Answer:
The empirical formula is the simplest form;
Given:
Oxygen O at 94.1% and
H at 5.9%
Assume 100grams.
94% = 0.941 x 100gm. = 94.1 gm x 1mole/16gm. = 5.88 moles of O
5.9% = 0.059 x 100gm. = 5.9gm. X 1moleH/1.002gm. = 5.88 moles of H
There is one mole of O for each mole of H so the empirical formula is 
and written as OH.
if you have 1mol of NO. how many molecules of NO are there
Answer:
6.02 x 10²³ molecules
Explanation:
Given parameters:
Number of moles of NO = 1 mole
Unknown:
Number of molecules in NO;
Solution:
A mole of compound contains the Avogadro's number of particles.
1 mole of a substance contains 6.02 x 10²³ molecules
So, 1 mole of NO contained 6.02 x 10²³ molecules
Answer:
A. The model could not explain how alpha particles could be deflected at large angles.
Explanation:
The plum pudding model of the atom was proposed by J. J Thomson. He suggested that that an atom is made up of dense particles of electrons surrounded by positive charges.
From the Gold foil experiment carried out by Ernest Rutherford, he noticed that the bulk of the alpha particles targeted at the foil passed through and a little fraction was heavily deflected back.
Rutherford then presented his nuclear model from here. He suggested a massive, dense and tiny nucleus where the protons and neutrons are located. The space outside the mass is dominated by orbiting electrons.
Answer:
B. The pressure has increased
Explanation:
