First convert volume to mass:
mass = 0.789 g/mL * 155 mL = 122.295 g
Then convert mass to number of moles:
number of moles = 122.295 g * (1 mole / 46 g) = 2.66 moles
Using avogadros number, we get the molecules:
<span>number of molecules = 2.66 moles * 6.022 x 10^23 molecules
/ mole = 1.6 x 10^24 molecules</span>
An Erlenmeyer flask is laboratory flask that has a conical shape and flat bottom with a tapered mouth. The Erlenmeyer flask is used for pouring, mixing and storing of chemicals in the laboratory. It was created by Emil Erlenmeyer in the 1860s.
Answer:
43.13Kg of melamine
Explanation:
The problem gives you the mass of urea and two balanced equations:
First we need to calculate the number of moles of urea that are used in the reaction, so:
molar mass of urea = 
The problem says that you have 161.2Kg of urea, so you take that mass of urea and find the moles of urea:
161.2Kg of urea
2684 moles of urea
Now from the stoichiometry you have:
2684 moles of urea
= 447 moles of melamine
The molar mass of the melamine is 
so we have:
= 5637.64 g of melamine
Converting that mass of melamine to Kg:
5637.64 g of melamine *
= 56.38 Kg of melamine, that is the theoretical yield of melamine.
Finally we need to calculate the mass of melamine with a yield of 76.5%, so we have:
%yield = 100*(Actual yield of melamine / Theoretical yield of melamine)
Actual yield of melamine = 
= 43.13Kg of melamine
Answer:
1,) True
2.) False
3.) A Moraine
Explanation:
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Answer is: <span> 3. 5.2x10−7.
</span>Balanced chemical reaction (dissociation):
Ba₃(PO₄)₂(s) → 3Ba²⁺(aq) + 2PO₄³⁻(aq).
[Ba²⁺<span>] = 0,0005 M.
</span>Ksp(Ba₃(PO₄)₂) = 3,4·10⁻²³.
Ksp = [Ba²⁺]³ · [PO₄³⁻]².
3,4·10⁻²³ = (0,0005 M)³ · [PO₄³⁻]².
[PO₄³⁻] = √3,4·10⁻²³ ÷ 1,25·10⁻¹⁰.
[PO₄³⁻] = 5,2·10⁻⁷ M.
<span>Ksp is the solubility product constant for a solid substance
dissolving in an aqueous solution.
</span>
