Answer is (3) protons and neutrons.
(P.S. The outer part contains the electrons)
I think the awnser would be C. becuase Pure Substances are made of mostly the same material and properties Such as: Nitrogen Gas, Oxygen Gas, Carbon, Iorn, Water, Sugar and Salt.
Answer:
548 g/mol
Explanation:
The freezing point depression of a solvent occurs when a nonvolatile solute is added to it. Because of the interactions between solute-solvent, it is more difficult to break the bonds, so the phase change will need more energy, and the freezing point will drop, which is called cryoscopy.
The drop in temperature can be calculated by:
ΔT = Kf*W*i
Where Kf is the cryoscopy constant of the solvent, W is the molality, and i is the van't Hoff factor, which indicates the fraction of the solute that dissolves.
The molality represents how much moles (n) of the solute is presented in each kg of the solvent (m2), thus
W = n/m2
The number of moles is the mass of the solute (m1) in g, divided by the molar mass (M1) of it:
W = m1/(M1*m2)
So, by the data:
0.2214 = 0.632/(M1*0.00521)
0.00115M1 = 0.632
M1 = 548 g/mol
Since the teacher has said to use quantitative observation, density is the easiest measurement to make. Aluminum has a density of 2.7 g/mL. Brass has a density of 8.73 g/mL. Copper has a density of 8.96 g/mL. As long as the mass and volume measurements are accurate (water displacement can be used for volume measurements), the resulting density values can be distinguished.
It may be possible to distinguish these three metals visually, based on color, but the instructions have stated to use quantitative observation.
Answer:
Increasing the temperature
Explanation:
According to Le Chatelier's principle, "if any of the conditions of a system in equilibrium is changed, the system will adjust itself in order to annul the effect of the change".
Since the forward reaction is exothermic, this suggests that heat is given off in the reaction.
Increasing the temperature will favors the reverse process which is endothermic.
In going from the reactants to the the products, the reaction is deemed exothermic which suggests that it produces heat.
The backward reaction is endothermic i.e it absorbs heat. If the temperature is increased, this process will be favored and more reactants produced. Less of the diiodine pentoxide will form. There is a leftward shift of the equilibrium
