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Chapter 1: Problem 5

State whether the following statements are true or false. Gay-Lussac's law of combining volumes is applicable to the reaction, \(2 \mathrm{C}+\mathrm{O}_{2} \rightarrow 2 \mathrm{CO}_{2}\)

Short Answer

Expert verified
Answer: Yes, the reaction follows Gay-Lussac's law of combining volumes as the volume ratios of the gaseous reactants and products are in a simple whole-number ratio.

Step by step solution

01

Write down the balanced equation

We are given the balanced equation for the reaction: \(2 \mathrm{C}+\mathrm{O}_{2} \rightarrow 2 \mathrm{CO}_{2}\). It shows the stoichiometric coefficients for each species present in the reaction.
02

Identify the gaseous components in the reaction

In the given reaction, the gaseous components are: - \(\mathrm{O}_{2}\): dioxygen gas - \(\mathrm{CO}_{2}\): carbon dioxide gas
03

Verify the ratio

According to the balanced equation, 1 mole of \(\mathrm{O}_{2}\) combines with 2 moles of carbon to form 2 moles of \(\mathrm{CO}_{2}\). The volume ratios of the gaseous components in this reaction are 1:2. Therefore, we can say that the reaction follows Gay-Lussac's law of combining volumes, as the volume ratios are in simple whole numbers.
04

Conclusion

The statement "Gay-Lussac's law of combining volumes is applicable to the reaction, \(2 \mathrm{C}+\mathrm{O}_{2} \rightarrow 2 \mathrm{CO}_{2}\)" is true because the volume ratios of the gaseous reactants and products are in a simple whole-number ratio.

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Most popular questions from this chapter

It is found that with an increase in temperature by \(40 \%\), the volume decreases by \(20 \%\) with change in pressure. Find the percentage change in pressure. (a) \(40 \%\) decrease (b) \(60 \%\) decrease (c) \(75 \%\) increase (d) \(80 \%\) increase

Fill in the blanks. The ratio of the gram atomic weight of nitrogen and oxygen is __

Fill in the blanks. The number of oxygen molecules required for the complete combustion of 5 moles of methane is

Select the correct alternative from the given choices. \(0.1225 \mathrm{~g}\) of potassium chlorate decomposes completely. Write the possible chemical equation and the amount of oxygen liberated. (a) \(4 \mathrm{KClO}_{3} \rightarrow 4 \mathrm{KCl}+6 \mathrm{O}_{2}, 0.048 \mathrm{~g}\) (b) \(4 \mathrm{KClO}_{3} \rightarrow 4 \mathrm{KCl}+5 \mathrm{O}_{2}, 0.48 \mathrm{~g}\) (c) \(2 \mathrm{KClO}_{3} \rightarrow 2 \mathrm{KCl}+3 \mathrm{O}_{2}, 0.048 \mathrm{~g}\) (d) \(2 \mathrm{KClO}_{3} \rightarrow 2 \mathrm{KCl}+3 \mathrm{O}_{2}, 0.48 \mathrm{~g}\)

Select the correct alternative from the given choices. The number of oxygen atoms present in 2 moles of a compound, which consists of a bivalent metal and a perchlorate ion is (a) \(4 \mathrm{~N}\) (b) \(6 \mathrm{~N}\) (c) \(8 \mathrm{~N}\) (d) \(16 \mathrm{~N}\)
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