For this case we have that by definition:
[tex]PV = nRT[/tex]
Where,
Since the pressure, the number of moles and the universal constant do not change, then the equation is reduced to:
[tex]V = kT[/tex]
Rewriting we have:
[tex]k = \frac {V} {T}[/tex]
Matching state 1 and state 2, we have:
[tex]\frac {V1} {T1} = \frac {V2} {T2}[/tex]
Clearing the volume in state 2 we have:
[tex]V2 = T2 (\frac {V1} {T1})[/tex]
Then, replacing values:
[tex]V2 = (17+273) (\frac {61.3} {68+273})\\V2 = 52.13 mL[/tex]
Rounding off we have:
[tex]V2 = 52 mL[/tex]
Answer:
The volume of the gas at 17 ° C would be:
[tex]V2 = 52 mL[/tex]
Option A
A certain quantity of a gas occupies 61.3 mL at 68°C and 52 mL at 17 °C.
Charles' law states that the volume of an ideal gas at constant pressure is directly proportional to the absolute temperature.
A certain quantity of a gas occupies 61.3 mL at 68°C (341 K). We can calculate the volume at 17°C (290 K) using Charles' law.
V1/T1 = V2/T2
V2 = V1 . T2/T1
V2 = 61.3 mL . 290 K/341 K = 52 mL
where,
A certain quantity of a gas occupies 61.3 mL at 68°C and 52 mL at 17 °C.
Learn more about Charles' law here: https://brainly.com/question/888898
