How Much Copper Dissolved When A 50.00 G Copper Plate Was Placed In A Mercury(II) Chloride Solution And Its Mass Increased To 52.74 G?

Introduction: Exploring the Chemistry of Copper and Mercury Chloride

In this comprehensive article, we delve into the fascinating chemical reaction between a copper plate and a mercury(II) chloride solution. Our primary focus is to meticulously analyze a scenario where a 50.00 g copper plate is immersed in a solution of mercury(II) chloride, leading to an increase in the plate's mass to 52.74 g after the reaction. The central question we aim to address is: how much copper dissolved during this process? To unravel this chemical puzzle, we will embark on a detailed exploration of the underlying principles, reaction mechanisms, and stoichiometric calculations. By meticulously examining the experimental setup and the observed mass change, we will accurately determine the mass of copper that transitioned into the solution. This investigation not only provides a quantitative answer but also offers valuable insights into the reactivity of metals and the nature of displacement reactions in chemistry.

To fully grasp the intricacies of this reaction, it's essential to first understand the fundamental properties of the reactants involved. Copper, a reddish-brown metal renowned for its excellent electrical conductivity and malleability, readily participates in redox reactions. On the other hand, mercury(II) chloride, also known as mercuric chloride, is a highly toxic compound with a strong oxidizing nature. When these two substances come into contact, a chemical reaction ensues, characterized by the transfer of electrons and the formation of new products. The reaction's outcome is influenced by several factors, including the concentration of the mercury(II) chloride solution, temperature, and the duration of the reaction. In our specific scenario, the observed increase in the copper plate's mass suggests that mercury ions from the solution are being deposited onto the copper surface, while copper atoms are simultaneously dissolving into the solution. This interplay of dissolution and deposition is the key to deciphering the quantitative aspects of the reaction.

The analysis of this reaction is not merely an academic exercise; it holds significant relevance in various fields of chemistry and materials science. Understanding the reactivity of metals in different chemical environments is crucial in designing corrosion-resistant materials, developing efficient electrochemical processes, and controlling metal-ion contamination in industrial settings. The reaction between copper and mercury(II) chloride, in particular, serves as a model system for studying metal displacement reactions, where a more reactive metal displaces a less reactive metal from its salt solution. By gaining a deeper understanding of these reactions, we can better predict and control the behavior of metals in complex chemical systems. Furthermore, this study highlights the importance of accurate measurements and stoichiometric calculations in chemical analysis. The precise determination of the mass change in the copper plate allows us to quantitatively assess the extent of the reaction and to verify the principles of mass conservation. In the following sections, we will delve into the step-by-step calculations and reasoning that lead to the solution of this problem, providing a clear and comprehensive understanding of the underlying chemistry.

Delving into the Chemical Equation: The Heart of the Reaction

The cornerstone of understanding any chemical reaction lies in its balanced chemical equation. For the reaction between copper and mercury(II) chloride, the equation provides a symbolic representation of the transformation occurring at the atomic and molecular level. The balanced chemical equation not only identifies the reactants and products but also specifies the stoichiometric ratios in which they interact. In our specific case, the balanced chemical equation is:

Cu(s) + HgCl2(aq) → CuCl2(aq) + Hg(s)

This equation reveals that one mole of solid copper (Cu) reacts with one mole of mercury(II) chloride (HgCl2) in aqueous solution to produce one mole of copper(II) chloride (CuCl2) in aqueous solution and one mole of solid mercury (Hg). The states of matter are indicated in parentheses: (s) for solid and (aq) for aqueous solution. This equation is a succinct yet powerful statement about the reaction, encapsulating the essence of the chemical transformation. However, to truly understand the equation's implications, we must delve deeper into the concepts of stoichiometry and molar masses.

Stoichiometry is the branch of chemistry that deals with the quantitative relationships between reactants and products in chemical reactions. It provides the tools to calculate the amounts of substances involved in a reaction, based on the balanced chemical equation. The coefficients in the balanced equation represent the molar ratios of the reactants and products. In our equation, the coefficients are all 1, indicating a 1:1:1:1 molar ratio. This means that for every one mole of copper that reacts, one mole of mercury(II) chloride is consumed, one mole of copper(II) chloride is formed, and one mole of mercury is produced. To translate these molar ratios into mass relationships, we need to consider the molar masses of the substances involved.

The molar mass of a substance is the mass of one mole of that substance, typically expressed in grams per mole (g/mol). The molar masses of copper and mercury are crucial for our calculations. The molar mass of copper (Cu) is approximately 63.55 g/mol, while the molar mass of mercury (Hg) is approximately 200.59 g/mol. These values serve as conversion factors between moles and grams, allowing us to relate the mass change observed in the experiment to the amount of copper that reacted and the amount of mercury that was deposited. By combining the balanced chemical equation, the stoichiometric ratios, and the molar masses, we can establish a quantitative framework for analyzing the reaction between copper and mercury(II) chloride. This framework will enable us to calculate the mass of copper that dissolved, which is the ultimate goal of our investigation. In the subsequent sections, we will apply these principles to the experimental data provided, meticulously tracing the steps required to arrive at the solution.

Stoichiometric Calculations: Unraveling the Copper Dissolution

Now, let's embark on the core of our analysis: the stoichiometric calculations that will reveal the mass of copper dissolved in the reaction. We begin with the fundamental observation that the mass of the copper plate increased after the reaction. This increase in mass is due to the deposition of mercury onto the copper surface, as mercury ions from the solution are reduced to solid mercury. The key to determining the amount of copper dissolved lies in recognizing that this process is directly linked to the amount of mercury deposited, according to the balanced chemical equation.

The mass increase of the copper plate is calculated as the difference between the final mass and the initial mass: 52.74 g - 50.00 g = 2.74 g. This 2.74 g represents the mass of mercury that was deposited onto the copper plate. Our next step is to convert this mass of mercury into moles, using the molar mass of mercury (200.59 g/mol). The number of moles of mercury deposited is calculated as follows:

Moles of Hg = Mass of Hg / Molar mass of Hg = 2.74 g / 200.59 g/mol ≈ 0.01366 mol

This calculation tells us that approximately 0.01366 moles of mercury were deposited during the reaction. Now, we turn to the balanced chemical equation, which states that one mole of copper dissolves for every one mole of mercury deposited. This 1:1 stoichiometric ratio is crucial, as it directly links the amount of mercury deposited to the amount of copper dissolved. Therefore, the number of moles of copper that dissolved is equal to the number of moles of mercury deposited, which is approximately 0.01366 mol.

To determine the mass of copper that dissolved, we multiply the number of moles of copper by its molar mass (63.55 g/mol):

Mass of Cu = Moles of Cu × Molar mass of Cu = 0.01366 mol × 63.55 g/mol ≈ 0.868 g

This calculation reveals that approximately 0.868 grams of copper dissolved during the reaction. However, there is a subtle but important point to consider. The initial mass increase of 2.74 g was due to the deposition of mercury. For every mole of mercury deposited, one mole of copper goes into the solution. This means that the increase in mass is the difference in the molar masses, therefore the difference in mass is (200.59 - 63.55) g per mole of reaction. Therefore, for each mole of reaction, the copper plate increases in mass by 137.04 g. Therefore, if the mass increases by 2.74 g, it involves 2.74/137.04 = 0.02 moles of the reaction. The amount of copper dissolved is 0.02 * 63.55 = 1.271 g. Rounding it, we get 1.27 g.

This result aligns closely with the answer provided (1.28 g), confirming the accuracy of our approach. The small discrepancy may be attributed to rounding errors or minor experimental variations. By meticulously applying stoichiometric principles and performing the necessary calculations, we have successfully determined the mass of copper that dissolved in the reaction with mercury(II) chloride. This analysis not only provides a quantitative answer but also underscores the power of stoichiometry in unraveling the intricacies of chemical reactions. In the following section, we will summarize our findings and highlight the key takeaways from this investigation.

Conclusion: Summarizing the Copper Dissolution Analysis

In this comprehensive analysis, we have successfully determined the mass of copper that dissolved when a 50.00 g copper plate was immersed in a mercury(II) chloride solution, resulting in a final plate mass of 52.74 g. Through a meticulous step-by-step approach, we have demonstrated the power of stoichiometric calculations in unraveling the quantitative aspects of chemical reactions. Our journey began with a thorough understanding of the reaction's context, including the properties of copper and mercury(II) chloride and the nature of metal displacement reactions. We then formulated the balanced chemical equation, which served as the foundation for our analysis:

Cu(s) + HgCl2(aq) → CuCl2(aq) + Hg(s)

This equation highlighted the 1:1 molar ratio between copper dissolved and mercury deposited, a crucial piece of information for our calculations. We then delved into the stoichiometric calculations, starting with the determination of the mass increase in the copper plate (2.74 g), which was attributed to the deposition of mercury. By converting this mass increase into moles of mercury using the molar mass of mercury (200.59 g/mol), we found that approximately 0.01366 moles of mercury were deposited. Applying the 1:1 stoichiometric ratio from the balanced equation, we concluded that the same number of moles of copper dissolved. Multiplying the moles of copper by its molar mass (63.55 g/mol), we initially calculated that approximately 0.868 g of copper dissolved. After considering the mass difference between mercury deposited and copper dissolved, we arrived at a more refined result of approximately 1.27 g of copper dissolved, which closely matches the provided answer of 1.28 g.

This investigation underscores the importance of understanding fundamental chemical principles, such as stoichiometry and molar masses, in solving quantitative problems. The ability to translate experimental observations, such as mass changes, into moles and then relate them through balanced chemical equations is a cornerstone of chemical analysis. Furthermore, this study highlights the significance of metal displacement reactions, which have numerous applications in various fields, including materials science, electrochemistry, and environmental chemistry. By understanding the factors that govern these reactions, we can design more efficient processes and develop novel materials with tailored properties.

In conclusion, our analysis has successfully elucidated the amount of copper that dissolved in the reaction with mercury(II) chloride. The meticulous application of stoichiometric principles, combined with a thorough understanding of the underlying chemistry, has allowed us to arrive at a quantitative answer and gain valuable insights into the nature of metal reactions. This investigation serves as a testament to the power of chemistry in unraveling the complexities of the world around us.