Answer: Rotation occurs at single bonds that are sigma bonds. Rotational barrier is the amount of activation energy required to covert rotamer to another by rotation that occurs around the sigma bond(C-C single bond). Due to the presence of steric hindrance that is the nonbonding interaction effects the reactivity of ions and molecules, activation energy increases. So the rotational barrier in butenyl cation is high.
Rate of production of NO₂ = 0.2 M/s
Rate of production of O₂ = 0.05 M/s
<h3>Further explanation</h3>
Given
The rate of N₂O₅ : 0.1 M/s
Reaction
2N₂O₅⇒4NO₂+O₂
Required
The rate of production of NO₂ and O₂ at the same time point
Solution
Rate of disappearance of N₂O₅ = reaction rate x coefficient of N₂O₅
0.1 M/s=reaction rate x 2
<em>reaction rate = 0.05 M/s</em>
The rate of production of NO₂=
Rate of production of NO₂ = reaction rate x coefficient of NO₂
Rate of production of NO₂ = 0.05 M/s x 4
Rate of production of NO₂ = 0.2 M/s
The rate of production of O₂=
Rate of production of O₂ = reaction rate x coefficient of O₂
Rate of production of O₂ = 0.05 M/s x 1
Rate of production of O₂ = 0.05 M/s
Divide the mass of the proton by the mass of the electron.
Answer:
a) 0.714g of bicarbonate of soda are required.
b) 0.221g of Al(OH)₃ are required
Explanation:
The reactions of HCl with bicarbonate of soda and aluminium hydroxide are:
HCl + NaHCO₃ → H₂O + NaCl + CO₂
3 HCl + Al(OH)₃ → 3H₂O + AlCl₃
The moles of HCl that we need neutralize are:
50mL = 0.050L * (0.17mol / L) = 0.0085 moles HCl
To solve these problem we need to find the moles of the antacid using the chemical reaction and its mass using its molar mass;
<em>a) </em><em>Moles NaHCO₃ = Moles HCl = 0.0085 moles </em>
The mass is -Molar mass NaHCO₃: -84g/mol-
0.0085 moles * (84g / mol) = 0.714g of bicarbonate of soda are required
b) 0.0085 moles HCl * (1mol Al(OH)₃ / 3mol HCl) = 2.83x10⁻³ moles Al(OH)₃
The mass is -Molar mass: 78g/mol-:
2.83x10⁻³ moles Al(OH)₃ * (78g/mol) =
<h3>0.221g of Al(OH)₃ are required</h3>
