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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.

Respuesta :

Neetoo

Answer:

n = 30.36 mol

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

samueladesida43

The number of moles of chlorine gas at 120.0°C and 26.1 bar that would occupy a vessel of 38.0 L is 30.4moles.

HOW TO CALCULATE NUMBER OF MOLES:

  • The number of moles can be calculated by using the following formula:

  • PV = nRT

Where;

  1. P = pressure (Bar)
  2. T = temperature (K)
  3. V = volume (L)
  4. n = number of moles (mol)
  5. R = gas law constant (0.08314 L･bar/mol･K.)

  • According to this question, chlorine gas at 120.0°C and 26.1 bar would occupy a vessel of 38.0 L. The number of moles can be calculated as follows:

T = 120°C + 273 = 393K

26.1 × 38 = n × 0.08314 × 393

991.8 = 32.67n

n = 991.8 ÷ 32.67

n = 30.4moles

  • Therefore,the number of moles of chlorine gas at 120.0°C and 26.1 bar that would occupy a vessel of 38.0 L is 30.4moles.

Learn more at: https://brainly.com/question/13821925?referrer=searchResults

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