Thermochemistry Overview

<p>Heat exchanged between system and surroundings (A)</p> Signup and view all the answers

<p>Exothermic process (B)</p> Signup and view all the answers

<p>Transfers heat but not mass (D)</p> Signup and view all the answers

<p>Positive overall (D)</p> Signup and view all the answers

<p>To absorb heat from the external environment (D)</p> Signup and view all the answers

<p>Endothermic reactions (D)</p> Signup and view all the answers

<p>Exothermic process (D)</p> Signup and view all the answers

<p>Isolated system (C)</p> Signup and view all the answers

<p>Both exothermic and endothermic processes (A)</p> Signup and view all the answers

<p>Exothermic reaction (A)</p> Signup and view all the answers

<p>q (B)</p> Signup and view all the answers

<p>Everything outside the system (C)</p> Signup and view all the answers

<p>Heat, light, and sound (A)</p> Signup and view all the answers

<p>Physical Change (D)</p> Signup and view all the answers

<p>Heat changes in chemical reactions (A)</p> Signup and view all the answers

<p>Chemical Change (C)</p> Signup and view all the answers

<p>Thermocolor Cup (C)</p> Signup and view all the answers

<p>Prevent heat transfer from surroundings to liquid (C)</p> Signup and view all the answers

<p>It helps understand the amount of energy produced (C)</p> Signup and view all the answers

<p>Chemical Change (A)</p> Signup and view all the answers

<p>Physical Change (C)</p> Signup and view all the answers

<p>q = mc∆T (D)</p> Signup and view all the answers

<p>Extensive property (D)</p> Signup and view all the answers

<p>H2O(l) (C)</p> Signup and view all the answers

<p>J/g°C (D)</p> Signup and view all the answers

<p>The change in temperature (C)</p> Signup and view all the answers

<p>Fe (B)</p> Signup and view all the answers

<p>Through calorimetry tests (D)</p> Signup and view all the answers

<p>Specific heat is an intensive property. (B)</p> Signup and view all the answers

<p>$-164 J$ (A)</p> Signup and view all the answers

<p>$69.5 J$ (C)</p> Signup and view all the answers

<p>$-1200 J$ (C)</p> Signup and view all the answers

<p>$-1670 J$ (C)</p> Signup and view all the answers

<p>$-334 J$ (A)</p> Signup and view all the answers

<p>Exothermic process (B)</p> Signup and view all the answers

<p>Using a calorimeter (B)</p> Signup and view all the answers

<p>They conducted experiments using ice-calorimeter (B)</p> Signup and view all the answers

<p>Heat added to the system (D)</p> Signup and view all the answers

<p>Temperature change (D)</p> Signup and view all the answers

<p>q = mcΔT (B)</p> Signup and view all the answers

<p>4184 J (A)</p> Signup and view all the answers

<p>Exothermic reaction (D)</p> Signup and view all the answers

<p>ΔT = Tf - Ti (D)</p> Signup and view all the answers

<p>m (D)</p> Signup and view all the answers

<p>8000 J (A)</p> Signup and view all the answers

<p>The amount of heat required to change the temperature of 1 g of a substance by 1°C (C)</p> Signup and view all the answers

<p>Surrounding temperature (C)</p> Signup and view all the answers

<p>-68400 J (A)</p> Signup and view all the answers

<p>Positive (C)</p> Signup and view all the answers

A change in a substance that does not change its chemical composition.

A change that alters a substance's chemical composition and creates new substances.

The study of heat changes in chemical reactions.

A cup that changes color with temperature.

A flask designed to prevent heat transfer, keeping liquids at a constant temperature.

Burning fuels to release energy.

The amounts of substances needed for a chemical reaction.

The amounts of substances produced in a chemical reaction.

A chemical reaction that releases heat into the surroundings.

A chemical reaction that absorbs heat from the surroundings.

These systems use endothermic processes to cool things down. They absorb heat from the area they are cooling and release it elsewhere.

Many cooking methods involve heat transfer. Endothermic reactions are used in baking to help dough rise.

The chemical processes in your body that break down food and release energy.

These batteries use exothermic reactions to generate electricity.

These rely on exothermic reactions that release a large amount of energy quickly, producing heat, light, and sound.

The transfer of thermal energy between two objects at different temperatures. It usually involves absorption or release during a process.

A system that can exchange both energy and mass with its surroundings.

A system that can exchange energy with its surroundings but not mass.

A system that cannot exchange energy or mass with its surroundings.

A process that absorbs heat from its surroundings.

A process that releases heat into its surroundings.

The total energy of an isolated system remains constant; energy can be transformed from one form to another, but it cannot be created or destroyed.

The total energy of a system, including kinetic and potential energy of the molecules.

Heat exchange between a system and its surroundings. Positive q means heat is absorbed by the system, negative q means heat is released.

The change in the total energy of a system, represented by ΔU, and calculated by the formula ΔU = q + w, where q is heat and w is work.

A reaction where heat is released to the surroundings, resulting in a negative value for ΔU.

A reaction where heat is absorbed from the surroundings, resulting in a positive value for ΔU.

The energy transferred by the system as it performs work, resulting in a negative value for work (w).

The energy transferred to the system when work is done on it, resulting in a positive value for work (w).

The energy transferred to the system as heat, resulting in a positive value for heat (q).

The energy lost by the system through heat transfer, resulting in a negative value for heat (q).

The science of measuring heat changes in chemical or physical processes using a calorimeter.

A device used in calorimetry to measure heat changes during reactions or processes.

The amount of heat energy required to raise the temperature of 1 gram of a substance by 1 degree Celsius.

The difference in temperature between the initial and final states of a substance.

The amount of matter in a substance.

This formula calculates the heat (q) transferred during a temperature change, where 'm' is mass, 'c' is specific heat capacity, and '∆T' is the temperature change.

To find the final temperature, rearrange the heat transfer formula: Tf = (q / mc) + Ti.

To find the initial temperature, rearrange the heat transfer formula: Ti = Tf - (q / mc).

Ensure consistent units are used: heat (q) in Joules (J), mass (m) in grams (g), specific heat capacity (c) in J/g°C, and temperature (T) in degrees Celsius (°C).

The heat capacity (C) measures a substance's ability to absorb heat without significantly changing its temperature. It's expressed in J/°C.

The specific heat (c) is the amount of heat needed to raise one gram of a substance by one degree Celsius. It's an intensive property, meaning it doesn't depend on the amount of substance. Measured in J/g°C.

The formula for heat capacity is: q = C∆T, where q is the heat energy, C is the heat capacity, and ∆T is the change in temperature.

The formula for specific heat is: q = mc∆T, where q is the heat energy, m is the mass, c is the specific heat, and ∆T is the change in temperature.

The amount of heat transfer (q) is proportional to the change in temperature (∆T). This proportionality is determined by the heat capacity (C) of the substance.

The total heat capacity (C) of a substance is equal to the product of its mass (m) and specific heat (c). This can be represented as C = mc.

An extensive property depends on the amount of matter in a substance (like mass or volume). An intensive property does not depend on the amount (like specific heat or temperature).