Question

Oxygen combines with two isotopes of carbon, \({ }^{12} \mathrm{C}\) and \({ }^{14} \mathrm{C}\), to form two samples of carbon dioxide. The data illustrates (1) Law of conservation of mass (2) Law of multiple proportions (3) Law of reciprocal proportions (4) None of these

Short answer

The law illustrated is the Law of Multiple Proportions.

Step-by-step solution

Understand the scenario

Oxygen combines with two isotopes of carbon (^{12}C and ^{14}C) to form carbon dioxide. Identifying which law is illustrated involves understanding these laws in chemistry.

Review the Law of Conservation of Mass

This law states that mass is neither created nor destroyed in a chemical reaction. The total mass of reactants equals the total mass of products.

Review the Law of Multiple Proportions

This law states that if two elements combine to form more than one compound, the masses of one element that combine with a fixed mass of the other element are in ratios of small whole numbers.

Review the Law of Reciprocal Proportions

This law states that if two elements, A and B, each combine separately with a third element C, the ratio of the masses in which they do so will be the same as the ratio in which they combine with each other.

Analyze the given data with respect to the laws

The data shows oxygen combining with two isotopes of carbon to form carbon dioxide. Since it involves the same elements, carbon and oxygen, forming different compounds (with ^{12}C and ^{14}C), check for fixed or multiple ratios of combination with oxygen.

Identify the applicable law

Since the two isotopes of carbon combine with oxygen to form carbon dioxide in potentially different ratios (small whole numbers), this illustrates the Law of Multiple Proportions.

Key concepts

isotopes

Isotopes are different forms of the same element that contain the same number of protons but different numbers of neutrons. This difference in neutron count results in isotopes having the same atomic number but different mass numbers. For example, Carbon has isotopes like ^{12}C and ^{14}C.

The significance of isotopes is crucial in various scientific fields:

• In chemistry, isotopes help in understanding the behaviors of elements during reactions.
• In medicine, radioactive isotopes are used in diagnostic tools and treatment procedures.
• Isotopes also play a vital role in archeological dating, such as Carbon-14 dating for estimating the age of fossils.

Understanding isotopes clarifies why elements can participate in different reactions or form compounds in varying proportions.

chemical reaction laws

Chemical reaction laws are fundamental principles that govern how substances interact and transform during chemical reactions. Some key laws include:

Law of Conservation of Mass:This law states that mass cannot be created or destroyed in a chemical reaction. In other words, the total mass of the reactants equals the total mass of the products.

Law of Multiple Proportions:This law applies when two elements combine to form more than one compound. It states that the masses of one element that combine with a fixed mass of the other element are in ratios of small whole numbers. For instance, carbon and oxygen can form CO and CO_2, where oxygen maintains a simple ratio with carbon.

Law of Definite Proportions:Also known as the Law of Constant Composition, this principle states that a chemical compound always contains exactly the same proportion of elements by mass.

Understanding these laws helps predict the outcome of chemical reactions and guides the synthesis of new compounds, ensuring reactions proceed as expected and efficiently.

carbon dioxide formation

Carbon dioxide formation occurs when carbon combines with oxygen during a chemical reaction.

For example, when carbon burns in the presence of sufficient oxygen, it forms carbon dioxide (CO_2): \[C + O_2 \rightarrow CO_2\]This reaction is crucial for several reasons:

• Carbon dioxide is a vital part of the carbon cycle, a key process for maintaining life on Earth.
• Plants use carbon dioxide during photosynthesis to produce oxygen, which is essential for most living organisms.
• It's also important for understanding global warming, as CO_2 is a significant greenhouse gas.

Additionally, when carbon combines in different ways, guided by the Law of Multiple Proportions, it can form other compounds such as CO (carbon monoxide). This highlights the versatility of carbon-oxygen combinations in forming diverse chemical substances.