Limiting Reactants and Molar Mass

This video tutorial covers the concept of limiting reactants in chemistry, explaining how to determine which reactant will run out first and how much product can be formed. It provides a practical example involving nitrogen and hydrogen to produce ammonia, demonstrating the step-by-step process of solving a limiting reactant problem. The tutorial emphasizes the importance of balancing chemical equations, using molar masses, and applying mole ratios. It concludes with tips for correctly identifying the limiting reactant and ensuring accurate calculations.

What are the two main objectives when solving a limiting reactant problem?

• Identify the limiting reactant and the excess reactant.

• Find the reaction time and the energy released.

• Determine the amount of reactants left and the temperature change.

• Calculate the amount of product formed and identify the limiting reactant.

Why is gram-to-gram conversion important in laboratory settings?

• It helps in measuring the temperature of reactions.

• It is essential for converting reactants to products in measurable quantities.

• It allows for the calculation of reaction speed.

• It is used to determine the color change in reactions.

What is the first step in solving a limiting reactant problem?

• Calculate the energy change.

• Identify the color of the reactants.

• Balance the chemical equation.

• Measure the temperature.

In the example problem, what is the molar mass of nitrogen used for conversion?

• 28.02 grams per mole

• 17.04 grams per mole

• 14.01 grams per mole

• 2.02 grams per mole

What is the mole ratio of nitrogen to ammonia in the balanced equation?

• 2:3

• 3:2

• 1:2

• 1:1

How many grams of ammonia are produced from 20 grams of nitrogen?

• 17.0 grams

• 20.0 grams

• 24.3 grams

• 11.2 grams

What is the molar mass of hydrogen used in the conversion process?

• 17.04 grams per mole

• 2.02 grams per mole

• 1.01 grams per mole

• 28.02 grams per mole

Which reactant is identified as the limiting reactant in the example?

• Oxygen

• Ammonia

• Hydrogen

• Nitrogen

What should you do to ensure clarity when presenting solutions to limiting reactant problems?

• Use different colors for each step.

• Box the correct answer.

• Write the answer in bold.

• Underline the reactants.

What is the final amount of ammonia produced according to the limiting reactant?

• 24.3 grams

• 11.2 grams

• 17.0 grams

• 20.0 grams