Some physical properties of the compound are related in this way.
Molecular mass of the compound, depends on the atomic masses of the elements.
Wether the compound is ionic or covalent depends on the nature of the bonds which depends on the electronic configuration of the elements.
Boiling pont depends, solubility, melting point and others depend on the strength of the bonds, wich depends on the electronic configuration of the elements.
So many other properties also are determined by the properties of the elements and the bonding of them to form the compound.
Solubility of the compound depends on
Answer:
Explanation:
Arrhenius defined an acid as a substance that interacts with water to produce excess hydrogen ions in aqueous solution.
A base is a substance which interacts with water to yield excess hydroxide ions, in an aqueous solution according to Arrhenius.
Bronsted-Lowry theory defined an acid as a proton donor while a base is a proton acceptor.
Nitrogen gas has the chemical formula N2. One molecule of nitrogen gas is made up of two atoms of nitrogen.
The correct option is C.
Explanation:
Nitrogen gas has the chemical formula
, which means that two atoms of nitrogen element combined to form nitrogen gas.
The combination of two atoms of element nitrogen produce dinitrogen atom.
Dinitrogen is the nitrogen gas usually present in atmosphere of the earth in abundance.
2 atoms of nitrogen element
N + N = ![N_{2}](https://tex.z-dn.net/?f=N_%7B2%7D)
the gas is colorless and odorless formed at standard condition of temperature and pressure. The two nitrogen atoms are tightly bonded with triple bonds in between the atoms.
The volume that would be occupied by 0.25 moles sample of H2 is calculated using ideal gas equation formula
that is PV =nRT
P(pressure)= 1.7 atm
V( volume)?
n(number of moles)= 0.250 moles
R(gas constant)=0.0821 l.atm/mol.K
T (temperature in kelvin)=35+273 = 308k
by making V the subject of the formula V=nRT/P
=(0.250 moles x 0.0821 L.atm/k.mol x 308 k)/( 1.70 atm) = 3.7 L of H2 gas
there are <u>4 </u>grams of product produced by the chemical reaction