what volume of a 0.272 M solution of HBr is needed for a reaction that requires 49.5 g of HBr? Answer in units of L.
massHBr=VolumeinLiters*Molarity*molmassHBr
solve for VolumeinLiters
To find the volume of the 0.272 M solution of HBr needed for the reaction, we can use the equation:
Molarity(M) = Moles(n) / Volume(V)
First, let's calculate the number of moles of HBr required for the reaction using the given mass:
molar mass of HBr = 1.0079 g/mol (atomic mass of H) + 79.904 g/mol (atomic mass of Br)
= 80.9129 g/mol
moles of HBr = mass / molar mass
= 49.5 g / 80.9129 g/mol
≈ 0.611 moles
Now, we can rearrange the equation to find the volume:
V = n / M
V = 0.611 moles / 0.272 moles/L
V ≈ 2.25 L
Therefore, approximately 2.25 liters (L) of the 0.272 M HBr solution is needed for the reaction.