Answer:
The strength of a bond depends on the amount of overlap between the two orbitals of the bonding atoms
Orbitals bond in the directions in which they protrude or point to obtain maximum overlap
Explanation:
The valence bond theory was proposed by Linus Pauling. Compounds are firmed by overlap of atomic orbitals to attain a favourable overlap integral. The better the overlap integral (extent of overlap) the better or stringer the covalent bond.
Orbitals overlap in directions which ensure a maximum overlap of atomic orbitals in the covalent bond.
Answer:
Mass of Cl₂ produced 12.78 g
Explanation:
Given data:
Mass of MnO₂ = 16 g
Mass of HCl = 30.0 g
Mass of Cl₂ produced = ?
Solution:
Chemical equation:
MnO₂ + 4HCl → MnCl₂ + Cl₂ + 2H₂O
Number of moles of MnO₂:
Number of moles = mass / molar mass
Number of moles = 16 g/ 87 g/mol
Number of moles = 0.18 mol
Number of moles of HCl:
Number of moles = mass / molar mass
Number of moles = 30 g/ 36.46 g/mol
Number of moles = 0.82 mol
Now we will compare the moles of Cl₂ with MnO₂ and HCl.
MnO₂ : Cl₂
1 : 1
0.18 : 0.18
HCl : Cl₂
4 : 1
0.82 : 1/4×0.82 = 0.205 mol
The number of moles of Cl₂ formed by HCl are less it will limiting reactant.
Mass of Cl₂ formed:
Mass = number of moles × molar mass
Mass = 0.18 mol × 71 g/mol
Mass = 12.78 g
Answer:
The final temperature of the given ideal diatomic gas: <u>T₂ = 753.6 K</u>
Explanation:
Given: Atmospheric pressure: P = 1.0 atm
Initial Volume: V₁ , Final Volume: V₂ = V₁ (1/10)
⇒ V₁ / V₂ = 10
Initial Temperature: T₁ = 300 K, Final temperature: T₂ = ? K
For a diatomic ideal gas: γ = 7/5
For an adiabatic process:


![\left [\frac{V_{1}}{V_{2}} \right ]^{\gamma-1 } = \frac{T_{2}}{T_{1}}](https://tex.z-dn.net/?f=%5Cleft%20%5B%5Cfrac%7BV_%7B1%7D%7D%7BV_%7B2%7D%7D%20%5Cright%20%5D%5E%7B%5Cgamma-1%20%7D%20%3D%20%5Cfrac%7BT_%7B2%7D%7D%7BT_%7B1%7D%7D)
![\left [10 \right ]^{\frac{7}{5}-1 } = \frac{T_{2}}{300 K}](https://tex.z-dn.net/?f=%5Cleft%20%5B10%20%5Cright%20%5D%5E%7B%5Cfrac%7B7%7D%7B5%7D-1%20%7D%20%3D%20%5Cfrac%7BT_%7B2%7D%7D%7B300%20K%7D)
![\left [10 \right ]^{\frac{2}{5} } = \frac{T_{2}}{300 K}](https://tex.z-dn.net/?f=%5Cleft%20%5B10%20%5Cright%20%5D%5E%7B%5Cfrac%7B2%7D%7B5%7D%20%7D%20%3D%20%5Cfrac%7BT_%7B2%7D%7D%7B300%20K%7D)


<em><u>Therefore, the final temperature of the given ideal diatomic gas</u></em><em>:</em> T₂ = 753.6 K