Complete the statement by calculating the required gas volume under constant temperature a… — JAMB UTME

Complete the statement by calculating the required gas volume under constant temperature and pressure conditions.

Answer:According to Gay-Lussac's law of combining volumes, in the reaction

2CO_{(g)} + O_{2(g)} \rightarrow 2CO_{2(g)}

40\text{ cm}^3

of carbon(II) oxide gas requires exactly 【20】

\text{cm}^3

of oxygen gas for complete reaction.

Answer

According to Gay-Lussac's law of combining volumes, gases react in volumes that bear a simple whole-number ratio to one another at constant temperature and pressure. In the balanced equation

2CO_{(g)} + O_{2(g)} \rightarrow 2CO_{2(g)}

, the volume combining ratio of

CO

O_2

2:1

. Therefore,

40\text{ cm}^3

CO

requires

\frac{40\text{ cm}^3}{2} = 20\text{ cm}^3

O_2

for complete combustion.

Step-by-Step Solution

Determine the stoichiometric volume ratio from the balanced chemical equation.

2 volumes of

CO_{(g)}

react with 1 volume of

O_{2(g)}

By Gay-Lussac's law of combining volumes, the combining volumes of reacting gases at constant temperature and pressure are proportional to their stoichiometric coefficients.

Calculate the volume of oxygen needed to react with

40\text{ cm}^3

of carbon(II) oxide.

Volume of

O_{2(g)} = 40\text{ cm}^3 \times \frac{1}{2} = 20\text{ cm}^3

Since the ratio of

CO

O_2

2:1

, the required volume of

O_2

is half the volume of

CO

Key Concept

Gay-Lussac's Law of Combining Volumes

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