A 20 ml sample of .875 m hcl solution was diluted t o150 ml. calculate the molarity of the resulting solution
1 answer:
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Complete question:
The decomposition of SO2Cl2 is first order in SO2Cl2 and has a rate constant of 1.44×10⁻⁴ s⁻¹ at a certain temperature.
If the initial concentration of SO2Cl2 is 0.125 M , what is the concentration of SO2Cl2 after 210 s ?
Answer:
After 210 s the concentration of SO2Cl2 will be 0.121 M
Explanation:
where;
At is the concentration of A at a time t
A₀ is the initial concentration of A
k is rate constant = 1.44×10⁻⁴ s⁻¹
t is time
ln(At/A₀) = -( 1.44×10⁻⁴)t
ln(At/0.125) = -( 1.44×10⁻⁴)210
ln(At/0.125) = -0.03024
At/0.125 = 0.9702
At = 0.125*0.9702
At = 0.121 M
Therefore, after 210 s the concentration of SO2Cl2 will be 0.121 M
This is an exercise in the general or combined gas law.
To start solving this exercise, we obtain the following data:
<h3>Data:</h3>- T₁ = 22.5 °C + 273 = 295.5 K
- P₁ = 1.95 atm
- V₁ = ¿?
- P₂ = 3.69 atm
- T₂ = 11.9 °C + 273 = 284.9 k
- V₂= 56.4 ml
We use the following formula:
P₁V₁T₂ = P₂V₂T₁ ⇒ General formula
Where
- P₁ = Initial pressure
- V₁ = Initial volume
- T₂ = Initial temperature
- P₂ = Final pressure
- V₂ = final volume
- T₁ = Initial temperature
We clear the formula for the initial volume:
We substitute our data into the formula to solve:
The helium-filled balloon has a volume of <u>110.697 ml.</u>