Question

How many moles of chlorine gas at 120.0°C and 26.1 bar would occupy a vessel of 38.0 L? R = 0.08314 L･bar/mol･K.

Answer 1

To calculate the number of moles of chlorine gas at a given temperature and pressure and for a given volume, we can use the ideal gas law equation.

Step-by-step explanation:

To calculate the number of moles of chlorine gas, we can use the ideal gas law equation:

PV = nRT

Where P is the pressure in bar, V is the volume in liters, n is the number of moles, R is the ideal gas constant, and T is the temperature in Kelvin.

Rearranging the equation to solve for n, we have:

n = PV / RT

Plugging in the given values (P = 26.1 bar, V = 38.0 L, T = 120.0°C which is 393.15 K, and R = 0.08314 L•bar/mol•K),

n = (26.1 bar) * (38.0 L) / (0.08314 L•bar/mol•K * 393.15 K)

Solving this equation gives us the number of moles of chlorine gas:

n = 12.302 mol

Answer 2

n = 30.36 mol

Step-by-step explanation:

Given data:

Temperature of gas = 120.0°C

Pressure of gas = 26.1 bar

Volume of gas = 38.0 L

Number of moles of Cl gas = ?

Solution:

Formula:

PV = nRT

P= Pressure

V = volume

n = number of moles

R = general gas constant = 0.08314 bar.L/ mol.K

T = temperature in kelvin

Now we will convert the temperature.

120+273 = 393 K

26.1 bar ×38.0 L = n × 0.08314 bar.L/ mol.K × 393 K

991.8 bar.L = n × 32.67bar.L/ mol

n = 991.8 bar.L/ 32.67bar.L/ mol

n = 30.36 mol