Question

Which of the following statements is false for the reaction of hydrogen gas with oxygen gas to produce water? \((a, b,\) and \(c\) represent coefficients) $$a \mathrm{H}_{2}(g)+b \mathrm{O}_{2}(g) \rightarrow c \mathrm{H}_{2} \mathrm{O}(g)$$ a. The ratio of " \(a / c "\) must always equal one. b. The sum of \(a+b+c\) equals 5 when balanced using the lowest whole-number coefficients. c. Coefficient \(b\) can equal \(1 / 2\) because coefficients can be fractions. d. The number of atoms on the reactant side must equal the number of atoms on the product side. e. Subscripts can be changed to balance this equation, just as they

Short answer

The false statement for the reaction of hydrogen gas with oxygen gas to produce water is option 'e': Subscripts can be changed to balance this equation. In a chemical equation, subscripts represent the chemical formula of a molecule and can never be changed. We balance chemical equations by adjusting coefficients, but not subscripts.

Step-by-step solution

Balance the given equation

First, we need to balance the given equation: \(a \mathrm{H}_{2}(g) + b \mathrm{O}_{2}(g) \rightarrow c \mathrm{H}_{2} \mathrm{O}(g)\) Balanced equation: \(2 \mathrm{H}_{2}(g) + 1 \mathrm{O}_{2}(g) \rightarrow 2 \mathrm{H}_{2} \mathrm{O}(g)\) Here, a = 2, b = 1, and c = 2.

Verify the given statements

Now, we will check if the given statements are true or false based on the balanced equation. a. The ratio of " \(a / c "\) must always equal one. Since \(a = 2\) and \(c = 2\), the ratio a/c is equal to one. Therefore, this statement is true. b. The sum of \(a+b+c\) equals 5 when balanced using the lowest whole-number coefficients. Here, \(a + b + c = 2+ 1+ 2 = 5\). Therefore, this statement is true. c. Coefficient \(b\) can equal \(1 / 2\) because coefficients can be fractions. In this reaction, \(b = 1\), which is a whole number. Although coefficients can sometimes be represented as fractions, it's not the case in this particular reaction. So, this statement is true. d. The number of atoms on the reactant side must equal the number of atoms on the product side. For the balanced equation, the number of Hydrogen atoms on both sides is 4, and the number of Oxygen atoms on both sides is 2. These are equal on both sides. This statement is true. e. Subscripts can be changed to balance this equation, just as they In a chemical equation, subscripts represent the chemical formula of a molecule and can never be changed. We balance chemical equations by adjusting coefficients, but not subscripts. This statement is false. So, based on our analysis, option 'e' is the false statement for this reaction.

Key concepts

Reaction Stoichiometry

Reaction stoichiometry focuses on the quantitative relationships between reactants and products in a chemical reaction.
It involves using the balanced chemical equation to determine the proportions of each substance involved. When you balance an equation, you ensure that the quantities of each element are conserved.
For example, the reaction of hydrogen gas and oxygen gas to produce water can be balanced as: \[ 2 \mathrm{H}_{2}(g) + 1 \mathrm{O}_{2}(g) \rightarrow 2 \mathrm{H}_{2} \mathrm{O}(g) \] In this balanced equation, one molecule of \( \mathrm{O}_{2}(g) \) (oxygen) reacts with two molecules of \( \mathrm{H}_{2}(g) \) (hydrogen) to form two molecules of \( \mathrm{H}_{2} \mathrm{O}(g) \) (water).
This tells us that every two molecules of hydrogen needs exactly one molecule of oxygen to react completely to form water.
Understanding stoichiometry is essential for calculating how much of each reactant you need or how much product will be formed in a reaction. It serves as a guide to ensure the reaction can occur fully without any shortages.

Coefficients in Chemical Equations

Coefficients in chemical equations are the numbers in front of molecules or elements that indicate their relative amounts in the reaction.
They play a crucial role in balancing chemical equations, ensuring the same number of each type of atom on both sides. You adjust these coefficients to balance the equation.
Using coefficients, the equation \( 2 \mathrm{H}_{2}(g) + 1 \mathrm{O}_{2}(g) \rightarrow 2 \mathrm{H}_{2} \mathrm{O}(g) \) shows:

• "2" in front of \( \mathrm{H}_{2} \) indicates two molecules of hydrogen gas are used.
• "1" in front of \( \mathrm{O}_{2} \) indicates that one molecule of oxygen gas is used.
• "2" in front of \( \mathrm{H}_{2} \mathrm{O} \) indicates two water molecules are produced.

Coefficients are the tools that help you achieve balanced equations.
It's important to remember that coefficients can sometimes be fractions in intermediary steps, but they're typically converted to whole numbers in the final balanced equation.

Law of Conservation of Mass

The Law of Conservation of Mass is a fundamental concept in chemistry.
It states that mass is neither created nor destroyed in a chemical reaction. This means that the mass of the reactants equals the mass of the products.
In our water formation reaction example, the number of hydrogen and oxygen atoms in the reactants equals the number in the products.

• 4 hydrogen atoms are found both in the \( \mathrm{H}_{2} \) and in the \( \mathrm{H}_{2} \mathrm{O} \),
• and 2 oxygen atoms are found both in the \( \mathrm{O}_{2} \) and in the \( 2 \mathrm{H}_{2} \mathrm{O} \).

This balance of atoms is a direct reflection of the conservation of mass.Remember, when balancing equations, you should never alter subscripts (the tiny numbers that make up molecules) to balance a reaction.
Instead, adjust only the coefficients.Ensuring the number of each type of atom is the same on both sides maintains the mass balance required by this law.