Question

Balance each of the following equations that describe synthesis reactions. a. \(\mathrm{Ni}(s)+\mathrm{CO}(g) \rightarrow \mathrm{Ni}(\mathrm{CO})_{4}(g)\). b. \(\mathrm{Al}(s)+\mathrm{S}(s) \rightarrow \mathrm{Al}_{2} \mathrm{S}_{3}(s)\) c. \(\mathrm{Na}_{2} \mathrm{SO}_{3}(a q)+\mathrm{S}(s) \rightarrow \mathrm{Na}_{2} \mathrm{S}_{2} \mathrm{O}_{3}(a q)\) d. \(\operatorname{Fe}(s)+\operatorname{Br}_{2}(l) \rightarrow \operatorname{Fe} \mathrm{Br}_{3}(s)\) e. \(\mathrm{Na}(s)+\mathrm{O}_{2}(g) \rightarrow \mathrm{Na}_{2} \mathrm{O}_{2}(s)\)

Short answer

The balanced equations for each synthesis reaction are as follows: a. \(Ni(s) + 4CO(g) \rightarrow Ni(CO)_4(g)\) b. \(2Al(s) + 3S(s) \rightarrow Al_2S_3(s)\) c. \(2Na_2SO_3(aq) + S(s) \rightarrow Na_2S_2O_3(aq)\) d. \(2Fe(s) + 3Br_2(l) \rightarrow 2FeBr_3(s)\) e. \(4Na(s) + O_2(g) \rightarrow 2Na_2O_2(s)\)

Step-by-step solution

Identify the unbalanced elements

In the given equation \(Ni(s) + CO(g) \rightarrow Ni(CO)_4(g)\), we can see that the number of carbon monoxide (CO) molecules is not equal on both sides.

Balance the equation

To balance the equation, we add a coefficient of 4 in front of CO, as there are 4 CO molecules in Ni(CO)4: \[Ni(s) + 4CO(g) \rightarrow Ni(CO)_4(g)\] b. Aluminum and Sulfur Reaction

Identify the unbalanced elements

In the given equation \(Al(s) + S(s) \rightarrow Al_2S_3(s)\), we can see that the number of aluminum (Al) and sulfur (S) atoms is not equal on both sides.

Balance the equation

To balance the equation, we add coefficients of 2 in front of Al and 3 in front of S: \[2Al(s) + 3S(s) \rightarrow Al_2S_3(s)\] c. Sodium Sulfite and Sulfur Reaction

Identify the unbalanced elements

In the given equation \(Na_2SO_3(aq) + S(s) \rightarrow Na_2S_2O_3(aq)\), we can see that the number of sulfur (S) atoms is not equal on both sides.

Balance the equation

To balance the equation, we add a coefficient of 2 in front of Na2SO3 and Na2S2O3: \[2Na_2SO_3(aq) + S(s) \rightarrow Na_2S_2O_3(aq)\] d. Iron and Bromine Reaction

Identify the unbalanced elements

In the given equation \(Fe(s) + Br_2(l) \rightarrow FeBr_3(s)\), we can see that the number of bromine (Br) atoms is not equal on both sides.

Balance the equation

To balance the equation, we add a coefficient of 2 in front of Fe and FeBr3, and 3 in front of Br2: \[2Fe(s) + 3Br_2(l) \rightarrow 2FeBr_3(s)\] e. Sodium and Oxygen Reaction

Identify the unbalanced elements

In the given equation \(Na(s) + O_2(g) \rightarrow Na_2O_2(s)\), we can see that the number of sodium (Na) and oxygen (O) atoms is not equal on both sides.

Balance the equation

To balance the equation, we add a coefficient of 4 in front of Na, and 2 in front of O2 and Na2O2: \[4Na(s) + O_2(g) \rightarrow 2Na_2O_2(s)\]

Key concepts

Synthesis Reactions

Synthesis reactions are fascinating chemical processes where two or more simple substances combine to form a more complex compound. These reactions are fundamental in creating many important compounds. Think of a synthesis reaction as a simple building project where smaller bricks (reactants) come together to form a beautiful wall (product).

In chemical terms, a synthesis reaction typically follows the formula:

• \( A + B \rightarrow AB \)

This formula illustrates how elements or compounds combine, indicating the movement toward forming a single product.

In the given exercise, each chemical equation involves synthesis reactions, where elements like Nickel and Carbon Monoxide merge to form nickel tetracarbonyl \( Ni(CO)_4 \), and Aluminum and Sulfur join to form aluminum sulfide \( Al_2S_3 \).

Understanding synthesis reactions allows scientists to predict and create various compounds essential for industrial applications, including metals, polymers, and pharmaceuticals.

Stoichiometry

Stoichiometry is the mathematical heart of chemical reactions, revealing the quantitative relationships between reactants and products. It's like the recipe behind the meal in cooking; it ensures the right proportions of ingredients are used to achieve the desired dish, or in chemistry, the correct chemical compound.

In the context of the exercise, stoichiometry helps us balance the chemical equations by ensuring the same number of atoms for each element on both sides of the equation.

• For example, in the sodium and oxygen reaction: \(4Na(s) + O_2(g) \rightarrow 2Na_2O_2(s)\).
• The stoichiometric coefficients (4, 2) in front of \(Na\) and \(O_2\) ensure that the atoms are balanced.

Without stoichiometry, it would be challenging to balance equations, as there would be no guidance on the amounts of each reactant and product.

Conservation of Mass

The law of conservation of mass is a fundamental concept in chemistry, stating that mass is neither created nor destroyed in a chemical reaction. This means the mass of the reactants must equal the mass of the products, ensuring no atoms are lost or gained during the transformation.

Think of it as a closed box where no matter can enter or leave. Anything you start with inside the box stays there, no matter how it changes form.

• When balancing the equations, realizing the law of conservation aids in understanding that each element's total number on the reactant side must equal the total on the product side.
• For instance, for the equation \(2Fe(s) + 3Br_2(l) \rightarrow 2FeBr_3(s)\), each side has an equal number of iron and bromine atoms, complying with this law.

Observing this law in balanced equations assures us that each element is accounted for, ensuring accurate chemical representation.

Chemical Reactions

Chemical reactions are processes where substances, the reactants, transform into one or more new substances, the products. Each reaction involves the breaking and forming of bonds, leading to changes in the chemical identity of the substances involved.

These transformations are represented by chemical equations, which express the conservation of mass and charge. For students learning chemistry, understanding the basics of chemical reactions is crucial, as they're the foundation for all changes in matter.

• Chemical equations not only show the reactants and products but also the conditions under which the reactions occur, such as temperature and pressure, if specified.
• During the balancing process, recognizing the pattern of reactants converting into products helps predict the outcome of similar reactions

In the exercise, each chemical reaction showcases unique transformations, demonstrating how different reactants lead to specific products through synthesis reactions.