Answer:
e. T₂= 4T₁
Explanation:
Initially, we have a number of moles (n₁) a gas sample at a certain pressure (P), temperature (T₁) and volume (V). We can relate these variables through the ideal gas equation.
P . V = n₁ . R . T₁
where,
R is the ideal gas constant
We can rearrange this equation like:
If only one fourth of the initial molecules remain n₂ = 1/4 n₁. The new temperature (T₂) assuming pressure and temperature remain constant is:
1) (C2H5)2CBrCH2CH3 is the answer
explaiation:-
so when HBr is added to an alkene , according to the Markonicoff's rule ...H atoms are bonded to the C containing the most amount of H and Br is added to the other C.
2) Just add alkoholic KOH∆
Answer:
The predominant intermolecular force in the liquid state of each of these compounds:
ammonia (NH3)
methane (CH4)
and nitrogen trifluoride (NF3)
Explanation:
The types of intermolecular forces:
1.Hydrogen bonding: It is a weak electrostatic force of attraction that exists between the hydrogen atom and a highly electronegative atom like N,O,F.
2.Dipole-dipole interactions: They exist between the oppositely charged dipoles in a polar covalent molecule.
3. London dispersion forces exist between all the atoms and molecules.
NH3 ammonia consists of intermolecular H-bonding.
Methane has London dispersion forces.
Because both carbon and hydrogen has almost similar electronegativity values.
NF3 has dipole-dipole interactions due to the electronegativity variations between nitrogen and fluorine.
Answer:
The correct answer is 6 possible states
Explanation:
