Question: Jennifer and Justin are examining the principle of chemical equilibrium in their second year organic chemistry course. They are performing a reaction that involves hydrogen gas and glucose as the starting reactants, and the products formed in the reaction are carbon dioxide and oxygen gas. Jennifer and Justin add the materials, and then wait until the reaction has reached equilibrium. Afterwards, Jennifer removes glucose from her reaction mixture, while Justin removes carbon dioxide from his reaction mixture. Given the paragraph above, please answer correctly the following question: Which person's reaction, Jennifer's or Justin's, will begin producing less carbon dioxide? Hint: An equilibrium can also be disrupted by the full or partial removal of a reactant or product. If the concentration of a substance is decreased, the system will respond by favoring the reaction that replaces that substance. In the industrial Haber-Bosch process, NH 3 is removed from the equilibrium system as the reaction proceeds. As a result, the forward reaction is favored so that more NH 3 will be produced. The concentrations of N 2 and H 2 decrease. Continued removal of NH 3 will eventually force the reaction to go to completion until all of the reactants are used up. If either N 2 or H 2 were removed from the equilibrium system, the reverse reaction would be favored, and the concentration of NH 3 would decrease.
Answer: Jennifer's

Question: Two colleagues read about types of chemical reactions. Sean studied about the influence of temperature on chemical reactions. Gabe studied about other influencing factors. Given the paragraph above, please answer correctly the following question: Which student read less about a greater frequency of collisions? Hint: Raising the temperature of a chemical reaction usually results in a higher rate of reaction. When the reactant particles are heated, they move faster and faster. This results in a greater frequency of collisions. A more important effect of the temperature increase is that the collisions occur with a greater force and are thus more likely to surmount the activation energy barrier and go on to form products. Increasing the temperature of a reaction increases the number of effective collisions between reacting particles, so the reaction rate increases.
Answer: Gabe

Question: Jordan is conducting an experiment to see how Iron rusts. He first takes Iron Bar A and puts it out on his porch on a rainy day. Then he puts Iron bar B in an airtight bag and removes all of the oxygen and air to vacuum seal it. After some time passes the bar he left outside is completely covered in rust. He removes the bar in the vacuum sealed bag and to his surprise it has no rust at all. Because there was no oxygen and water in the air tight bag, iron bar B has no rust at all. Iron bar A was exposed to a lot of water and oxygen and there for it rusted completely. Given the paragraph above, please answer correctly the following question: Given a new piece of iron, will leaving it outside or sealing it in a bag cause it to rust? Hint: Iron is first oxidized to iron(II) ions by oxygen. In the second step, the iron(II) ions are further oxidized and combine with water and oxygen gas to produce a hydrated form of iron(III) oxide known as rust. Rusting is one of many example of corrosion. Corrosion is the deterioration of metals by redox processes. Corrosion causes enormous amounts of damage to buildings, bridges, ships, cars, and other objects. It has been estimated that corrosion costs the U.S. economy over 100 billion dollars each year. A great amount of time and effort is spent to try to limit or prevent corrosion.
Answer:
outside