Question

How many grams of CO2 gas would occupy 25.7 L of volume at a temperature of –22.2oC and a pressure of 997 mm Hg? (***Must convert moles into gram at the end of this problem)

Answer 1

72.028g

Step-by-step explanation:

Data obtained from the question. This includes:

Volume (V) = 25.7 L

Temperature (T) = –22.2°C

Pressure (P) = 997 mmHg

Mass of CO2 =..?

Mass of CO2 can be obtained as follow:

Step 1:

Conversion to appropriate unit:

It is important to express each variables in their appropriate units in order to obtain the desired result in the right unit.

For temperature:

We shall be converting from celsius to Kelvin. This is illustrated below:

Temperature (Kelvin) = temperature (celsius) + 263

temperature (celsius) = –22.2°C

Temperature (Kelvin) = –22.2°C + 263

Temperature (Kelvin) = 250.8K

For Pressure:

We shall be converting from mmHg to atm. This is illustrated below:

760mmHg = 1 atm

Therefore, 997 mmHg = 997/760 = 1.31 atm

Step 2:

Determination of the number of mole of CO2.

With the ideal gas equation, we can obtain the number of mole of CO2 as follow:

Volume (V) = 25.7 L

Temperature (T) = 250.8K

Pressure (P) = 1.31 atm

Gas constant (R) = 0.082atm.L/Kmol

Number of mole (n) =...?

PV = nRT

n = PV/RT

n = (1.31 x 25.7)/(0.082 x 250.8)

n = 1.637 mole

Step 3:

Converting 1.637 mole of CO2 to grams. This is illustrated below:

Number of mole of CO2 = 1.637 mole

Molar Mass of CO2 = 12 + (2x16) = 12 + 32 = 44g/mol

Mass of CO2 =...?

Mass = number of mole x molar Mass

Mass of CO2 = 1.637 x 44

Mass of CO2 = 72.028g.