Probably Sulfur, low mp and hardness compared to the other metals
Answer:
Explanation:
Depression in freezing point is given by:

= Depression in freezing point
i= vant hoff factor = 1 (for non electrolyte like urea)
= freezing point constant = 
m= molality

Weight of solvent (X)= 950 g = 0.95 kg
Molar mass of non electrolyte (urea) = 60.06 g/mol
Mass of non electrolyte (urea) added = ?


Thus
urea was dissolved.
Answer: The net change in the atoms is the conversion of a neutron to a proton, turning Carbon (6 protons) into Nitrogen (7 protons).
Explanation:
Carbon-14, generated from the atmosphere, has 6 protons and 8 neutrons. That's where the 14 comes from, called the mass number, is the sum of protons and neutrons (6+8=14).
Carbon-14 is radioactive and decays by beta decay. That means one of its neutrons spontaneously turns into a proton, an electron, and a neutrino, according to:

After that, the atom has 7 protons and 7 neutrons, maintaining its mass number but changing its atomic number from 6 to 7, turning into Nitrogen.
Answer:
The entropy change for a real, irreversible process is equal to <u>zero.</u>
The correct option is<u> 'c'.</u>
Explanation:
<u>Lets look around all the given options -:</u>
(a) the entropy change for a theoretical reversible process with the same initial and final states , since the entropy change is equal and opposite in reversible process , thus this option in not correct.
(b) equal to the entropy change for the same process performed reversibly ONLY if the process can be reversed at all. Since , the change is same as well as opposite too . Therefore , this statement is also not true .
(c) zero. This option is true because We generate more entropy in an irreversible process. Because no heat moves into or out of the surroundings during the procedure, the entropy change of the surroundings is zero.
(d) impossible to tell. This option is invalid , thus incorrect .
<u>Hence , the correct option is 'c' that is zero.</u>
first we have to find the empirical formula of the compound
empirical formula is the simplest ratio of whole numbers of components making up a compound
for 100 g of the compound
N O
mass 46.7 g 53.3 g
number of 46.7 g/ 14 g/mol 53.3 g/ 16 g/mol
moles = 3.34 mol = 3.33 mol
divide by the least number of moles
3.34/3.33 = 1.00 3.33/ 3,33 = 1.00
therefore number of atoms are
N - 1
O - 1
empirical formula is - NO
mass of empirical unit - 14 g/mol + 16 g/mol = 30 g
molecular formula is actual composition of elements in the compound
molecular mass - 60.01 g/mol
number of empirical units = molecular mass / empirical unit mass
= 60.01 g/mol / 30 g = 2
there are 2 empirical units
2(NO)
molecular formula = N₂O₂