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Numbers and Scientific Notation
- Created by Mitchell Foltz , last modified by Leta R Moser on May 13, 2021
At any point you can email [email protected] with questions or concerns regarding technical difficulties using the system.
Some questions you may encounter in Quest will use numeric free response answers that you type in. The following example is a numeric type question on a learning module slide, but these questions can appear on all types of Quest assignments.
- If your instructor has allowed retries, you will be given 7 attempts
- Most solution answers are at least six digits (unless significant figures are relevant to the question/otherwise denoted)
- For credit your answer must be within 1% of the correct answer, unless tolerance is otherwise denoted (so entering in four digits to the right of the decimal is usually sufficient)
- Start with at least four significant digits for numeric entry; your response must be within 1% of the correct answer unless otherwise designated
- Scientific notation may use the format of "e" or "x10^"
- Comma use is fine.
- Do not use symbols in solutions (ie do not use $ in monetary solutions, but you can write 'dollars'-or the specified 'answer in units of ---- ' stated in the question, after your numeric answer).
- If offered, use the function pallet. If you don't see the pallet, plan on entering an actual number calculated out or simple expression (ex: 3x-5).
For applicable practice, your professor may opt to include a short 3 part question ( sig fig practice , #222082 ) for you to get use to what is and is not acceptable:
Note that if you get a 'that response has already been entered' message, try to use another way to say the same thing (ie, if used 10^, try e). If you continue to get the 'that response has already been entered' accept that it is not correct and try again. This is a safeguard in place so you don't spend all your tries insisting on an answer that is incorrect.
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Hours Tuesday – Wednesday 10AM-4PM
- 1.1 Chemistry in Context
- 1.2 Phases and Classification of Matter
- 1.3 Physical and Chemical Properties
- 1.4 Measurements
- 1.5 Measurement Uncertainty, Accuracy, and Precision
- 1.6 Mathematical Treatment of Measurement Results
- Key Equations
- 2.1 Early Ideas in Atomic Theory
- 2.2 Evolution of Atomic Theory
- 2.3 Atomic Structure and Symbolism
- 2.4 Chemical Formulas
- 2.5 The Periodic Table
- 2.6 Molecular and Ionic Compounds
- 2.7 Chemical Nomenclature
- 3.1 Formula Mass and the Mole Concept
- 3.2 Determining Empirical and Molecular Formulas
- 3.3 Molarity
- 3.4 Other Units for Solution Concentrations
- 4.1 Writing and Balancing Chemical Equations
- 4.2 Classifying Chemical Reactions
- 4.3 Reaction Stoichiometry
- 4.4 Reaction Yields
- 4.5 Quantitative Chemical Analysis
- 5.1 Energy Basics
- 5.2 Calorimetry
- 5.3 Enthalpy
- 6.1 Electromagnetic Energy
- 6.2 The Bohr Model
- 6.3 Development of Quantum Theory
- 6.4 Electronic Structure of Atoms (Electron Configurations)
- 6.5 Periodic Variations in Element Properties
- 7.1 Ionic Bonding
- 7.2 Covalent Bonding
- 7.3 Lewis Symbols and Structures
- 7.4 Formal Charges and Resonance
- 7.5 Strengths of Ionic and Covalent Bonds
- 7.6 Molecular Structure and Polarity
- 8.1 Valence Bond Theory
- 8.2 Hybrid Atomic Orbitals
- 8.3 Multiple Bonds
- 8.4 Molecular Orbital Theory
- 9.1 Gas Pressure
- 9.2 Relating Pressure, Volume, Amount, and Temperature: The Ideal Gas Law
- 9.3 Stoichiometry of Gaseous Substances, Mixtures, and Reactions
- 9.4 Effusion and Diffusion of Gases
- 9.5 The Kinetic-Molecular Theory
- 9.6 Non-Ideal Gas Behavior
- 10.1 Intermolecular Forces
- 10.2 Properties of Liquids
- 10.3 Phase Transitions
- 10.4 Phase Diagrams
- 10.5 The Solid State of Matter
- 10.6 Lattice Structures in Crystalline Solids
- 11.1 The Dissolution Process
- 11.2 Electrolytes
- 11.3 Solubility
- 11.4 Colligative Properties
- 11.5 Colloids
- 12.1 Chemical Reaction Rates
- 12.2 Factors Affecting Reaction Rates
- 12.3 Rate Laws
- 12.4 Integrated Rate Laws
- 12.5 Collision Theory
- 12.6 Reaction Mechanisms
- 12.7 Catalysis
- 13.1 Chemical Equilibria
- 13.2 Equilibrium Constants
- 13.3 Shifting Equilibria: Le Châtelier’s Principle
- 13.4 Equilibrium Calculations
- 14.1 Brønsted-Lowry Acids and Bases
- 14.2 pH and pOH
- 14.3 Relative Strengths of Acids and Bases
- 14.4 Hydrolysis of Salt Solutions
- 14.5 Polyprotic Acids
- 14.6 Buffers
- 14.7 Acid-Base Titrations
- 15.1 Precipitation and Dissolution
- 15.2 Lewis Acids and Bases
- 15.3 Multiple Equilibria
- 16.1 Spontaneity
- 16.2 Entropy
- 16.3 The Second and Third Laws of Thermodynamics
- 16.4 Free Energy
- 17.1 Balancing Oxidation-Reduction Reactions
- 17.2 Galvanic Cells
- 17.3 Standard Reduction Potentials
- 17.4 The Nernst Equation
- 17.5 Batteries and Fuel Cells
- 17.6 Corrosion
- 17.7 Electrolysis
- 18.1 Periodicity
- 18.2 Occurrence and Preparation of the Representative Metals
- 18.3 Structure and General Properties of the Metalloids
- 18.4 Structure and General Properties of the Nonmetals
- 18.5 Occurrence, Preparation, and Compounds of Hydrogen
- 18.6 Occurrence, Preparation, and Properties of Carbonates
- 18.7 Occurrence, Preparation, and Properties of Nitrogen
- 18.8 Occurrence, Preparation, and Properties of Phosphorus
- 18.9 Occurrence, Preparation, and Compounds of Oxygen
- 18.10 Occurrence, Preparation, and Properties of Sulfur
- 18.11 Occurrence, Preparation, and Properties of Halogens
- 18.12 Occurrence, Preparation, and Properties of the Noble Gases
- 19.1 Occurrence, Preparation, and Properties of Transition Metals and Their Compounds
- 19.2 Coordination Chemistry of Transition Metals
- 19.3 Spectroscopic and Magnetic Properties of Coordination Compounds
- 20.1 Hydrocarbons
- 20.2 Alcohols and Ethers
- 20.3 Aldehydes, Ketones, Carboxylic Acids, and Esters
- 20.4 Amines and Amides
- 21.1 Nuclear Structure and Stability
- 21.2 Nuclear Equations
- 21.3 Radioactive Decay
- 21.4 Transmutation and Nuclear Energy
- 21.5 Uses of Radioisotopes
- 21.6 Biological Effects of Radiation
- A | The Periodic Table
- B | Essential Mathematics
- C | Units and Conversion Factors
- D | Fundamental Physical Constants
- E | Water Properties
- F | Composition of Commercial Acids and Bases
- G | Standard Thermodynamic Properties for Selected Substances
- H | Ionization Constants of Weak Acids
- I | Ionization Constants of Weak Bases
- J | Solubility Products
- K | Formation Constants for Complex Ions
- L | Standard Electrode (Half-Cell) Potentials
- M | Half-Lives for Several Radioactive Isotopes
The temperature of 1 gram of burning wood is approximately the same for both a match and a bonfire. This is an intensive property and depends on the material (wood). However, the overall amount of produced heat depends on the amount of material; this is an extensive property. The amount of wood in a bonfire is much greater than that in a match; the total amount of produced heat is also much greater, which is why we can sit around a bonfire to stay warm, but a match would not provide enough heat to keep us from getting cold.
Heat capacity refers to the heat required to raise the temperature of the mass of the substance 1 degree; specific heat refers to the heat required to raise the temperature of 1 gram of the substance 1 degree. Thus, heat capacity is an extensive property, and specific heat is an intensive one.
(a) 47.6 J/°C; 11.38 cal °C −1 ; (b) 407 J/°C; 97.3 cal °C −1
1310 J; 313 cal
(a) 0.390 J/g °C; (b) Copper is a likely candidate.
We assume that the density of water is 1.0 g/cm 3 (1 g/mL) and that it takes as much energy to keep the water at 85 °F as to heat it from 72 °F to 85 °F. We also assume that only the water is going to be heated. Energy required = 7.47 kWh
lesser; more heat would be lost to the coffee cup and the environment and so Δ T for the water would be lesser and the calculated q would be lesser
greater, since taking the calorimeter’s heat capacity into account will compensate for the thermal energy transferred to the solution from the calorimeter; this approach includes the calorimeter itself, along with the solution, as “surroundings”: q rxn = −( q solution + q calorimeter ); since both q solution and q calorimeter are negative, including the latter term ( q rxn ) will yield a greater value for the heat of the dissolution
The temperature of the coffee will drop 1 degree.
5.7 × × 10 2 kJ
-2.2 kJ; The heat produced shows that the reaction is exothermic.
22.6. Since the mass and the heat capacity of the solution is approximately equal to that of the water, the two-fold increase in the amount of water leads to a two-fold decrease of the temperature change.
1.4 × × 10 2 Calories
The enthalpy change of the indicated reaction is for exactly 1 mol HCL and 1 mol NaOH; the heat in the example is produced by 0.0500 mol HCl and 0.0500 mol NaOH.
25 kJ mol −1
81 kJ mol −1
1.83 × × 10 −2 mol
–802 kJ mol −1
(a) −1615.0 kJ mol −1 ; (b) −484.3 kJ mol −1 ; (c) 164.2 kJ; (d) −232.1 kJ
−54.04 kJ mol −1
−2660 kJ mol −1
On the assumption that the best rocket fuel is the one that gives off the most heat, B 2 H 6 is the prime candidate.
(a) C 3 H 8 ( g ) + 5 O 2 ( g ) ⟶ 3 CO 2 ( g ) + 4 H 2 O ( l ) ; C 3 H 8 ( g ) + 5 O 2 ( g ) ⟶ 3 CO 2 ( g ) + 4 H 2 O ( l ) ; (b) 330 L; (c) −104.5 kJ mol −1 ; (d) 75.4 °C
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Access for free at https://openstax.org/books/chemistry/pages/1-introduction
- Authors: Paul Flowers, William R. Robinson, PhD, Richard Langley, Klaus Theopold
- Publisher/website: OpenStax
- Book title: Chemistry
- Publication date: Mar 11, 2015
- Location: Houston, Texas
- Book URL: https://openstax.org/books/chemistry/pages/1-introduction
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UT Quest Sign-Up Instructions In chemistry this year, you will be
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