Question

missed this? watch kcv: simple gas laws and ideal gas law; read section 6.3. you can click on the review link etext. a 48.3 ml sample of gas in a cylinder is warmed from 28°c to 81°c. part a what is its volume at the final temperature? (assume constant pressure.) express your answer in milliliters to three significant figures. view available hint(s) v₂ = ml

Explanation:

Step1: Convert temperatures to Kelvin

Charles's Law requires temperatures in Kelvin.
$T_1=(28 + 273.15)\text{ K}=301.15\text{ K}$
$T_2=(81 + 273.15)\text{ K}=354.15\text{ K}$

Step2: Apply Charles's Law ($\frac{V_1}{T_1}=\frac{V_2}{T_2}$)

We know $V_1 = 48.3\text{ mL}$, $T_1 = 301.15\text{ K}$, and $T_2 = 354.15\text{ K}$. Rearranging for $V_2$ gives $V_2=\frac{V_1T_2}{T_1}$.
Substitute the values:
$V_2=\frac{48.3\times354.15}{301.15}$
$V_2=\frac{48.3\times354.15}{301.15}\approx56.9\text{ mL}$

Answer:

$56.9\text{ mL}$