Question

# Complete the following table for an ideal gas.$\begin{matrix} \text{ } & \text{P} & \text{V} & \text{n} & \text{T}\\ \hline \text{a.} & \text{7.74 \times 10^{3} \mathrm{Pa}} & \text{12.2 mL} & \text{ } & \text{25^{\circ} \mathrm{C}}\\ \end{matrix}$

Solution

Verified
Step 1
1 of 2

We simply use and rearrange the ideal gas equation to solve for the missing molar amount ($n$). Temperatures should strictly be converted to Kelvin before calculations (25 $^o$C = 298.2 K). Volume should be in liters and pressure should be in atm (7.74 $\times 10^{3}$ Pa = 0.0764 atm):

\begin{align*} PV &= nRT\\ n &= \dfrac{PV}{RT}\\ &= \mathrm{\dfrac{(0.0764~atm)(0.0122~L)}{(0.08206~\frac{L \cdot atm}{mol \cdot K})(298.2~K)}}\\ &= \boxed{\mathrm{3.81 \times 10^{-5} ~mol}}\\ \end{align*}

## Recommended textbook solutions #### Chemistry: The Molecular Nature of Matter and Change

7th EditionISBN: 9780073511177 (4 more)Patricia Amateis, Silberberg
3,171 solutions #### Chemistry

9th EditionISBN: 9781133611097 (16 more)Steven S. Zumdahl, Susan A. Zumdahl
5,605 solutions #### Chemistry

10th EditionISBN: 9781305957404 (1 more)Donald J. DeCoste, Steven S. Zumdahl, Susan A. Zumdahl
5,864 solutions #### Chemistry, AP Edition

10th EditionISBN: 9781305957732Donald J. DeCoste, Steven S. Zumdahl, Susan A. Zumdahl
5,934 solutions