
Calculate the volume occupied by \[8.8\] gram of \[CO_2\] at \[31.1\] degree Celsius and \[1\] bar pressure R= \[0.083\] by LK inverse mole inverse (molecular mass of \[CO_2 = 44\] gram mole inverse)
Answer
351k+ views
Hint: According to the ideal gas law, the product of volume and temperature is equal to the number of moles, universal gas constant, and temperature. The moles can be defined as the ratio of mass to molar mass. The mass of \[CO_2\] was already given whereas the molar mass of \[CO_2\] was also given.
Formula used:
\[PV = nRT\]
P is pressure
V is volume
n is number of moles
R is universal gas constant
T is temperature
Complete answer:
The ideal gas law is also known as the general gas equation. It relates the pressure, volume, temperature, number of moles, and universal gas constant.
Moles relate the ratio of the mass and molar mass. The given gas is carbon dioxide. It has a mass of \[8.8\] gram. The mass occupied by one mole of carbon dioxide is \[44\] atomic mass units, which is nothing but molar mass.
By substituting all the given values in the above formula,
\[V = \dfrac{{8.8 \times 0.083 \times 304.1}}{{44 \times 1}}\]
The volume V will be \[5.0486L\]
Thus, the volume occupied by \[8.8\] gram of \[CO_2\] at \[31.1\]degree Celsius and \[1\] bar pressure R= \[0.083\] by LK inverse mole inverse (molecular mass of \[CO_2 = 44\] gram mole inverse) will be \[5.0486L\]
Note:
While calculating any term or quantity related to ideal gas law, the units must be considered. As the pressure must be in atm, and the volume must be in Litres, the temperature must be in kelvins, and the number of moles in moles only.
Formula used:
\[PV = nRT\]
P is pressure
V is volume
n is number of moles
R is universal gas constant
T is temperature
Complete answer:
The ideal gas law is also known as the general gas equation. It relates the pressure, volume, temperature, number of moles, and universal gas constant.
Moles relate the ratio of the mass and molar mass. The given gas is carbon dioxide. It has a mass of \[8.8\] gram. The mass occupied by one mole of carbon dioxide is \[44\] atomic mass units, which is nothing but molar mass.
By substituting all the given values in the above formula,
\[V = \dfrac{{8.8 \times 0.083 \times 304.1}}{{44 \times 1}}\]
The volume V will be \[5.0486L\]
Thus, the volume occupied by \[8.8\] gram of \[CO_2\] at \[31.1\]degree Celsius and \[1\] bar pressure R= \[0.083\] by LK inverse mole inverse (molecular mass of \[CO_2 = 44\] gram mole inverse) will be \[5.0486L\]
Note:
While calculating any term or quantity related to ideal gas law, the units must be considered. As the pressure must be in atm, and the volume must be in Litres, the temperature must be in kelvins, and the number of moles in moles only.
Recently Updated Pages
Master Class 11 Accountancy: Engaging Questions & Answers for Success

Glucose when reduced with HI and red Phosphorus gives class 11 chemistry CBSE

The highest possible oxidation states of Uranium and class 11 chemistry CBSE

Find the value of x if the mode of the following data class 11 maths CBSE

Which of the following can be used in the Friedel Crafts class 11 chemistry CBSE

A sphere of mass 40 kg is attracted by a second sphere class 11 physics CBSE

Trending doubts
10 examples of friction in our daily life

Difference Between Prokaryotic Cells and Eukaryotic Cells

State and prove Bernoullis theorem class 11 physics CBSE

What organs are located on the left side of your body class 11 biology CBSE

Define least count of vernier callipers How do you class 11 physics CBSE

The combining capacity of an element is known as i class 11 chemistry CBSE
