Answer: There are 7.4 moles of helium gas present in a 1.85 liter container at the same temperature and pressure.
Explanation:
Given: = 2.25 L,
= 9.0 mol
= 1.85 L,
= ?
Formula used to calculate the moles of helium are as follows.
Substitute the values into above formula as follows.
Thus, we can conclude that there are 7.4 moles of helium gas present in a 1.85 liter container at the same temperature and pressure.
Answer:
The answer is "2.5 mole"
Explanation:
The reaction for producing can be defined as follows:
Reaction:
According to the above reaction, to produce 2 moles of we need 1 mole of nitrogen:
So, according to the question to produce 5.0 mole the required
:
To produce 5.0 mole we need 2.5 mole
Answer:
Indeed, the two samples should contain about the same number of gas particles. However, the molar mass of is larger than that of
(by a factor of about
.) Therefore, the mass of the
sample is significantly larger than that of the
sample.
Explanation:
The and the
sample here are under the same pressure and temperature, and have the same volume. Indeed, if both gases are ideal, then by Avogadro's Law, the two samples would contain the same number of gas particles (
and
molecules, respectively.) That is:
.
Note that the mass of a gas is different from the number of gas particles
in it. In particular, if all particles in this gas have a molar mass of
, then:
.
In other words,
The ratio between the mass of the and that of the
sample would be:
.
Since by Avogadro's Law:
.
Look up relative atomic mass data on a modern periodic table:
Therefore:
Verify whether :
Note that the mass of the sample comes with only two significant figures. The two sides of this equations would indeed be equal if both values are rounded to two significant figures.