Answer:
9.7 g
Explanation:
From the question,
Note: The molar volume of all gas at stp is 22.4 dm³ or 22.4 L
1 mol of oxygen gas (O₂) at stp = 22.4 dm³
X mole of oxygen gas (O₂) at stp = 6.8 L
X = (1 mol×6.8 L)/22.4 L
X = 0.3036 mol.
But,
Number of mole (n) = mass (m)/molar mass (m')
n = m/m'
m = n×m'.................. Equation 2
Where n = 0.3036 mol, m' = 32 g/mol
Substitute into equation 2
m = 0.3036×32
m = 9.7 g
Explanation:
As it is given that there are six electrons with four of them unpaired in the degenerate orbital.
As in a p-orbital there are only 3 sub-orbitals, that is,
,
, and
. In these sub-orbitals, a maximum of 6 electrons can be accommodated.
Th next higher orbital is d-orbital which can contain a maximum of 10 electrons. There are 5 degenerate orbitals present in a d-orbital.
So, a d-orbital can easily accommodate six electrons with four of them unpaired.
Thus, we can conclude that 5 degenerate orbitals are needed to contain six electrons with four of them unpaired.
Answer:
Molar concentration is 0.050 M
Explanation:
Osmotic pressure -
Osmotic pressure is pressure applied to stop the flow of solvent across a semipermeable membrane, from its high concentration to its low concentration , it is a type of colligative property , i.e. , it depends on the number of moles of solute.
Osmotic pressure can be calculated from the formula -
π = CRT
π = Osmotic pressure ( in atm )
C = molarity of the solution
R = universal gas constant ( 0.082 L.atm / K.mol )
T = temperature ( Kelvin )
From the question ,
π = 945 torr
since,
760 torr = 1 atm
1 torr = 1 / 760 atm
945 torr = 1 / 760 * 945 atm
945 torr = 1.24 atm
Temperature = T = 28°C
(adding 273 To °C to convert it to K)
T = 28 + 273 = 301 K
Using the equation of osmotic pressure,
π = CRT
C = π / RT
putting the
C = 1.24 atm / 0.082 L.atm / K.mol * 301 K
C = 1.24 / 24.68
C = 0.050 M
Hence,
The Molar concentration is 0.050 M.
Answer:
5.167 kJ
Explanation:
We have to divide the heating process into two steps: one for the heating process of liquid water (1) and the other for the phase transition from liquid water to steam at 100°C (2)
1 - heating from 52.1°C to 100°C:
heat(1) = m x Cp x ΔT = 2.1 g x 4.184 J/g°C x (100°C-52.1°C) = 420.9 J
2 - vaporization at 100°C:
heat(2) = m x ΔHv = 2.1 g x 2260 J/g = 4746 J
Finally, we add the heat values of the steps:
heat required = heat(1) + heat(2) = 420.9 J + 4746 J = 5166.9 J
Since 1 kJ= 1000 J, we convert from J to kJ:
5166.9 J x 1 kJ/1000 J = 5.1669 kJ ≅ 5.167 kJ
Answer : The volume for 6.0m HCl solution required = 62.5 ml
Solution : Given,
Initial concentration of HCl solution = 6.0m
Final concentration of HCl solution = 1.5m
Final volume of HCl solution = 250 ml
Initial volume of HCl solution = ?
Formula used for dilution is,

where,
= initial concentration
= final concentration
= initial volume
= final volume
Now put all the given values in above formula, we get the initial volume of HCl solution.

= 62.5 ml
Therefore, the volume for 6.0m HCl solution required = 62.5 ml