Answer: C2H6O2
Explanation: solution attached:
First convert mass to moles.
Second divide each moles on the lowest amount to find the number of atoms in the empirical formula.
Third calculate the empirical formula mass.
Fourth calculate for the molecular formula by dividing the molar mass over the empirical formula mass.
Fifth multiply the empirical formula by the answer and that is the molecular formula of the compound.
Answer:
2.83 g
Explanation:
At constant temperature and pressure, Using Avogadro's law
Given ,
V₁ = 2.12 L
V₂ = 3.12 L
n₁ = 0.120 moles
n₂ = ?
Using above equation as:
n₂ = 0.17660 moles
Molar mass of methane gas = 16.05 g/mol
So, Mass = Moles*Molar mass = 0.17660 * 16.05 g = 2.83 g
<u>2.83 g are in the piston.</u>
Answer:
Here's what I get
Explanation:
(g) Titration curves
I can't draw two curves on the same graph, but I can draw two separate curves for you.
The graph in part (d) had an equivalence point at 20 mL.
In the second titration, the NaOH was twice as concentrated, so the volume to equivalence point would be half as much — 10 mL.
The two titration curves are below.
(h) Evidence of reaction
HCl and NaOH are both colourless.
They don't evolve a gas or form a precipitate when they react.
The student probably noticed that the Erlenmeyer flask warmed up — a sign of a chemical change.
