•3.9g of ammonia
•molar mass of ammonia = 17.03g/mol
1st you have to covert grams to moles by dividing the mass of ammonia with the molar mass:
(3.9 g)/ (17.03g/mol) = 0.22900763mols
Then convert the moles to molecules by multiplying it with Avogadro’s number:
Avogadro’s number: 6.022 x 10^23
0.22900763mols x (6.022 x 10^23 molecs/mol)
= 1.38 x 10^23 molecules
It is true yes :) happy to help
Answer:
DECREASE BY A FACTOR OF FOUR
Explanation:
Using pressure equation:
P 1 / T1 = P2 /T2 (at constant volume)
P1 = P
T1 =T
P2 = ?
T2 = 4 T
So therefore;
P2 = P1T1/ T2
P2 = P T/ 4 T
P2 = 1/4 P
The pressure is decreased by a factor of four, the new pressure is a quarter of the formal pressure of the gas.
Mass/volume cause you divide to get density
