0.6675 moles of solute are present in .75 l of a .89 m (molar) solution.
<h3>Define the molarity of a solution.</h3>
Molarity (M) is the amount of a substance in a certain volume of solution. Molarity is defined as the moles of a solute per litres of a solution.
Given data:
V= 0.75
M=0.89
Molality = 
0.89 M= 
Moles= 0.6675
Hence, 0.6675 moles of solute are present in .75 l of a .89 m (molar) solution.
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4.176 g of Al that was reacted with excess HCl if 2.12 L of hydrogen gas were collected at STP in the following reaction.
2 Al (s) + 6 HCl (aq) → 2 AlCl₃ (aq) + 3 H₂ (g)
<h3>What is an ideal gas equation?</h3>
The ideal gas law (PV = nRT) relates the macroscopic properties of ideal gases. An ideal gas is a gas in which the particles (a) do not attract or repel one another and (b) take up no space (have no volume).
2 Al (s) + 6 HCl (aq) → 2 AlCl₃ (aq) + 3 H₂ (g)
Given data:
Volume of
(g) = 5.20L
At STP
Pressure= 1 atm
Temperature =273K
R = 0.0821 L.atm/mol K
PV=nRT
n= 
n= 
n= 0.2324 mol 
2 Al (s) + 6 HCl (aq) → 2 AlCl₃ (aq) + 3 H₂ (g)
=

=4.176 g of Al
Hence, 4.176 g of Al that were reacted with excess HCl if 2.12 L of hydrogen gas were collected at STP in the following reaction.
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Convert the 48.7 grams into moles and then use the balanced equation to convert to moles of hydrogen gas. Then divide by avogadro's number<span />
They are atoms like hydrogen oxygen or nitrogen
Explanation:
atomic number;number of protons in an atom of an element.
mass number ;number of nucleons ( neutrons) in an atom of an element.