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Chapter 11: Problem 54

What is the first step in all stoichiometric calculations?

Short Answer

Expert verified
The first step in all stoichiometric calculations is to write a balanced chemical equation for the reaction of interest. This ensures that the number of atoms of each element in the reactants equals the number of atoms of each element in the products, adhering to the law of conservation of mass. A balanced chemical equation provides the necessary mole ratios for stoichiometric calculations.

Step by step solution

01

Write a Balanced Chemical Equation

To begin any stoichiometric calculation, it's crucial to have a balanced chemical equation for the reaction of interest. A balanced chemical equation means that the number of atoms of each element in the reactants is equal to the number of atoms of each element in the products. This is due to the fact that matter cannot be created or destroyed during a chemical reaction (law of conservation of mass). Remember that stoichiometric calculations are based on the mole ratios of reactants and products within a chemical reaction, making it essential to have a balanced chemical equation.

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Key Concepts

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

Balanced Chemical Equation
A balanced chemical equation is fundamental to understanding and performing stoichiometry in chemistry. It represents a chemical reaction in which the number of atoms of each element is the same on both sides of the equation. This balance reflects how molecules interact in a real reaction.

To create a balanced chemical equation, follow these steps:
  • Write the unbalanced equation, showing all reactants turning into products.
  • Count the number of atoms for each element on both sides of the equation.
  • Add coefficients to adjust and ensure that each side has the same number of atoms for every element. Coefficients are numerical multipliers placed in front of compounds or elements.
Balancing an equation is necessary because it provides the correct proportions of reactants and products needed for precise measurements and predictions in stoichiometry. Without this balance, calculations would be inaccurate.
Law of Conservation of Mass
The Law of Conservation of Mass is a cornerstone of chemistry and physics. It tells us that mass is conserved in an isolated system during any chemical or physical change. In simple terms, this means that mass cannot be created or destroyed.

In the context of a chemical reaction, this law implies:
  • The total mass of the reactants equals the total mass of the products.
  • The mass of elements remains constant before and after a reaction.
Understanding this law helps chemists ensure that their equations reflect reality. For example, if 10 grams of reactants result in 10 grams of products, this confirms the law is upheld. This principle must guide every step of stoichiometric calculations, from writing balanced equations to measuring quantities.
Mole Ratios
Mole ratios are the bridge between the quantities in a balanced chemical equation and the calculations in stoichiometry. They come from the coefficients of each compound or element in the equation.

The importance of mole ratios includes:
  • Offering a way to convert between moles of different substances.
  • Enabling calculations of amounts needed or produced in a reaction.
  • Guiding the scaling of reactions up or down, depending on required quantities.
For instance, in the balanced equation \( aA + bB \rightarrow cC + dD \), mole ratios might be \( a:b:c:d \). If you know how many moles of \( A \) you've started with, you can calculate the moles of \( B, C, \) or \( D \) using these ratios. This concept makes stoichiometry a predictive and practical tool in chemistry.

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Most popular questions from this chapter

Chlorine forms from the reaction of hydrochloric acid with manganese(IV) oxide. The balanced equation is: $$\mathrm{MnO}_{2}+4 \mathrm{HCl} \rightarrow \mathrm{MnCl}_{2}+\mathrm{Cl}_{2}+2 \mathrm{H}_{2} \mathrm{O}$$ Calculate the theoretical yield and the percent yield of chlorine if 86.0 \(\mathrm{g}\) of \(\mathrm{MnO}_{2}\) and 50.0 \(\mathrm{g}\) of HCl react. The actual yield of \(\mathrm{Cl}_{2}\) is 20.0 \(\mathrm{g}\)

Describe how a mole ratio is correctly expressed when it is used to solve a stoichiometric problem.

Apply When a campfire begins to die down and smolder, you can rekindle the flame by fanning the fire. Explain, in terms of stoichiometry, why the fire again begins to flare up when fanned.

Explain how percent yield is calculated.

Why are coefficients used in mole ratios instead of subscripts?
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