The density of the liquid is 0.2 g/mL.
The mass of the liquid is 6 g.
The volume of the liquid is 30.0 mL.
Density = mass/volume = 6 g/30.0 mL = 0.2 g/mL
Answer:
Ca2s that is answers and CuSO4is
The mass of C₂H₂ that would be produced by complete reaction of 3.75 g of calcium carbide is 1.524 grams
<u><em>calculation</em></u>
calcium carbide (CaC₂) react with water(H₂O) to produce C₂H₂ and Ca(OH)₂ according to reaction below
CaC₂ +2H₂O C₂H₂ + Ca(OH)₂
calculate the moles of CaC₂
moles = mass÷ molar mass
from periodic table the molar mass of CaC₂ = 40 + (12 x2) = 64 g/mol
moles is therefore =3.75 g÷ 64 g/mol =0.0586 moles
Use the mole ratio to determine the moles of C₂H₂
from equation above CaC₂: C₂H₂ is 1:1 therefore the moles of C₂H₂ is also
= 0.0586 moles
mass of C₂H₂ = moles x molar mass
from periodic table the molar mass of C₂H₂ = (12 x 2) + (1 x 2) = 26 g/mol
mass =0.0586 moles x 26 g/mol =1.524 grams
Answer:
9.4L
Explanation:
Given parameters:
Mass of Cl₂ gas = 30g
Unknown:
Volume of gas = ?
Solution:
To solve this problem, let us assume that this reaction takes place under standard temperature and pressure conditions.
Therefore;
Volume of gas = number of moles x 22.4
To find the number of moles;
Number of moles = 
molar mass of Cl₂ = 2(35.5) = 71g/mol
Number of moles = 
= 0.42mole
So;
Volume of gas = 0.42 x 22.4 = 9.4L
