It is B: Fixed volume, takes the shape of the container
Answer:
Making oxygen
Oxygen can be made from hydrogen peroxide, which decomposes slowly to form water and oxygen:
hydrogen peroxide → water + oxygen
2H2O2(aq) → 2H2O(l) + O2(g)
The rate of reaction can be increased using a catalyst, manganese(IV) oxide. When manganese(IV) oxide is added to hydrogen peroxide, bubbles of oxygen are given off.
Apparatus arranged to measure the volume of gas in a reaction. Reaction mixture is in a flask and gas travels out through a pipe in the top and down into a trough of water. It then bubbles up through a beehive shelf into an upturned glass jar filled with water. The gas collects at the top of the jar, forcing water out into the trough below.
To make oxygen in the laboratory, hydrogen peroxide is poured into a conical flask containing some manganese(IV) oxide. The gas produced is collected in an upside-down gas jar filled with water. As the oxygen collects in the top of the gas jar, it pushes the water out.
Instead of the gas jar and water bath, a gas syringe could be used to collect the oxygen.
Si -Atomic number -14 -1s2 2s2 2p6 3s2 3p2 - 4 valence electrons
The two samples don’t contain different atoms so it will be false
The given question is incomplete. The complete question is
If 1.0 M HI is placed into a closed container and the reaction is allowed to reach equilibrium at 25∘C∘C, what is the equilibrium concentration of H2 (g). Given the equilibrium constant is 62.
Answer: The equilibrium concentration of 
is 0.498 M
Explanation:
Initial concentration of 
= 1.0 M
The given balanced equilibrium reaction is,
initial (1.0) M 0 0
At eqm (1.0-2x) M (x) M (x) M
The expression for equilibrium constant for this reaction will be,
![K_c=\frac{[H_2]\times [I_2]}{[HI]^2}](https://tex.z-dn.net/?f=K_c%3D%5Cfrac%7B%5BH_2%5D%5Ctimes%20%5BI_2%5D%7D%7B%5BHI%5D%5E2%7D)
Now put all the given values in this expression, we get :
By solving we get :
Thus the equilibrium concentration of is 0.498 M
