Unit 5 Review - Stoichiometry

Front

In a chemical reaction, the mass of reactants is equal to the mass of products. What principle does this statement illustrate?

Back

Law of Conservation of Mass

Front

What is the theoretical yield in a chemical reaction?

Back

The maximum amount of product that could be obtained from a given amount of reactants.

Front

Given the reaction: 2 KClO3 → 2 KCl + 3 O2, how many moles of oxygen are produced from 6.7 moles of KClO3?

Back

10.1 mol of O2

Front

In the balanced reaction: 3 Mg + 1 Fe2O3 → 3 MgO + 2 Fe, what is the mole ratio of MgO to Fe?

Back

3 mol MgO / 2 mol Fe

Front

In the combustion reaction CH4 + 2 O2 → CO2 + 2 H2O, how many moles of carbon dioxide are produced from 110 g of CH4?

Back

6.85 mol of CO2

Front

What is stoichiometry?

Back

The calculation of reactants and products in chemical reactions.

Front

Define molar mass.

Back

The mass of one mole of a substance, usually expressed in grams per mole (g/mol).

Front

What is a mole ratio?

Back

A ratio that relates the amounts in moles of any two substances involved in a chemical reaction.

Front

What does the term 'actual yield' refer to in a chemical reaction?

Back

The amount of product actually obtained from a reaction.

Front

What is the difference between theoretical yield and actual yield?

Back

Theoretical yield is the maximum possible amount of product, while actual yield is the amount obtained in practice.