Question

the ideal gas equation is
$$pv = nrt$$
where $p$ is pressure, $v$ is volume, $n$ is the number of moles, $r$ is a constant, and $t$ is temperature.
you are told that a sample of gas has a pressure of $p = 843$ torr, a volume of $v = 5230$ ml, and a temperature of $t = 303$ k. if you use $r = 8.200 \times 10^{-2} \text{ l·atm/(k·mol)}$, which of the following conversions would be necessary before you could find the number of moles of gas, $n$, in this sample?
check all that apply.

• view available hint(s)
• convert the pressure to atmospheres (atm)
• convert the pressure to pascals (pa)
• convert the volume to cubic meters ($\text{m}^3$)
• convert the volume to liters (l)
• convert the temperature to degrees celsius ($\degree \text{c}$)
• convert the temperature to degrees fahrenheit ($\degree \text{f}$)

Explanation:

Step1: Match R's units to given values

The gas constant $R = 8.206 \times 10^{-2}\ \text{L·atm/(K·mol)}$ has units of liters (L), atmospheres (atm), Kelvin (K), and moles.

Step2: Analyze pressure units

Given pressure $P = 843\ \text{torr}$; need to convert to atm to match $R$'s pressure unit.

Step3: Analyze volume units

Given volume $V = 5230\ \text{mL}$; need to convert to liters (L) to match $R$'s volume unit.

Step4: Analyze temperature units

Given temperature $T = 303\ \text{K}$, which already matches $R$'s temperature unit, so no conversion needed.

Answer:

• Convert the pressure to atmospheres (atm)
• Convert the volume to liters (L)