A certain gas is present in a 13.0 l cylinder at 4.0 atm pressure. if the pressure is increased to 8.0 atm , the volume of the g
2 answers:
Answer:
Yes, gas is obeying the Boyle's law.
Explanation:
Boyle's Law states that 'pressure is inversely proportional to the volume of the gas at constant temperature and number of moles'.
(At constant temperature and number of moles)
Initial volume of the gas =
Initial pressure of the gas =
Initial value of k :
Final volume of the gas =
Final pressure of the gas =
Final value of k :
As we can see that initial value of k is equal to the final value of k which means that gas is obeying the Boyle's law.
You might be interested in
Hope this helpssssssnsnekwnwjwj
The pink color in the solution fades. Some of the colored indicator ion converts to the colorless indicator molecule.
<h3>Explanation</h3>What's the initial color of the solution?
is a salt soluble in water.
dissociates into ions completely when dissolved.
.
The first test tube used to contain .
is a weak base that dissociates partially in water.
.
There's also an equilibrium between and
ions.
.
ions from
will shift the equilibrium between
and
to the right and reduce the amount of
in the solution.
The indicator equilibrium will shift to the right to produce more ions along with the colored indicator ions. The solution will show a pink color.
What's the color of the solution after adding NH₄Cl?
Adding will add to the concentration of
ions in the solution. Some of the
ions will combine with
ions to produce
.
The equilibrium between and
ions will shift to the left to produce more of both ions.
The indicator equilibrium will shift to the left as the concentration of increases. There will be less colored ions and more colorless molecules in the test tube. The pink color will fade.