Consider a balloon that has a volume V. It contains n moles of gas, it has an internal pressure of P, and its temperature is T.
2 answers:
Answer: The temperature will not change and will remain T.
Explanation: Accoding to ideal gas law:
where,
P = pressure of the gas
V = volume of the gas
T = temperature of the gas
n = number of moles of gas
R = Gas constant = 0.0821 Latm/moleK
= initial pressure
= initial volume
= initial temperature
= final pressure
= final volume
= final temperature
Putting in the values:
You might be interested in
Answer:
1) After adding 15.0 mL of the HCl solution, the mixture is before the equivalence point on the titration curve.
2) The pH of the solution after adding HCl is 12.6
Explanation:
10.0 mL of 0.25 M NaOH(aq) react with 15.0 mL of 0.10 M HCl(aq). Let's calculate the moles of each reactant.
There is an excess of NaOH so the mixture is before the equivalence point. When HCl completely reacts, we can calculate the moles in excess of NaOH.
NaOH + HCl ⇒ NaCl + H₂O
Initial 2.5 × 10⁻³ 1.5 × 10⁻³ 0 0
Reaction -1.5 × 10⁻³ -1.5 × 10⁻³ 1.5 × 10⁻³ 1.5 × 10⁻³
Final 1.0 × 10⁻³ 0 1.5 × 10⁻³ 1.5 × 10⁻³
The concentration of NaOH is:
NaOH is a strong base so [OH⁻] = [NaOH].
Finally, we can calculate pOH and pH.
pOH = -log [OH⁻] = -log 0.040 = 1.4
pH = 14 - pOH = 14 - 1.4 = 12.6
Answer:
Explanation:
If you insist on filling in the first blank you can put a one.
