Calorimetry Quiz - Bomb Calorimeters

False (B)

C

<p>T</p> Signup and view all the answers

<p>Reaction Chamber = Houses the sample during combustion Thermometer = Monitors temperature change O₂ Inlet = Provides oxygen for the reaction Motorized Stirrer = Ensures uniform temperature in water bath</p> Signup and view all the answers

<p>Color of the substance (D)</p> Signup and view all the answers

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

<p>Enthalpy change</p> Signup and view all the answers

<p>T</p> Signup and view all the answers

<p>To measure the heat changes associated with chemical reactions (D)</p> Signup and view all the answers

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

<p>Specific heat capacity = The amount of heat needed to change the temperature of a substance by 1°C ΔH = Enthalpy change of a reaction Calorimetry = The measurement of heat changes in physical and chemical processes Kinetic energy = Energy of motion that can lead to temperature change</p> Signup and view all the answers

<p>Lid</p> Signup and view all the answers

<p>water</p> Signup and view all the answers

<p>Simple Calorimeter = Uses a styrofoam cup and a lid Flame Calorimeter = Uses a burner and a copper calorimeter Bomb Calorimeter = Includes ignition wires and a steel container All Calorimeters = Measure heat changes in reactions</p> Signup and view all the answers

<p>The heat released or absorbed by the system (D)</p> Signup and view all the answers

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

<p>ΔH = -Q</p> Signup and view all the answers

<p>1.0</p> Signup and view all the answers

<p>Q = Heat absorbed or released by the system c = Specific heat capacity of water m = Mass of water ΔT = Change in temperature of the water</p> Signup and view all the answers

<p>To compare quantities of different fuels (B)</p> Signup and view all the answers

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

<p>Enthalpy change</p> Signup and view all the answers

<p>water</p> Signup and view all the answers

<p>Heat lost equals heat gained. (C)</p> Signup and view all the answers

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

<p>closed</p> Signup and view all the answers

<p>Zeroth Law = Heat flows from hot to cold. First Law = Energy cannot be created or destroyed. Calorimetry = Process of measuring energy change indirectly. Thermochemistry = Study of energy change in chemical reactions.</p> Signup and view all the answers

<p>Theoretical value of the reaction (C)</p> Signup and view all the answers

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

<p>Eff</p> Signup and view all the answers

<p>change in temperature</p> Signup and view all the answers

<p>Eff = Efficiency Q = Output from heating $ ext{ΔH}$ = Input of reaction $m$ = Mass of the material</p> Signup and view all the answers

Heat always moves from a hotter object to a colder object.

Energy cannot be created or destroyed, it can only change forms.

The study of energy changes in chemical reactions.

A device used to measure the heat changes in a chemical reaction.

The process of measuring heat changes using a calorimeter.

In calorimetry experiments, we assume no heat escapes the system because the styrofoam container is considered a perfect insulator.

We disregard the energy absorbed or released by the calorimeter itself.

We only consider the heat absorbed or released by water, ignoring any other components present.

We assume that 1 milliliter of water has a mass of 1 gram.

The heat change of a reaction is represented by the enthalpy change ('Delta H') and is equal to the heat absorbed or released by the system ('Q').

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

The change in temperature of a substance or system during a reaction, measured in degrees Celsius or Fahrenheit.

The total amount of energy contained within a system, including its potential and kinetic energy.

The amount of heat energy transferred between a system and its surroundings, measured in Joules (J).

A simple calorimeter measures the heat changes in a chemical reaction using a styrofoam cup, thermometer, stirrer, and lid to minimize heat loss. The cup is often surrounded by an insulating outer container filled with water.

A flame calorimeter uses a burner to heat a copper calorimeter containing water. The temperature change of the water measures the heat produced by the flame.

A bomb calorimeter is used to measure the heat of combustion of a sample. The sample is ignited inside a steel container (the bomb) surrounded by water. The temperature change in the water is measured.

The styrofoam cup in a simple calorimeter is useful because it is a good insulator and minimizes heat loss to the surroundings. This allows for a more accurate measurement of the heat change in the reaction.

The water surrounding the bomb in a bomb calorimeter absorbs the heat released by the combustion of the sample. The temperature change of the water is directly proportional to the heat released by the reaction.

A sealed, insulated container used to measure the energy released or absorbed in a chemical reaction, especially those involving explosions or implosions.

A fine wire submerged in the reaction chamber of a bomb calorimeter that ignites the sample for the reaction.

The specific heat capacity of the bomb calorimeter, representing the amount of energy needed to raise its temperature by 1 degree Celsius.

The change in enthalpy of a reaction measured using a bomb calorimeter, symbolized as ΔH. This value is negative for exothermic reactions and positive for endothermic reactions.

The enthalpy change per mole of reactant in a reaction, symbolized as nHm, calculated using the bomb calorimeter constant and temperature change.

The amount of heat energy absorbed or released during a chemical reaction.

The heat energy absorbed by the pot, calculated using the mass of the pot, its specific heat capacity, and the change in its temperature.

The heat energy absorbed by the water, calculated using the mass of the water, its specific heat capacity, and the change in its temperature.

A measure of how much energy is transferred from the input to the output in a process.

The energy released in a chemical reaction, usually calculated using the enthalpy of combustion.

The energy gained by the material being heated, calculated using the change in temperature of the material.

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

The amount of heat released by a chemical reaction, typically expressed in joules per mole.