Hydrogen Bonding is considered as the strongest Intermolecular Interactions between two protic compounds.
Formation of Hydrogen Bonding:
Hydrogen Bonding takes place between the Hydrogen atom bonded to most electronegative element (i.e. F, O, N) of one molecule and the most electronegative element (i.e. F, O, N) of other molecule. This is because the Hydrogen atom attains a partial positive charge which creates attractive forces with the electronegative atom with partial negative charge.
In given options Hydrogen Bonding can only exist in Methanol (CH₃-O-H). As, the hydrogen atom is directly bonded with Oxygen atom, so it will attain partial positive charge and will interact with the Oxygen atom of second Methanol molecule.
CH₃-O-H - - - - -OHCH₃ ∴ - - - - = Hydrogen Bond
Result:
Methanol (CH₃-OH) <span>exhibits hydrogen bonding as its strongest intermolecular force.</span>
Answer:
23.226 psi
Explanation:
From the source,
The mass of the carbon dioxide is:- 16.0 g
Molar mass of carbon dioxide = 44.01 g/mol
The formula for the calculation of moles is shown below:
Thus,
Moles of = 0.3636 moles
Volume = 3.79 L
n = 0.3636 mol
Temperature = 297 K
Using ideal gas equation as:
PV=nRT
where,
P is the pressure
V is the volume
n is the number of moles
T is the temperature
R is Gas constant having value = 0.0821 L.atm/K.mol
Applying the equation as:
P × 3.79 L = 0.3636 mol × 0.0821 L.atm/K.mol × 297 K
⇒P = 2.34 atm
Also, 1 atm = 14.7 psi
So, Pressure = psi = 37.926 psi
THus, pressure by the gas is:-
P = Total pressure - Atmospheric pressure = 37.926 - 14.7 psi = 23.226 psi
<u>The carbon dioxide in the cartridge inflate a 3.79 L mountain bike tire to 23.226 psi pressure.</u>
Answer:
Yes
Explanation:
Lithium can cause nausea, diarrhea, dizziness, change in heart rhythm, muscle weakness, fatigue, and a dazed feeling
Continued use of Lithium could mean fine tremor, frequent urination, and thirst
Source: Webmd.com
Answer:
Option A. It has stayed the same.
Explanation:
To answer the question given above, we assumed:
Initial volume (V₁) = V
Initial temperature (T₁) = T
Initial pressure (P₁) = P
From the question given above, the following data were:
Final volume (V₂) = 2V
Final temperature (T₂) = 2T
Final pressure (P₂) =?
The final pressure of the gas can be obtained as follow:
P₁V₁/T₁ = P₂V₂/T₂
PV/T = P₂ × 2V / 2T
Cross multiply
P₂ × 2V × T = PV × 2T
Divide both side by 2V × T
P₂ = PV × 2T / 2V × T
P₂ = P
Thus, the final pressure is the same as the initial pressure.
Option A gives the correct answer to the question.
Answer: 61.3 g of will be produced from the given masses of both reactants.
Explanation:
To calculate the moles, we use the equation:
a) moles of
b) moles of
According to stoichiometry :
5 moles of require 4 moles of
Thus 2.84 moles of require= of
Thus is the limiting reagent as it limits the formation of product.
As 5 moles of give = 6 moles of
Thus 2.84 moles of give = of
Mass of
Thus 61.3 g of will be produced from the given masses of both reactants.