Question

What volume will be occupied by 33.0 grams of CO2 at 500 torr and 27 °C?

Answer 1

Answer:

V = 27.98 L

Explanation:

Given data:

Mass of CO₂ = 33.0 g

Pressure = 500 torr

Temperature = 27°C

Volume occupied = ?

Solution:

Number of moles of CO₂:

Number of moles = mass/molar mass

Number of moles = 33.0 g/ 44 g/mol

Number of moles = 0.75 mol

Volume of CO₂:

PV = nRT

R = general gas constant = 0.0821 atm.L/ mol.K  

Now we will convert the temperature.

27+273 = 300 K

Pressure = 500 /760 = 0.66 atm

By putting values,

0.66 atm×V = 0.75 mol × 0.0821 atm.L/ mol.K  × 300 K

V = 18.47 atm.L/0.66 atm

V = 27.98 L

Answer 2

The volume that will be occupied by 33.0 grams of CO2 at 500 torr and 27 °C is 28.11L.

IDEAL GAS LAW:

The volume of an ideal gas can be calculated using the ideal gas law equation as follows:

PV = nRT

Where;

• P = pressure (atm)
• V = volume (L)
• n = number of moles (mol)
• R = gas law constant (0.0821 Latm/molK)
• T = temperature (K)

According to this question;

• P = 500torr = 0.657atm
• V = ?
• n = 33/44 = 0.75mol
• T = 27°C = 27 + 273 = 300K

0.657 × V = 0.75 × 0.0821 × 300

0.657V = 18.4725

V = 18.4725 ÷ 0.657

V = 28.11L

Therefore, the volume that will be occupied by 33.0 grams of CO2 at 500 torr and 27 °C is 28.11L.

Learn more about ideal gas law at: https://brainly.com/question/4147359