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. Use the values in the table to find the value of R. volume (Liters): 4.155, 16.62, 33.24. pressure: 2, 0.5, 0.25

Answer 1

Answer:

The value of R is, 8.31

Step-by-step explanation:

Given the universal gas law:

pV = nRT              ....[1]

where,

p = pressure

V = volume

T = temperature (Kelvin)

n = number of moles (quantity of gas particles)

R = universal gas constant

It is given that at a constant temperature of 1 K, the pressure and volume of 1 mole of gas vary inversely.

⇒T = 1 K and n = 1

Since, pressure and volume varies inversely.

⇒$pV = k$   where, k is constant

to find k:

From the given table:

p=2 and V = 4.155

then;

$2 \cdot 4.155 = k$

⇒$8.31 = k$

or

k = 8.31

$pV =8.31$

We have to find value of R:

Substitute pV = 8.31 and the given values in [1] we have;

$8.31 = 1 \cdot R \cdot 1$

⇒$8.31 = R$

or

$R = 8.31$

Therefore, the value of R is, 8.31

Answer 2

Answer:

R ≈ 8.31

Step-by-step explanation:

Filling in the given values ...

... pV = nRT

... 2·4.155 = 1·R·1

... 8.31 = R