The chemical reaction involving Mg(OH)2 and HCl is:
<span>Mg(OH)2 + 2HCl
--> MgCl2 + 2H2O</span>
So we see that for every 2 moles of HCl, 1 mole of Mg is
reacted.
Calculating for moles HCl:
moles HCl = 0.300 M * 0.215 L
moles HCl = 0.0645 mol
The moles Mg then is:
moles Mg = 0.0645 mol * (1 / 2)
<span>moles Mg = 0.03225 mol</span>
Missing question: <span>A 5.00 L sample of O2 at a given temperature and pressure contains a 1.08x10^23 molecules. How many molecules would be contained in each of the following at the same temperature and pressure? </span>
a) 5.00 L H2.
<span>b) 5.00 L CO2.
Use </span>Avogadro's Law: The Volume Amount Law: <span>equal </span>volumes<span> of all gases, at the same temperature and pressure, have the same </span>number<span> of molecules. Because hydrogen and carbon(IV) oxide are gases, number of molecules are the same as number of oxygen molecules, so:
a) N(H</span>₂) = 1.08·10²³.
b) N(CO₂) = 1.08·10²³
Answer:
it would be the ideal gas law also known as Avagadro's law
Explanation:
Answer:
i think protons and neutrons
Explanation:
im not sure tho