The second one and the 2 last ones
Mass, charge, and energy are conserved, no matter how much volume of
space they may be spread through either before or after the reaction.
Concerning density ...
Think about the fascinating classroom demonstration where the teacher
drops a tiny pellet of sodium into a glass of water. The sodium gets very
excited, and it skates and skitters around on the surface of the water,
faster and faster, and eventually it explodes. All the girls in the class
scream, while the guys are just sitting there and staring at the cloud
of steam that's rising from the glass of water. The whole point here
is that the density of the steam is much different from the density of
either the water or the sodium that reacted to create it. The density
is not conserved.
We can use the heat equation,
Q = mcΔT
where Q is the amount of energy transferred (J), m is the mass of the substance (kg), c is the specific heat (J g⁻¹ °C⁻¹) and ΔT is the temperature difference (°C).
Q = 11.2 kJ = 11200 J
m = <span>145 g
</span>c = ?
ΔT = (67 - 22) °C = 45 °C
By applying the formula,
11200 J = 145 g x c x 45 °C
c = 1.72 J g⁻¹ °C⁻¹
Hence, specific heat of benzene is 1.72 J g⁻¹ °C⁻¹.
Many compunds have a terminal carbonyl
Aldehyde, Ketone, Carboxylic acid, Amide, Imide, Acid anhydride are the first that come to my mind.
There are two big advantages of using molarity to express concentration. The first advantage is that it's easy and convenient to use because the solute may be measured in grams, converted into moles, and mixed with a volume.
The second advantage is that the sum of the molar concentrations is the total molar concentration. This permits calculations of density and ionic strength
