Questions on gay lussacs law of combining volume

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How can Gay-Lussac's law of combining volumes be used to deduce chemical formulas?

Short Answer

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Gay-Lussac's law states that volumes of gases involved in a chemical reaction exhibit a simple ratio, equal to the ratio of stoichiometric coefficients of the reactants and products in the balanced chemical equation. By using this property, the volumes of gaseous reactants and products can be represented as ratios which correspond to the stoichiometry of the chemical reaction. Various volumes of gases involved can provide the stoichiometric coefficients in the chemical equation, which can be used to deduce the chemical formulas of the reactants and products.

Step by step solution

01

Understand Gay-Lussac's Law

Gay-Lussac's law of combining volumes states that the ratio of volumes of gases in any chemical reaction is directly proportional to the ratio of stoichiometric coefficients in the balanced chemical equation, when temperature and pressure are held constant. To put it simply, it says that volumes o

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Gay Lussac’s Law of Combining Volumes

 

Gay Lussac’s Law of Combining Volumes states that when gases react, they do so in volumes which bear a simple ratio to one another, and to the volume of the product(s) formed if gaseous, provided the temperature and pressure remain constant.

The law explains experimental facts about how gaseous atoms combine. Example:

For the reactions:

(i) N2(g) + 3H2(g) → 2NH3(g)

   1 vol.    3 vols.    2 vols.

1 volume of nitrogen combines with 3 volumes of hydrogen to form 2 volumes of ammonia.

(ii) 2H2(g) + O2(g) → 2H2O(g)

     2 vols.   1 vol.     2 vols.

2 volumes of hydrogen combine with 1 volume of oxygen to form 2 volumes of steam.

(iii) Cl2(g) + H2(g) → 2HCl(g)

     1 vol.    1 vol.    2 vols.

1 volume of chlorine gas combines with 1 volume of hydrogen to form 2 volumes of hydrochloric acid.

Question: Consider the reaction: 2H2(g) + O2(g) → 2H

Gay-Lussac's Law
Problems #1 - 10

Ten Examples

KMT & Gas Laws Menu

Problem #1: A L sample of nitrogen inside a rigid, metal container at &#;C is placed inside an oven whose temperature is &#;C. The pressure inside the container at &#;C was at atm. What is the pressure of the nitrogen after its temperature is increased to &#;C?

Solution:

P1  P2
––– = –––
T1  T2

  x
––– = –––
 

Solution technique: cross-multiply and divide.

x = atm (to three sig figs)

Note: you will see set ups (especially in gas laws) that simply omit all the units in the solution. If you execute that on a homework problem or test, you may get a deduction. It's not laziness on the part of the person writing the noun, it's simply assuming the reader knows what the units are and how they cancel out to leave the final unit.

Many times, you (as the student) are not allowed that luxury.

Problem #2: Determine the pressure change when a continual v