Gas Calculations Worksheets, Questions, and Revision

GCSEAQAChemistry Higher

Gas Calculations

One of the most interesting properties of gasses is the volume of space that they occupy. All gasses, no matter the substances, will occupy the same volume of space per mole at a given temperature and pressure. At $20degree text{C}$ and $1text{ atm (atmospheres)}$ of pressure, one mole of gas will occupy a volume $24text{ dm}^3$ . This will be true no matter what substance makes up the gas. This means that we can always calculate the moles of a gas (and therefore its mass) in a given volume provided we know it’s temperature and pressure.

Calculating Moles and Volumes

Calculation of the moles or volume of a gas is relatively simple. If we know one, we are able to find the other thought the following relationship:

$text{Volume of Gas at }20degree text{C}text{ and }1text{ atm}$ $=$ $24 times text{Moles of Gas Present}$

If we know the volume occupied by a gas at $20degree text{C}$ and $1text{ atm}$ of pressure we can calculate the number of moles present by rearranging this formula.

It is important to remember that this relationship will only hold for gasses at $20degreetext{C}$ and $1text{ atm}$ . At other temperatures or pressures, the volume occupied by one mole of gas will be different and so this different volume will need to be used in the above equation.

Chemistry Higher

Calculating Gas Volumes from Equations

One result of this property of gasses is that, if we have a balanced equation where one or more of the chemicals involved is a gas, we can work out the volume of space occupied by this gas at $20degreetext{C and }1text{ atm}$ . This because the balanced equation will tell us the ratios of moles of each chemical are present in the reaction.

Take the example of the reaction between hydrochloric acid $left(text{HCl}right)$ and sodium hydrogen carbonate $left(text{NaHCO}_3right)$ :

$text{HCl}_{text{ (aq)}}+text{NaHCO}_{3text{ (s)}} rarr text{NaCl}_{text{ (s)}}+text{H}_2text{O}_{text{ (l)}}+text{CO}_{2text{ (g)}}$

This equation tells us that the ratio of moles of $left(text{HCl}right)$ & $left(text{NaHCO}_3right)$ to $text{CO}_2$ is $1:1$ . As such, if we know the mass of either $left(text{HCl}right)$ or $left(text{NaHCO}_3right)$ , we can calculate the volume of $text{CO}_2$ evolved.

Chemistry Higher

Example 1: Calculating Volume

Calculate the volume occupied by $textcolor{#00bfa8}{2.3text{ moles}}$ of nitrogen gas at $20degreetext{C and }1text{ atm}$ :

[1 mark]

Volume of Nitrogen at $20degree text{C}$ and $1text{ atm}$ :

$= 24 times text{Moles of Nitrogen Present} = 24times textcolor{#00bfa8}{2.3} =textcolor{#008d65}{55.2text{ dm}^3}$

Chemistry Higher

Example 2: Calculating Moles

Calculate the moles of oxygen present in $textcolor{#00bfa8}{179text{ dm}^3}$ of gas at $20degreetext{C and }1text{ atm}$ :

[1 mark]

Volume of Oxygen at $20degree text{C}$ and $1text{ atm}$ :

$= 24 times text{Moles of Oxygen Present}$

$text{Moles of Oxygen} =$ $frac{text{Volume of Oxygen}}{24} , = frac{textcolor{#00bfa8}{179}}{24} , =textcolor{#008d65}{7.5text{ mol}}$

Chemistry Higher

Example 3: Calculating Volumes from Equations

Calculate the volume of $text{CO}_2$ released when $textcolor{#00bfa8}{8.35text{ g}}$ of $text{NaHCO}_3$ $(text{M}_r =textcolor{#f21cc2}{84})$ reacts with $text{HCl}$ at $20degreetext{C and }1text{ atm}$ :

[3 marks]

Step 1: calculate the moles of $text{NaHCO}_3$ that have reacted:

$text{Moles NaHCO}_3 = frac{text{Mass NaHCO}_3}{text{M}_r text{NaHCO}_3} , =frac{textcolor{#00bfa8}{8.35}}{textcolor{#f21cc2}{84}} , =textcolor{#008d65}{0.099text{ mol}}$

Step 2: calculate the moles of $text{CO}_2$ that are evolved from the balanced equation of the reaction:

$text{HCl}_{text{ (aq)}}+text{NaHCO}_{3text{ (s)}} rarr text{NaCl}_{text{ (s)}}+text{H}_2text{O}_{text{ (l)}}+text{CO}_{2text{ (g)}}$

$text{Ratio of Moles}=1:1$

$text{Moles of CO}_2=text{Moles of NaHCO}_3$

Step 3: calculate the volume occupied by $text{CO}_2$ at $1degreetext{C and }1text{ atm}$ :

Volume of $text{CO}_2$ at $20degree text{C}$ and $1text{ atm}$ :

$= 24 times text{Moles of CO}_2 , = 24times 0.099 , =textcolor{#008d65}{2.4text{ dm}^3}$

Chemistry Higher

Gas Calculations Worksheets, Questions, and Revision Example Questions

Question 1: Calculate the volume of gas occupied by $0.070text{ mol}$ of HCl Gas at $20degreetext{C and }1text{ atm}$ .

[1 mark]

Chemistry Higher

$begin{aligned}text{Volume of HCl at }20degree text{C}text{ and }1text{ atm} &= 24 times text{Moles of HCl Present} &=24 times 0.070 &=underline{1.68text{ dm}^3}end{aligned}$

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Question 2: Calculate the moles of air present in a room of volume $70text{ million cm}^3$ at $20degreetext{C and }1text{ atm}$ .

[2 marks]

Chemistry Higher

Firstly, convert the volume of the room into $text{ dm}^3$ :

$begin{aligned}text{Volume in dm}^3&=frac{text{Volume in cm}^3}{1000} &=frac{70000000}{1000} &=underline{70000text{ dm}^3}end{aligned}$

Second, calculate the moles of air present:

$begin{aligned}text{Moles of Air}&=frac{text{Volume of Room}}{24} &=frac{70000}{24} &=underline{2917text{ mol}}end{aligned}$

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Question 3: Calculate the volume of $text{CO}_2$ released when $4.67text{ g}$ of $text{NaHCO}_3$ $(text{M}_r =84)$ reacts with $text{HCl}$ at $20degreetext{C and } 1text{ atm}$ .

[3 marks]

Chemistry Higher

Calculation should be broken down into steps. One mark per correct step.

Balanced Equation:

$text{HCl}_{text{ (aq)}}+text{NaHCO}_{3text{ (s)}} rarr text{NaCl}_{text{ (s)}}+text{H}_2text{O}_{text{ (l)}}+text{CO}_{2text{ (g)}}$

Step 1: Calculate moles of $text{NaHCO}_3$ .

$begin{aligned}text{Moles NaHCO}_3 &= frac{text{Mass NaHCO}_3}{text{M}_r text{NaHCO}_3} &=frac{4.67}{84} &=underline{0.056text{ mol}}end{aligned}$

Step 2: Calculate Moles of $text{CO}_2$ .

$text{Ratio of Moles}=1:1$

$text{Moles of CO}_2=text{Moles of NaHCO}_3$

Step 3: Calculate the volume of $text{CO}_2$ $text{ at } 20degreetext{C and }1text{ atm}$ :

$begin{aligned}text{Volume of CO}_2text{ at }20degree text{C}text{ and }1text{ atm} &= 24 times text{Moles of CO}_2 & 24times 0.056 &=underline{1.34text{ dm}^3}end{aligned}$