<h3>Further explanation</h3>
Given
Reaction
H₂ (g) + I₂ (g) → 2HI(g)
Required
The equilibrium constant
Solution
The equilibrium constant is the value of the product in the equilibrium state of the substance in the right (product) divided by the substance in the left (reactant) with the exponents of each reaction coefficient
The equilibrium constant for reaction
pA + qB ⇒ mC + nD
So for the above reaction :
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:
The activation energy was reached was 10:45 a.m. The additional energy did not affect the reaction.
Explanation:
The number of moles of O2 that are needed to react with 24 moles of C2H6 is 84 moles of O2
<u><em>Explanation</em></u>
Step 1: write the equation for reaction
= 2C2H6 +7O2 → 4CO2 + 6H2O
Step 2: use the mole ratio to determine the moles of O2
- that is the mole ratio of C2H6 : O2 is 2:7
- therefore the moles of O2= 24 x7/2= 84 moles of O2
A solvent is something that can have something else dissolved within it and turn into a homogenous solution, while the solute is that something else that can be dissolved into the solvent. Usually, the solvent is found in greater amount because most (except for rare cases) solvents have a saturation point that is below the equal-mass point.