1.Calculate the mass of compound required to prepare 100.00 mL of a 1.40x10-2M CuCl2.Show your work.
1 answer:
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The density of a rectangle : ρ = 0.372 g/cm³
<h3>Further explanation</h3>Given
The volume of rectangle : 395 cm³
Mass : 147 g
Required
The density
Solution
Density is a quantity derived from the mass and volume
Density is the ratio of mass per unit volume
Density formula:
ρ = density
m = mass
v = volume
Input the value :
ρ = 147 g : 395 cm³
ρ = 0.372 g/cm³
Answer: The empirical formula for the given compound is
Explanation:
The chemical equation for the combustion of compound having carbon and hydrogen follows:
where, 'x' and 'y' are the subscripts of carbon and hydrogen respectively.
We are given:
Mass of
We know that:
Molar mass of carbon dioxide = 44 g/mol
For calculating the mass of carbon:
In 44 g of carbon dioxide, 12 g of carbon is contained.
So, in 22.0 g of carbon dioxide, of carbon will be contained.
For calculating the mass of hydrogen:
Mass of hydrogen = Mass of sample - Mass of carbon
Mass of hydrogen = 7.0 g - 6 g
Mass of hydrogen = 1.0 g
To formulate the empirical formula, we need to follow some steps:
Step 1: Converting the given masses into moles.
Moles of Carbon =
Moles of Hydrogen =
Step 2: Calculating the mole ratio of the given elements.
For the mole ratio, we divide each value of the moles by the smallest number of moles calculated which is 0.5 moles.
For Carbon =
For Hydrogen =
Step 3: Taking the mole ratio as their subscripts.
The ratio of Fe : C : H = 1 : 2
Hence, the empirical formula for the given compound is