A system initially has a pressure of 12 atm and a volume of 9 L. What is the volume if the pressure is decreased to 6 atm?
1 answer:
Answer:
<h3>The answer is 18 L</h3>Explanation:
In order to find the volume , we use the formula for Boyle's law which is
where
P1 is the initial pressure
P2 is the final pressure
V1 is the initial volume
V2 is the final volume
Since we are finding the final volume
From the question
P1 = 12 atm
V1 = 9 L
P2 = 6 atm
We have
We have the final answer as
<h3>18 L</h3>Hope this helps you
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Explanation:
It is known that of
=
.
(a) Relation between and
is as follows.
Putting the values into the above formula as follows.
=
= 3.347
Also, relation between pH and is as follows.
pH =
=
= 3.44
Therefore, pH of the buffer is 3.44.
(b) No. of moles of HCl added =
=
= 0.0116 mol
In the given reaction, will react with
to form
Hence, before the reaction:
No. of moles of =
= 0.15 mol
And, no. of moles of =
= 0.12 mol
On the other hand, after the reaction :
No. of moles of = moles present initially - moles added
= (0.15 - 0.0116) mol
= 0.1384 mol
Moles of = moles present initially + moles added
= (0.12 + 0.0116) mol
= 0.1316 mol
As, =
=
= 3.347
Since, volume is both in numerator and denominator, we can use mol instead of concentration.
As, pH =
= 3.347+ log {0.1384/0.1316}
= 3.369
= 3.37 (approx)
Thus, we can conclude that pH after the addition of 1.00 mL of 11.6 M HCl to 1.00 L of the buffer solution is 3.37.
Answer:
0.0010 mol·L⁻¹s⁻¹
Explanation:
Assume the rate law is
rate = k[A][B]²
If you are comparing two rates,
You are cutting each concentration in half, so
Then,