Textbook Question
A compound, KBrO𝑥, where x is unknown, is analyzed and found to contain 52.92% Br. What is the value of x?
2
views
Ch.3 - Chemical Reactions and Reaction Stoichiometry
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970
Not the one you use?Change textbookSelect a different textbook
Table of contents
- Ch.1 - Introduction: Matter, Energy, and Measurement111
- Ch.2 - Atoms, Molecules, and Ions166
- Ch.3 - Chemical Reactions and Reaction Stoichiometry138
- Ch.4 - Reactions in Aqueous Solution127
- Ch.5 - Thermochemistry104
- Ch.6 - Electronic Structure of Atoms109
- Ch.7 - Periodic Properties of the Elements107
- Ch.8 - Basic Concepts of Chemical Bonding102
- Ch.9 - Molecular Geometry and Bonding Theories120
- Ch.10 - Gases122
- Ch.11 - Liquids and Intermolecular Forces79
- Ch.12 - Solids and Modern Materials102
- Ch.13 - Properties of Solutions99
- Ch.14 - Chemical Kinetics153
- Ch.15 - Chemical Equilibrium83
- Ch.16 - Acid-Base Equilibria109
- Ch.17 - Additional Aspects of Aqueous Equilibria117
- Ch.18 - Chemistry of the Environment60
- Ch.19 - Chemical Thermodynamics109
- Ch.20 - Electrochemistry113
- Ch.21 - Nuclear Chemistry79
- Ch.22 - Chemistry of the Nonmetals52
- Ch.23 - Transition Metals and Coordination Chemistry57
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry7
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970Not the one you use?Change textbook
Chapter 3, Problem 99
The fat stored in a camel's hump is a source of both energy and water. Calculate the mass of H2O produced by the metabolism of 1.0 kg of fat, assuming the fat consists entirely of tristearin 1C57H110O62, a typical animal fat, and assuming that during metabolism, tristearin reacts with O2 to form only CO2 and H2O.
Verified step by step guidance1
Write the balanced chemical equation for the metabolism of tristearin (C_{57}H_{110}O_6) with oxygen (O_2) to form carbon dioxide (CO_2) and water (H_2O).
Determine the molar mass of tristearin (C_{57}H_{110}O_6) by adding the atomic masses of all the atoms in the formula.
Calculate the number of moles of tristearin in 1.0 kg (1000 g) by dividing the mass of tristearin by its molar mass.
Use the stoichiometry of the balanced equation to find the number of moles of water (H_2O) produced per mole of tristearin metabolized.
Convert the moles of water obtained to mass by multiplying by the molar mass of water (H_2O).
Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Stoichiometry
Stoichiometry is the calculation of reactants and products in chemical reactions. It involves using balanced chemical equations to determine the relationships between the amounts of substances consumed and produced. In this case, stoichiometry will help us find the mass of water produced from the metabolism of tristearin by relating the fat's molecular composition to the products formed.
Recommended video:
Guided course
01:16
Stoichiometry Concept
Combustion of Tristearin
The combustion of tristearin (C57H110O6) involves its reaction with oxygen (O2) to produce carbon dioxide (CO2) and water (H2O). This process is an example of a complete combustion reaction, where the fat is fully oxidized. Understanding the balanced equation for this reaction is crucial for calculating the amount of water produced from a given mass of fat.
Recommended video:
Guided course
02:24Combustion Apparatus
Molar Mass and Mass-to-Mole Conversions
Molar mass is the mass of one mole of a substance, expressed in grams per mole. To calculate the mass of water produced, we first need to convert the mass of tristearin into moles using its molar mass. Then, using the stoichiometric coefficients from the balanced equation, we can determine the moles of water produced and convert that back into grams for the final answer.
Recommended video:
Guided course
02:28Mass and Moles Conversion
Related Practice
Textbook Question
A method used by the U.S. Environmental Protection Agency (EPA) for determining the concentration of ozone in air is to pass the air sample through a 'bubbler' containing sodium iodide, which removes the ozone according to the following equation: O31g2 + 2 NaI1aq2 + H2O1l2¡ O21g2 + I21s2 + 2 NaOH1aq2 (b) How many grams of sodium iodide are needed to remove 1.3 mg of O3?
537
views
Textbook Question
A mixture of N21g2 and H21g2 reacts in a closed container to form ammonia, NH31g2. The reaction ceases before either reactant has been totally consumed. At this stage 3.0 mol N2, 3.0 mol H2, and 3.0 mol NH3 are present. How many moles of N2 and H2 were present originally?
978
views
Textbook Question
When a mixture of 10.0 g of acetylene (C2H2) and 10.0 g of oxygen (O2) is ignited, the resulting combustion reaction produces CO2 and H2O. (c) How many grams of C2H2 are present after the reaction is complete?
799
views
Textbook Question
An element X forms an iodide (XI3) and a chloride (XCl3). The iodide is quantitatively converted to the chloride when it is heated in a stream of chlorine: 2 XI3 + 3 Cl2 → 2 XCl3 + 3 I2 If 0.5000 g of XI3 is treated with chlorine, 0.2360 g of XCl3 is obtained. (a) Calculate the atomic weight of the element X. (b) Identify the element X.
992
views