Question

The sugar sucrose, which is present in many fruits and vegetables, reacts in the presence of certain yeast enzymes to produce ethanol and carbon dioxide gas. Balance the following equation for this reaction of sucrose. $$ \mathrm{C}_{12} \mathrm{H}_{22} \mathrm{O}_{11}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \rightarrow \mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}(a q)+\mathrm{CO}_{2}(g) $$

Short answer

The balanced chemical equation for the reaction of sucrose with water to produce ethanol and carbon dioxide is: \[ \mathrm{C}_{12} \mathrm{H}_{22} \mathrm{O}_{11}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \rightarrow 6\,\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}(a q) + 6\,\mathrm{CO}_{2}(g) \]

Step-by-step solution

List the elements present in the reaction

Elements: 1. Carbon (C) 2. Hydrogen (H) 3. Oxygen (O) Step 2: Count the number of atoms of each element on both sides of the equation

Tally atoms for each element on reactants and products

Reactants: C: 12 (in sucrose) H: 22 (in sucrose) + 2 (in water) = 24 O: 11 (in sucrose) + 1 (in water) = 12 Products: C: 2 (in ethanol) + 1 (in carbon dioxide) H: 6 (in ethanol) O: 1 (in ethanol) + 2 (in carbon dioxide) Step 3: Balance the atoms on both sides

Adjust coefficients to balance the equation

Start by balancing carbon atoms: C: 12 (reactants) = 2 (in ethanol) + 1 (in CO2) * coefficient_x We require 12 carbon atoms on the products side, thus we need to multiply ethanol by 6 and CO2 by 6, because 6*2 (in ethanol) + 6*1 (in CO2) = 12. Now the products side has: C: 2 * 6 (in ethanol) + 1 * 6 (in CO2) H: 6 * 6 (in ethanol) O: 1 * 6 (in ethanol) + 2 * 6 (in CO2) Next, balance the hydrogen atoms: H: 24 (reactants) = 6 * 6 (in ethanol) In this case, the hydrogen atoms are already balanced. Finally, balance the oxygen atoms: O: 12 (reactants) = 1 * 6 (in ethanol) + 2 * 6 (in CO2) Again, the oxygen atoms are also balanced. Step 4: Write the balanced equation

Write the balanced chemical equation

The balanced chemical equation for the reaction of sucrose with water to produce ethanol and carbon dioxide is: \[ \mathrm{C}_{12} \mathrm{H}_{22} \mathrm{O}_{11}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \rightarrow 6\,\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}(a q) + 6\,\mathrm{CO}_{2}(g) \]

Key concepts

Stoichiometry Demystified

Stoichiometry is the heart of chemistry, and it helps us understand the quantitative relationships in chemical reactions. Imagine you're baking a cake. You need the right amounts of ingredients in order to get the best result. In chemistry, stoichiometry works similarly by ensuring chemical equations are balanced with the same number of atoms for each element on both sides of a reaction. This process allows chemists to predict the amounts of reactants needed and products formed.

Here's what stoichiometry involves:

• Counting atoms: First, identify how many atoms of each element are in the reactants and products.
• Balancing equations: Adjust coefficients in the chemical equation to have equal numbers of each type of atom on both sides.
• Ratio interpretation: These coefficients allow us to understand the ratios in which substances react and form products.

By mastering stoichiometry, students gain insight into how different compounds interact, making it essential for fields like biochemistry and pharmacology. It's a skill that transforms abstract chemical equations into tangible insights about chemical behavior.

Understanding Reaction Products

When a chemical reaction occurs, it leads to the formation of one or more products. Products are substances generated from the reactants through the breaking and forming of chemical bonds.

In our equation, which describes the fermentation process of sucrose, the products are ethanol (\(\text{C}_2\text{H}_5\text{OH}\)) and carbon dioxide (\(\text{CO}_2\)). These are produced when sucrose and water react under the influence of yeast enzymes. This transformation follows the conservation of mass principle, meaning the total matter remains constant throughout the reaction.

Here are key elements when examining reaction products:

• Identification: Determine which new substances appear in a finished reaction.
• Yield: Consider how much product can be formed from given amounts of reactants.
• Properties: Understand the physical and chemical properties of the products formed.
• Applications: Products can be useful in various fields, e.g., ethanol is used as a fuel and in beverages.

Exploring reaction products in depth helps recognize the potential and limitations of chemical reactions, impacting industries like energy and medicine.

Exploring Chemical Reactions

Chemical reactions are processes where substances, called reactants, transform into different substances, called products. These changes involve making and breaking chemical bonds, leading to new arrangements of atoms. In our example, sucrose reacts with water facilitated by yeast, illustrating a fermentation reaction typical in food production.

Important aspects of chemical reactions include:

• Types of reactions: Common types include synthesis, decomposition, single and double replacement, and combustion.
• Energy changes: Reactions can release (exothermic) or absorb (endothermic) energy, affecting temperature and reaction favorability.
• Catalysts: Substances like enzymes that speed up reactions without being consumed.
• Kinetics: The rate at which reactions occur, influenced by factors such as temperature, concentration, and pressure.

Understanding chemical reactions is fundamental in explaining phenomena from digestion in biology to the mechanism of industrial processes, emphasizing the transformative power of chemistry.