Chapter 1: Problem 23
\(\mathrm{II}_{2} \mathrm{~S}\) contain \(5.88 \%\) hydrogen, \(\mathrm{I}_{2} \mathrm{O}\) contain \(11.11 \%\) hydrogen while \(\mathrm{SO}_{2}\) contains \(50 \%\) sulphur. The data illustrate the law of (1) Conservation of mass (2) Constant proportions (3) Multiple proportions (4) Reciprocal proportions
Short Answer
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The data illustrate the law of reciprocal proportions.
Step by step solution
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Key Concepts
These are the key concepts you need to understand to accurately answer the question.
conservation of mass
The law of conservation of mass states that mass is neither created nor destroyed in chemical reactions. For example, when you burn wood, the mass of the ashes and gases together equals the original mass of the wood and the oxygen used up. This principle ensures that chemical equations are balanced, meaning the mass and number of atoms of each element are the same before and after a reaction. This law is fundamental in chemistry and is a key idea to understand before moving on to more complex concepts.
When you perform a chemical reaction, write down the reactants and products. Ensure that the total mass and the number of atoms for each element are equal on both sides of the equation.
This foundational law applies to all types of chemical reactions, including synthesis, decomposition, and displacement reactions.
When you perform a chemical reaction, write down the reactants and products. Ensure that the total mass and the number of atoms for each element are equal on both sides of the equation.
This foundational law applies to all types of chemical reactions, including synthesis, decomposition, and displacement reactions.
constant proportions
The law of constant proportions, also known as the law of definite proportions, states that a chemical compound always contains the exact same proportion of elements by mass. This means that no matter where you obtain a pure chemical compound, it will always be composed of the same elements in the same ratio.
For instance, water (H₂O) always consists of hydrogen and oxygen in a 2:1 ratio by atoms, or roughly 11.11% hydrogen and 88.89% oxygen by mass.
This principle helps chemists predict the outcomes and compositions of compounds formed during reactions.
Understanding this law is crucial when analyzing chemical formulas and predicting how different elements will combine to form compounds.
For instance, water (H₂O) always consists of hydrogen and oxygen in a 2:1 ratio by atoms, or roughly 11.11% hydrogen and 88.89% oxygen by mass.
This principle helps chemists predict the outcomes and compositions of compounds formed during reactions.
Understanding this law is crucial when analyzing chemical formulas and predicting how different elements will combine to form compounds.
multiple proportions
The law of multiple proportions states that when two elements form more than one compound, the ratios of the masses of one element that combine with a fixed mass of the other element are ratios of small whole numbers.
An excellent example is the compounds carbon monoxide (CO) and carbon dioxide (CO₂). In CO, 12 grams of carbon combine with 16 grams of oxygen, while in CO₂, 12 grams of carbon combine with 32 grams of oxygen. Here, the ratio of the masses of oxygen that combine with 12 grams of carbon is 1:2.
This law supports the idea that elements combine in simple, whole-number ratios, underscoring the discrete nature of atomic particles.
It provides deeper insights into the way elements interact at the atomic level and helps in understanding the stoichiometry of chemical reactions.
An excellent example is the compounds carbon monoxide (CO) and carbon dioxide (CO₂). In CO, 12 grams of carbon combine with 16 grams of oxygen, while in CO₂, 12 grams of carbon combine with 32 grams of oxygen. Here, the ratio of the masses of oxygen that combine with 12 grams of carbon is 1:2.
This law supports the idea that elements combine in simple, whole-number ratios, underscoring the discrete nature of atomic particles.
It provides deeper insights into the way elements interact at the atomic level and helps in understanding the stoichiometry of chemical reactions.
reciprocal proportions
In chemistry, the law of reciprocal proportions states that the ratio by mass in which one element A combines with element B is the ratio in which element B combines with element C.
For example, if sulfur and oxygen react with fixed amounts of hydrogen to form compounds, the way sulfur and oxygen react with each other should reflect these fixed proportions. If hydrogen forms II₂S and I₂O, as well as another compound with sulfur, the ratio of the elements is consistent.
Imagine II₂S has 5.88% hydrogen and I₂O has 11.11% hydrogen. Comparing sulfur proportions in this mix demonstrates the importance of how elements combine according to reciprocal laws.
This concept is fundamental when predicting how different elements will combine and is crucial for understanding reactivity and formation of diverse chemical compounds.
