Question

One mole of fluorine is reacted with two mole of hot and concentrated \(\mathrm{KOH}\). The products formed are \(\mathrm{KF}, \mathrm{H}_{2} \mathrm{O}\) and \(\mathrm{O}_{2}\). The molar ratio of \(\mathrm{KF}, \mathrm{H}_{2} \mathrm{O}\) and \(\mathrm{O}_{2}\) respectively is: (a) \(1: 2: 1\) (b) \(1: 2: 2\) (c) \(0.5: 1: 2\) (d) \(2: 1: 0.5\)

Short answer

The molar ratio of \(\mathrm{KF}, \mathrm{H}_2\mathrm{O}, \mathrm{O}_2\) is \(2 : 1 : 0.5\) (option d).

Step-by-step solution

Write the Balanced Chemical Equation

The balanced chemical equation for the reaction of fluorine with potassium hydroxide is:\[\mathrm{2F}_2 + 4\mathrm{KOH} \rightarrow 4\mathrm{KF} + 2\mathrm{H}_2\mathrm{O} + \mathrm{O}_2\]

Determine Moles of Reactants

One mole of fluorine \(\mathrm{(F_2)}\) is used in the reaction with two moles of hot and concentrated \(\mathrm{KOH}\). Since 2 moles of \(\mathrm{F_2}\) react with 4 moles of \(\mathrm{KOH}\), using just 1 mole of \(\mathrm{F_2}\) will require 2 moles of \(\mathrm{KOH}\), which matches the given conditions.

Calculate Moles of Each Product

From the equation, every 2 moles of \(\mathrm{F_2}\) used forms 4 moles of \(\mathrm{KF}\), 2 moles of \(\mathrm{H}_2\mathrm{O}\), and 1 mole of \(\mathrm{O}_2\). When only 1 mole of \(\mathrm{F_2}\) is used, the product formation will be half, resulting in 2 moles of \(\mathrm{KF}\), 1 mole of \(\mathrm{H}_2\mathrm{O}\), and 0.5 mole of \(\mathrm{O}_2\).

Determine Molar Ratio of Products

Referencing Step 3, when 1 mole of \(\mathrm{F_2}\) is used, the molar ratio of products \(\mathrm{KF} : \mathrm{H}_2\mathrm{O} : \mathrm{O}_2\) is \(2 : 1 : 0.5\).

Key concepts

Balanced Chemical Equation

A balanced chemical equation is fundamental in chemistry because it represents a chemical reaction where the number of atoms for each element is the same on both sides of the reaction. This balance is crucial because it reflects the law of conservation of mass, which states that mass is neither created nor destroyed in a chemical reaction. In the exercise, the equation \(2\mathrm{F}_2 + 4\mathrm{KOH} \rightarrow 4\mathrm{KF} + 2\mathrm{H}_2\mathrm{O} + \mathrm{O}_2\) is perfectly balanced. Each element's atom count matches on both sides: fluorine (F), potassium (K), hydrogen (H), and oxygen (O). Think of balancing equations like making sure there are equal parts on both sides of a scale. It's essential for accurate calculations and predicting the outcome of reactions.

• Identify each atom in the equation.
• Ensure every atom's count is equal on both reactant and product sides.
• Use additional coefficients to balance if needed.

Stoichiometry

Stoichiometry is the area of chemistry that focuses on the quantitative analysis of a chemical reaction. It involves calculating the amounts of reactants and products in a chemical equation, based on their proportions in the balanced equation. This is essential because it helps chemists to scale reactions, determine yields, and optimize the use of resources. In our case, stoichiometry allows the determination that 1 mole of \(\mathrm{F}_2\) requires 2 moles of \(\mathrm{KOH}\) to produce specific amounts of \(\mathrm{KF}, \mathrm{H}_2\mathrm{O},\) and \(\mathrm{O}_2\). By looking at the balanced equation, you can understand and calculate the precise yield of products given any amount of reactants.

• Use the balanced equation coefficients to find mole ratios.
• Convert between moles and grams, if necessary, using molar mass.
• Predict product quantities from given reactant amounts.

Molar Ratios

Molar ratios are derived from the coefficients of a balanced chemical equation and express the relative amounts of moles of each reactant and product involved in the reaction. These ratios are crucial for calculating how much of a product you can expect to get from certain reactant quantities or to determine the amount of reactants needed for a desired amount of product. In the problem exercise, the molar ratios tell us that with 1 mole of \(\mathrm{F}_2\), you will form 2 moles of \(\mathrm{KF}\), 1 mole of \(\mathrm{H}_2\mathrm{O}\), and 0.5 mole of \(\mathrm{O}_2\).

• Derived directly from the balanced chemical equation.
• Critical for converting between moles of different substances.
• Helps in experimental preparation and ensuring efficiency.

Inorganic Chemistry

Inorganic chemistry is the branch of chemistry that deals with inorganic compounds, typically not covered by organic chemistry. This area involves substances that do not have carbon-hydrogen bonds, including metals, minerals, and organometallics. The reaction studied involves inorganic compounds: fluorine (\(\mathrm{F}_2\)), potassium hydroxide (\(\mathrm{KOH}\)), and the products of their reaction (\(\mathrm{KF}\), \(\mathrm{H}_2\mathrm{O}\), and \(\mathrm{O}_2\)). Understanding inorganic chemical reactions, like the one in the exercise, allows chemists to perform practical applications in fields such as material science, medicine, and environmental chemistry.

• Focuses on compounds typically without carbon-hydrogen bonds.
• Includes synthesis and behavior of inorganic and organometallic compounds.
• Involves complex reactions and processes applied across various industries.