Answer:
the mass of the glycerine needed in the given solution is 23.92 g
Explanation:
Given;
molarity of the solution (C₃H₈O₃), C = 2.60 M
Volume of the solution, V = 100 mL = 100 x 10⁻³ L = 0.1 M
The molarity of a solution is given as follows;
The molecular mass of the given solution;
molecular mass = (12 x 3) + (8 x 1) + (16 x 3)
molecular mass = 92 g/mol
The mass of the glycerine needed in the given solution is calculated as follows;
reacting mass = amount of solute (moles) x molecular mass (g/mol)
reacting mass = 0.26 x 92
reacting mass = 23.92 g
Therefore, the mass of the glycerine needed in the given solution is 23.92 g
Answer:
116.6 lbs
Explanation:
There are 2.2 lbs per Kilogram of weight - and likewise 0.454 Kilograms per pound - but instead of dividing by .454 I multiplied the weight by 2.2 to get 116.6 pounds (of course you could round up and get 117 but 116.6 is a little more accurate).
Answer:
If the volume of the container is decreased by a factor of 2 the pressure is is increased by the same factor to 1664 torr.
Explanation:
Here we have Boyle's law which states that, at constant temperature, the volume of a given mass of gas is inversely proportional to its pressure
V ∝ 1/P or V₁·P₁ = V₂·P₂
Where:
V₁ = Initial volume
V₂ = Final volume = V₁/2
P₁ = Initial pressure = 832 torr
P₂ = Final pressure = Required
From V₁·P₁ = V₂·P₂ we have,
P₂ = V₁·P₁/V₂ = V₁·P₁/(V₁/2)
P₂ = 2·V₁·P₁/V₁ = 2·P₁ = 2× 832 torr = 1664 torr
