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Chapter 14: Problem 33

How can you convert between moles of a substance and grams of a substance?

Short Answer

Expert verified
Convert moles to grams by multiplying with molar mass; convert grams to moles by dividing by molar mass.

Step by step solution

01

Identify What You Have

Determine what information you have. Are you starting with moles or grams? Also, identify the molar mass of the substance involved in the conversion.
02

Use the Molar Mass Formula

Apply the following formula to convert from moles to grams: \[\text{Grams} = \text{Moles} \times \text{Molar Mass (g/mol)} \]This formula uses the molar mass to find the weight in grams for the given amount of moles.
03

Use the Inverse to Convert From Grams to Moles

To convert from grams back to moles, use the inverse of the molar mass formula:\[\text{Moles} = \frac{\text{Grams}}{\text{Molar Mass (g/mol)}}\]Divide the weight in grams by the molar mass to find the corresponding amount in moles.

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Key Concepts

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

Understanding Molar Mass
Molar mass is a fundamental concept in chemistry. It serves as a bridge between the microscopic world of atoms and molecules and the macroscopic world we observe. Essentially, molar mass is the mass of one mole of a substance, measured in grams per mole (g/mol).
  • Molecules are made up of atoms, and each type of atom has a unique atomic mass, measured in atomic mass units (amu).
  • To find the molar mass of a compound, sum up the atomic masses of all the atoms present in one molecule of the substance. For example, water (H鈧侽) has a molar mass calculated by adding twice the atomic mass of hydrogen (approximately 1 amu each) plus the atomic mass of oxygen (approximately 16 amu), resulting in a molar mass of about 18 g/mol.
The molar mass allows chemists to convert between the number of moles and mass of a substance, providing a tangible way to count and measure molecules.
Chemical Calculations Simplified
Chemical calculations often involve converting between different units of measurement to determine the amounts of substances involved in a reaction. One of the most common conversions is from moles to grams or grams to moles. This is where the molar mass comes into play.
  • For instance, if you are given a certain number of moles and need to find the mass, multiply the moles by the molar mass as described by the formula: \[ \text{Grams} = \text{Moles} \times \text{Molar Mass (g/mol)} \]
  • Conversely, to convert grams back to moles, divide the mass by the molar mass:\[ \text{Moles} = \frac{\text{Grams}}{\text{Molar Mass (g/mol)}} \]
This process is crucial for stoichiometric calculations when determining reactant or product quantities in chemical reactions.
Stoichiometry: Balancing the Equation
Stoichiometry is the quantitative relationship between reactants and products in a chemical reaction. It uses the principles of conservation of mass and proportional reasoning to predict the outcomes of chemical equations. Understanding the stoichiometry of a reaction is essential for predicting the amounts of each substance involved.
  • The balanced chemical equation of a reaction tells us the ratio in which reactants convert to products. For example, the combustion of propane (C鈧僅鈧�) can be represented by the equation: \[ \text{C}_{3}\text{H}_{8} + 5\text{O}_{2} \rightarrow 3\text{CO}_{2} + 4\text{H}_{2}\text{O} \]
  • This equation indicates that one mole of propane reacts with five moles of oxygen to produce three moles of carbon dioxide and four moles of water.
  • Using stoichiometry, you can calculate the mass of products yielded from given reactants by applying the molar mass and mole-to-mole relationships shown in the balanced equation.
These calculations allow chemists to scale reactions for practical applications, from creating new materials to designing efficient industrial processes.

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Most popular questions from this chapter

Find at least i ve products at home with labels that warn of toxicity. Give the name of each product, and answer these questions: a. How does each label advise you to avoid harmful exposure to the product? b. What does each label tell you to do if a dangerous exposure does occur? c. Using all of this information, what can you hypothesize about the chemical properties of each product? d. Look at the recommended treatment for dangerous exposure to each product. What chemical and physical processes do you think might be involved in the treatment?

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