Answer:
your question is incomplete and its
particles which is one mole of a substance
Explanation:
you can solve the question by using this formular 1 mole of a substance=mass of the substance/ its molar mass
you find molar mass of a compound by adding individual molar masses of elements in that compound
a. W = 0 J
b. W = - 308.028 J
<h3>Further explanation</h3>
Given
Nitrogen gas expands in volume from 1.6 L to 5.4 L
Required
The work done
Solution
Isothermal :
W = -P . ΔV
Input the value :
a. At a vacuum, P = 0
So W = 0
b. At pressure = 0.8 atm
W = - 0.8 x ( 5.4 - 1.6)
W = -3.04 L.atm ( 1 L.atm = 101.325 J)
W = - 3.04 x 101.325
W = - 308.028 J
Answer:
Frecuency = 5,83x10⁻⁷ Hz
Explanation:
The equation that connects wavelenght and frequency is given by:
λ = c/ν
λ=wavelenght (expressed in lenght´s units)
c= speed of light (3x10⁸ m/sec)
ν=frequency (expressed in units of time⁻¹ or Herzt)
In our case, λ=5,14x10⁻⁷ m , so replacing in our previous formula, this gives us the final result of ν (frequency for green light) of 5,83x10¹⁴ Hz (or Herzt)
Answer:
False
Explanation:
False. The molecules of liquid are hold in the liquid state due to intermolecular forces or Van de Waals forces , without affecting the molecule itself and its atomic bonds (covalent bonds). When the temperature increases the kinetic energy of the molecules is higher , therefore they have more possibilities to escape from the attractive intermolecular forces and go to the gas state.
Note however that this is caused because the intermolecular forces are really weak compared to covalent bonds, therefore is easier to break the first one first and go to the gas state before any covalent bond breaks ( if it happens).
A temperature increase can increase vaporisation rate if any reaction is triggered that decomposes the liquid into more volatile compounds , but nevertheless, this effect is generally insignificant compared with the effect that temperature has in vaporisation due to Van der Waals forces.
