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Chapter 10: Problem 77

Write the balanced chemical equation for the following reactions: (a) Solid potassium chlorate decomposes to yield solid potassium chloride and oxygen gas. (b) Potassium metal reacts with water with the evolution of hydrogen gas. (c) Excess hydrogen gas is injected into a flask containing a small amount of liquid bromine. Upon heating, the bromine liquid disappears and a colorless gas is formed.

Short Answer

Expert verified
(a) 2KClO鈧� (s) 鈫� 2KCl (s) + 3O鈧� (g) (b) 2K (s) + 2H鈧侽 (l) 鈫� 2KOH (aq) + H鈧� (g) (c) H鈧� (g) + Br鈧� (l) 鈫� 2HBr (g)

Step by step solution

01

Identify Reactants and Products

For each reaction, identify the reactants and products. (a) The reactant is solid potassium chlorate (KClO鈧�) and the products are solid potassium chloride (KCl) and oxygen gas (O鈧�). (b) The reactants are potassium metal (K) and water (H鈧侽), and the products are potassium hydroxide (KOH) and hydrogen gas (H鈧�). (c) The reactants are hydrogen gas (H鈧�) and liquid bromine (Br鈧�), and the product is hydrogen bromide gas (HBr).
02

Write Unbalanced Equations

Write the chemical equation for each reaction using the formulas of the identified reactants and products. (a) KClO鈧� (s) 鈫� KCl (s) + O鈧� (g) (b) K (s) + H鈧侽 (l) 鈫� KOH (aq) + H鈧� (g) (c) H鈧� (g) + Br鈧� (l) 鈫� HBr (g)
03

Balance the First Equation

Balance the reaction: KClO鈧� decomposes to yield KCl and O鈧�. Start by balancing the number of K and Cl atoms, then balance O atoms. (a) 2KClO鈧� (s) 鈫� 2KCl (s) + 3O鈧� (g)
04

Balance the Second Equation

Balance the reaction between potassium metal and water. Balance the K atoms first, then H, and finally O. (b) 2K (s) + 2H鈧侽 (l) 鈫� 2KOH (aq) + H鈧� (g)
05

Balance the Third Equation

Balance the reaction between hydrogen gas and bromine liquid. Start with smaller molecules and balance the hydrogen and bromine atoms. (c) H鈧� (g) + Br鈧� (l) 鈫� 2HBr (g)

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Balancing Chemical Equations
Balancing chemical equations is a crucial skill in chemistry. It involves ensuring that the number of atoms for each element is the same on both the reactant and product sides of an equation. In essence, it reflects the law of conservation of mass, which states that matter cannot be created or destroyed. Let's break down the process with examples:
  • Start by outlining the unbalanced chemical equation using the correct formulas for reactants and products.
  • Balance the equation by adjusting the coefficients in front of each substance, ensuring that you have the same number of each type of atom on both sides.
  • Check each element one by one. For example, in the decomposition of potassium chlorate ( KClO鈧� ightarrow KCl + O鈧� ), you start by balancing potassium (K) and chlorine (Cl) before oxygen ( O ).
  • Sometimes, it鈥檚 easier to balance more complex molecules, such as oxygen or hydrogen, last.
Once balanced, the equation becomes: 2KClO鈧� 鈫� 2KCl + 3O鈧�. Each component is adjusted to reflect an equal count of elements on either side, maintaining the chemical identity of the reaction.
Reaction Stoichiometry
Stoichiometry is the calculation of reactants and products in chemical reactions. It helps determine the proportions in which chemical species react. Here鈥檚 why it's important:
  • Stoichiometry allows chemists to predict the amounts of substances consumed and produced during a reaction.
  • It is based on the molar relationships derived from balanced chemical equations.
  • For instance, in the reaction involving potassium and water, 2K + 2H鈧侽 鈫� 2KOH + H鈧� , the coefficients (2:2:2:1) represent the ratio in which the molecules react and form products.
  • By knowing these ratios, it's possible to calculate the quantities of reactants needed or the products formed using the concept of moles, which applies Avogadro's number to calculate actual amounts of substances.
This foundational concept in chemistry ensures that experiments can be accurately planned and executed, maximizing the yield of desired chemicals while minimizing waste.
Chemical Reactions
Chemical reactions involve the transformation of reactants into products. They are often accompanied by energy changes and are influenced by factors like temperature and concentration. All reactions can generally be classified into several types:
  • Decomposition Reaction: This occurs when a single compound breaks down into two or more simpler substances, such as KClO鈧� 鈫� KCl + O鈧� .
  • Combination or Synthesis Reaction: Two or more simple substances combine to form a more complex compound. For example, hydrogen and bromine combine to form hydrogen bromide in H鈧� + Br鈧� 鈫� 2HBr .
  • Replacement Reaction: This involves a change in partners between compounds, seen in reactions with potassium and water where hydrogen is displaced.
Understanding these basic types of chemical reactions helps in predicting the results of other reactions and planning new experiments. They also help in identifying potential applications of the reactions, such as in industry or environmental applications. Learning how different reactions occur and under what conditions allows chemists to harness these processes effectively.

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Most popular questions from this chapter

Nitrogen forms oxyacids with formulas of \(\mathrm{HNO}_{2}\) and \(\mathrm{HNO}_{3}\), whereas phosphorous forms oxyacids with formulas of \(\mathrm{H}_{3} \mathrm{PO}_{3}\) and \(\mathrm{H}_{3} \mathrm{PO}_{4}\) and arsenic forms oxyacids with formulas of \(\mathrm{H}_{3} \mathrm{AsO}_{3}\) and \(\mathrm{H}_{3} \mathrm{AsO}_{4}\). Explain why nitrogen, which is in the same group as phosphorous and arsenic, does not form oxyacids analogous to those of the other two elements.

Write the balanced chemical equation for the following reactions: (a) When sulfuric acid is placed on chalk (calcium carbonate), the chalk bubbles, forming a gas. (b) When tin metal is placed in a solution of hydrochloric acid, bubbles form and the metal is slowly dissolved. (c) Magnesium ribbon burns in air with a bright blue flame, leaving behind a white powdery solid residue.

Write the formulas of the following common household chemicals: (a) sodium hypochlorite (the active ingredient bleach) (b) hydrogen peroxide (used medicinally in dilute solutions) (c) potassium hydroxide (found in some drain cleaners) (d) acetic acid (the active ingredient in vinegar)

An unknown aqueous solution may contain one or more of the following ions: \(\mathrm{NH}_{4}^{+}(a q), \mathrm{Pb}^{2+}(a q)\), \(\mathrm{Ca}^{2+}(a q)\), and \(\mathrm{Fe}^{3+}(a q) .\) Devise a procedure (it may help to make a flowchart) by which you determine with certainty which ion(s) are present in the solution.

Write the chemical formula for (a) sodium perchlorate (b) potassium permanganate (c) calcium sulfite (d) lithium cyanide
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