your hypothesis correct? make a general rule about the effects of concentration of reactants on reaction rates. for practice, the molecular formula for ascorbic acid is c6h8o6, and you used 6 g in this experiment, calculate the molarity of the ascorbic acid. now calculate the concentration in moles per drop (assume 1 ml = 20 drops).