Answer:
The C14 would be found in Glyceraldehyde-3-Phosphate, and the O18 would also be found in the same molecule
Explanation:
Isotopic labeling is a common method for deducing reaction mechanism in chemistry.
In photosynthesis, the oxygen in the found in Glyceraldehyde-3-Phosphate comes from the carbon dioxide, This is also finally found in the glucose produced at the end of the cycle.
The oxygen in water is released into the atmosphere as the oxygen molecule.
Therefore, the C14 would be found in Glyceraldehyde-3-Phosphate, and the O18 would also be found in the same molecule.
Answer:
Explanation:
Remark
First of all you have to identify what is happening. You make the following observations.
The solution in the test tube in a cold water bath is colorless.
As you add heat, the color changes from colorless to brown.
What you are told
N2O4 is colorless
NO2 is brownish red.
What you conclude
The reaction is endothermic. That means it requires heat to happen. An endothermic reaction is
A + Heat ===> B
So you have three possible correct answers
N2O4 + 14 kCal ===> 2NO2
N2O4 ====> 2NO2 dH = 14 kCal
N2O4 ====> 2NO2 - 14 kCal
I can't read the last 4 equations.
Other answers
As the temperature increased, the N2O4 became less.
As the temperature increased, the products were favored. (color change)
The reaction is exothermic (gives off heat) when the reaction goes from
NO2 - Heat ===> N2O2
Geiger–Marsden experiment(s)<span> (also called the </span>Rutherford gold foil experiment<span>) were a landmark series of experiments by which scientists discovered that every </span>atom<span> contains a nucleus where its positive charge and most of its mass are concentrated. They deduced this by measuring how an </span>alpha particle<span> beam is scattered when it strikes a thin metal foil. The experiments were performed between 1908 and 1913 by </span>Hans Geiger<span> and </span>Ernest Marsden<span> under the direction of </span>Ernest Rutherford<span> at the Physical Laboratories of the </span>University of Manchester<span>.</span>
Answer:
83.6 g
Explanation:
The limiting reactant is carbon and oxygen is in excess.
C + O₂ ⟶ CO₂
Data:
Mass of C = 22.8 g
Mass of O₂ = 78.0 g
Mass of unreacted O₂ = 17.2 g
Calculations:
Mass of O₂ reacted = 78.0 g - 17.2 g = 60.8 g
Mass of reactants (C + O₂) = 22.8 g + 60.8 g = 83.6 g
According to the Law of Conservation of Mass, the mass of the product (CO₂) equals the sum of the masses of the reactants.
The mass of CO₂ is 83.6 g.