11.....6 for Na, 1 for S and 4 for O
Answer:
mass
Explanation:
The amount of kinetic energy an object has, depends on its mass and its speed.
If we assume this two gases behave like ideal gas, then we use the ideal gas law
, where P is the pressure, V is the volume, n number of moles, R gas constant and T the temperature in kelvins. As well as the density formula
. First we calculate the molarity for Freon
.
The number of moles for freon are
![D=\frac{m}{V} =\frac{ nM}{L} \implies n= \frac{DL}{M} = \frac{5.58 g \times L}{L \times 137.36g/mol}= 0.0406 mol](https://tex.z-dn.net/?f=D%3D%5Cfrac%7Bm%7D%7BV%7D%20%3D%5Cfrac%7B%20nM%7D%7BL%7D%20%5Cimplies%20n%3D%20%5Cfrac%7BDL%7D%7BM%7D%20%3D%20%5Cfrac%7B5.58%20g%20%5Ctimes%20L%7D%7BL%20%5Ctimes%20137.36g%2Fmol%7D%3D%200.0406%20mol)
We know
, so we insert this concept to our ideal gas equation
. Since
, we insert this concept to the formula
. The measurements take place in same conditions so,
![M=\frac{DRT}{P} = \frac{4.38g}{L}\times \frac{1L}{0.0406mol} = 107.9\ g/mol](https://tex.z-dn.net/?f=M%3D%5Cfrac%7BDRT%7D%7BP%7D%20%3D%20%5Cfrac%7B4.38g%7D%7BL%7D%5Ctimes%20%5Cfrac%7B1L%7D%7B0.0406mol%7D%20%3D%20107.9%5C%20g%2Fmol)
Answer:
just by making or answering the questions
Answer:
0 %
Explanation:
As we know 10.81 is the average atomic mass of boron which can not be contained by a single boron atom. Therefore, when isolated, a single boron atom will weight either 10 amu for ¹⁰B and 11 amu for ¹¹B respectively.
The average atomic mass is calculated as;
Atomic Mass of ¹⁰B = 10
Atomic Mass of ¹¹B = 11
Natural Abundance of ¹⁰B = 20 %
Natural Abundance of ¹¹B = 80 %
So,
Average Atomic Mass = (10 × 0.2) + (11 × 0.8)
Average Atomic Mass = 2 + 8.8
Average Atomic Mass = 10.8