A 3.00-liter sample of gas is at 288 K and 1.00 atm. If the pressure of the gas is increased to 2.00 atm and its volume is decre
1 answer:
Answer:
288K
Explanation:
In most situation where the name of the gas is not mentioned, the best option we have is to use the ideal gas law.
Remember, the pressure was doubled, and the volume was halved, numerically cancelling each other out. As a result, the final temperature be the same as the initial temperature.
Now, solving for T
You might be interested in
Answer:
For the control experiment: of aqueous solution of erioglaucine has absorbance of
From Lambert-Beer's law we know:
Here; e is the molar absorptivity coefficient of erioglaucine
l = length of cuvette in which the solution is taken =
A sorbance by the erioglaucine = total absorbance - absorbance by distilled
So; by putting the values in the above equation; we get:
So;
The molar absorptivity coefficient of erioglaucine is
The absorbance of erioglaucine in distilled water (contaminated with metal ions) is:
The absorbance of distilled water is
So; absorbance of erioglaucine itself is :
Again using Lambert Beer law; we get:
c = 0.198/5.65 M = 0.035 M
The concentration of the erioglaucine is
Explanation:
Atomic Mass will be 23 the new magnesium formed will be its isotope of magnesium.
We know that,
In stable condition
Number of electrons = Number of protons
Atomic number represents number of proton .
So, here number of proton is 12
Therefore, number of electron is 12
We know that -
Atomic mass = number of protons +Number of neutron
So if magnesium loses one neutron i.e. new number of neutron is 11
then its atomic mass changes.
New atomic mass will be
Atomic mass =
Atomic mass = 23
This new element with atomic mass 23 and atomic number 12 is the isotope of magnesium.
To know more about isotopes
#SPJ4