Answer: There are 4.8 x 1024 hydrogen atoms in 2.0 moles of CH4
Answer:
B
Explanation:
It is important to only test one variable at a time because you need to be able to disprove or prove a problem with just one independent variable. When you have several variables in the experiment, it would be impossible to know which variable honestly caused the end result.
Yes, because it comes from a one thing and spreads throughout the entire space. Similar to dripping foot coloring into a glass of water, or spraying air freshener.
Answer:
Here you go!
Explanation:
Our Universe is just a small part. There are many other Universes’ that exist. We live in a Multiverse. ...
Astronomer Edwin Hubble, in 1920’s, discovered that the Universe is not static. It is expanding and contracting continuously.
There is a dark energy that is making the Universe expand and accelerate at a larger rate than it did many years ago. ...
The Universe is infinite. It has no end. Thus scientists believe that the Universe is not a closed sphere but as flat as a sheet of paper and has no ...
According to the scientists the planets, stars and galaxies include only 4% of what a Universe consists of. 96% of the things in the Universe cannot be seen.
Answer:
The total heat required is 691,026.36 J
Explanation:
Latent heat is the amount of heat that a body receives or gives to produce a phase change. It is calculated as: Q = m. L
Where Q: amount of heat, m: mass and L: latent heat
On the other hand, sensible heat is the amount of heat that a body can receive or give up due to a change in temperature. Its calculation is through the expression:
Q = c * m * ΔT
where Q is the heat exchanged by a body of mass m, constituted by a substance of specific heat c and where ΔT is the change in temperature (Tfinal - Tinitial).
In this case, the total heat required is calculated as:
- Q for liquid water. This is, raise 248 g of liquid water from O to 100 Celsius. So you calculate the sensible heat of water from temperature 0 °C to 100° C
Q= c*m*ΔT

Q=103,763.2 J
- Q for phase change from liquid to steam. For this, you calculate the latent heat with the heat of vaporization being 40 and being 248 g = 13.78 moles (the molar mass of water being 18 g / mol, then
)
Q= m*L

Q=562.0862 kJ= 562,086.2 J (being 1 kJ=1,000 J)
- Q for temperature change from 100.0
∘
C to 154
∘
C, this is, the sensible heat of steam from 100 °C to 154°C.
Q= c*m*ΔT

Q=25,176.96 J
So, total heat= 103,763.2 J + 562,086.2 J + 25,176.96 J= 691,026.36 J
<u><em>The total heat required is 691,026.36 J</em></u>