the universal gas law, pv = nrt, describes the relationship among the pressure, volume, and temperature of a…

the universal gas law, pv = nrt, describes the relationship among the pressure, volume, and temperature of a gas.\np = pressure v = volume\nt = temperature (kelvin)\nn = number of moles (quantity of gas particles)\nr = universal gas constant\nat a constant temperature of 1 k, the pressure and volume of 1 mole of gas vary inversely.\np = \\frac{r}{v}\nuse the values in the table to find the value of r.\n| volume (liters) | pressure (kilopascals) |\n| ---- | ---- |\n| 4.155 | 2 |\n| 16.62 | 0.5 |\n| 33.24 | 0.25 |\nr = \ndone

the universal gas law, pv = nrt, describes the relationship among the pressure, volume, and temperature of a gas.\np = pressure v = volume\nt = temperature (kelvin)\nn = number of moles (quantity of gas particles)\nr = universal gas constant\nat a constant temperature of 1 k, the pressure and volume of 1 mole of gas vary inversely.\np = \\frac{r}{v}\nuse the values in the table to find the value of r.\n| volume (liters) | pressure (kilopascals) |\n| ---- | ---- |\n| 4.155 | 2 |\n| 16.62 | 0.5 |\n| 33.24 | 0.25 |\nr = \ndone

Answer

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