Question

How many moles of chlorine gas at 120.0 °c and 26.1 bar would occupy a vessel of 31.0 l?

r = 0.08314 l･bar/mol･k.
a. 14.8 mol
b. 25.2 mol
c. 18.3 mol
d. 20.1 mol

Answer 1

Using the ideal gas law, PV = nRT, and substituting the provided values, the calculation reveals that 25.2 moles of chlorine gas occupy a vessel of 31.0 L at 120.0 °C and 26.1 bar, which corresponds to answer choice (b).

Step-by-step explanation:

To calculate the number of moles of chlorine gas that would occupy a vessel of 31.0 L at 120.0 °C (393 K) and 26.1 bar, we can use the ideal gas law:

PV = nRT

where P is the pressure in bars, V is the volume in liters, n is the number of moles of the gas, R is the universal gas constant (0.08314 L·bar/mol·K), and T is the temperature in Kelvin.

Rearranging the equation to solve for n (number of moles), we get:

n = PV / RT

Substituting the given values into the equation:

n = (26.1 bar)(31.0 L) / ((0.08314 L·bar/mol·K)(393 K))

After performing the calculation:

n = 25.2 mol

Therefore, 25.2 moles of chlorine gas would occupy a vessel of 31.0 L at 120.0 °C and 26.1 bar, which corresponds to answer choice (b).