Question

the universal gas law, pv = nrt, describes the relationship among the pressure, volume, and temperature of a gas.
p = pressure v = volume
t = temperature (kelvin)
n = number of moles (quantity of gas particles)
r = universal gas constant
at a constant temperature of 1 k, the pressure and volume of 1 mole of gas vary inversely.
p = \frac{r}{v}
use the values in the table to find the value of r.

volume (liters)	pressure (kilopascals)
16.62	0.5
33.24	0.25

r =
done

Explanation:

Step1: Recall the ideal - gas law formula

Given $pV = nRT$, when $n = 1$ mole and $T=1$ K, the formula simplifies to $pV=R$.

Step2: Calculate $pV$ for each row

For the first row: $p = 2$ kPa and $V = 4.155$ L, so $pV=2\times4.155 = 8.31$ L·kPa.
For the second row: $p = 0.5$ kPa and $V = 16.62$ L, so $pV=0.5\times16.62 = 8.31$ L·kPa.
For the third row: $p = 0.25$ kPa and $V = 33.24$ L, so $pV=0.25\times33.24 = 8.31$ L·kPa.

Answer:

$8.31$ L·kPa