Find the mass of 0.456 mol of Ca(OH)2 Please if you can show the work.
2 answers:
<h2>Answer:</h2>
<em>Hey, </em>
<h3><u>QUESTION)</u></h3>A) Let's first calculate the molar mass M of the molecule :
<em>M(Ca(OH)₂) = M(Ca) + 2M(O) + 2M(H) </em>
- M(Ca(OH)₂) = 40 + 2 x 16 + 2 x 1
- M(Ca(OH)₂) = 74 g/mol
B) Let's deduct the corresponding mass m :
<em>m = M x n </em>
- m = 74 x 0.456
- m = 33.744 g
- m ≈ 34,0 g
The mass of calcium hydroxide corresponding to this quantity of substance (in mol) is therefore 34 g.
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Answer:
Explanation:
Your unbalanced nuclear equation is:
The main point to remember in balancing nuclear equations is that the sums of the superscripts and the subscripts must be the same on each side of the equation.
Then
84 = x + 2, so x = 84 - 2 = 82
210 = y + 4, so y = 210 - 4 = 206
Element 82 is lead, so the nuclear equation becomes
0.012moldm⁻³
Explanation:
Given parameters:
Mass of AgNO₃ = 1000mg
Volume of water = 500mL
Unknown:
Molarity of solution = ?
Solution:
The molarity of a solution is the number of moles of a solute dissolved in volume of solvent.
Molarity =
Number of moles of AgNO₃ = ?
Number of moles =
Molar mass of AgNO₃ = 108 + 14 + 3(16) = 170g/mol
convert mass to g;
1000mg = 1g
Number of moles = = 0.00588moles
convert the given volume to dm³;
1000mL = 1dm³;
500mL = 0.5dm³
Now solve;
Molarity = = 0.012moldm⁻³
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Molarity brainly.com/question/9324116
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