Question

A certain quantity of a gas occupies 61.3 mL at 68°C. If the pressure remains constant, what would the volume of the gas be at 17°C?A. 52 mLB. 72 mLC. 32 mLD. 92 mL

Answer 1

For this case we have that by definition:

$PV = nRT$

Where,

• P: Pressure
• V: volume
• n: number of moles
• R: universes constant of gases
• T: temperature

Since the pressure, the number of moles and the universal constant do not change, then the equation is reduced to:

$V = kT$

Rewriting we have:

$k = \frac {V} {T}$

Matching state 1 and state 2, we have:

$\frac {V1} {T1} = \frac {V2} {T2}$

Clearing the volume in state 2 we have:

$V2 = T2 (\frac {V1} {T1})$

Then, replacing values:

$V2 = (17+273) (\frac {61.3} {68+273})\\V2 = 52.13 mL$

Rounding off we have:

$V2 = 52 mL$

Answer:

The volume of the gas at 17 ° C would be:

$V2 = 52 mL$

Option A