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higher CHEMISTRY > chemistry in society > Flashcards

chemistry in society Flashcards

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1
Q

Designing chemical processes to maximize profit, minimize environmental impact, and ensure safety and efficiency.

A

Industrial Process Design

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2
Q

Factors include availability, sustainability, and cost of feedstocks; opportunities for recycling; energy requirements; marketability of by-products; and product yield.

A

Factors Influencing Industrial Process Design

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3
Q

Environmental Considerations in Industrial ProcessesInclude minimizing waste, avoiding the use or production of toxic substances, and designing biodegradable products.

A

Environmental Considerations in Industrial Processes

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4
Q

Representations of chemical reactions using symbols and formulas to show reactants and products, including their states.

A

Chemical Equations

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5
Q

The amount of substance containing the same number of entities as there are in 12 grams of carbon-12.

A

Mole

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6
Q

The mass of one mole of a substance, calculated using the sum of the atomic masses of its constituent atoms.

A

Gram Formula Mass (GFM)

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7
Q

The volume occupied by one mole of a gas at a specific temperature and pressure, typically 22.4 L at STP (Standard Temperature and Pressure).

A

Molar Volume

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8
Q

A measure of the efficiency of a reaction, calculated by dividing the actual yield by the theoretical yield and multiplying by 100.

A

Percentage Yield

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9
Q

A measure of the efficiency of a chemical reaction in terms of the amount of starting materials that become useful products.

A

Atom Economy

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10
Q

The reactant that is completely consumed in a reaction, thus determining the maximum amount of product that can be formed.

A

Limiting Reactant

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11
Q

A reactant that remains after a chemical reaction has stopped due to the limiting reactant being completely used up.

A

Excess Reactant

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12
Q

The maximum amount of product that could be formed from given amounts of reactants, calculated based on the balanced chemical equation.

A

Theoretical Yield

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13
Q

The amount of product actually obtained from a reaction, often less than the theoretical yield due to inefficiencies.

A

Actual Yield

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14
Q

Explains how chemical reactions occur and why reaction rates differ, based on the frequency and energy of colliding particles.

A

Collision Theory

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15
Q

Factors include concentration, pressure, surface area (particle size), temperature, and collision geometry

A

Factors Affecting Reaction Rate

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16
Q

A graph that shows the energy changes during a chemical reaction, with reactants, products, and the activation energy.

A

Potential Energy Diagram

17
Q

The heat change associated with a chemical reaction, negative for exothermic reactions and positive for endothermic reactions.

A

Enthalpy Change (ΔH)

18
Q

The minimum energy required for reactants to collide and form an activated complex, leading to a chemical reaction.

A

activation energy

19
Q

A transient, unstable arrangement of atoms formed at the peak of the activation energy barrier during a chemical reaction.

A

Activated Complex

20
Q

A substance that increases the rate of a chemical reaction without being consumed, by lowering the activation energy.

A

Catalyst

21
Q

Temperature and Kinetic EnergyTemperature is a measure of the average kinetic energy of particles in a substance, influencing reaction rates.

A

Temperature and Kinetic Energy

22
Q

A graph that shows the distribution of kinetic energy among molecules in a sample at a given temperature.

A

Energy Distribution Diagram

23
Q

A measure of the total energy of a system, including internal energy and the energy required to displace its environment.

A

Enthalpy

24
Q

A reaction that releases heat to the surroundings, resulting in a negative enthalpy change (ΔH).

A

Exothermic Reaction

25
Q

A reaction that absorbs heat from the surroundings, resulting in a positive enthalpy change (ΔH).

A

Endothermic Reaction

26
Q

The energy transferred due to a temperature difference, calculated using Eh = cmΔT.

A

Heat Energy (Eh)

27
Q

The enthalpy change when one mole of a substance burns completely in oxygen.

A

Enthalpy of Combustion

28
Q

States that the enthalpy change for a chemical reaction is the same, regardless of the route taken.

A

Hess’s Law

29
Q

The energy required to break one mole of bonds in a gaseous molecule; mean bond enthalpy is an average over several compounds.

A

Bond Enthalpy

30
Q

A state in a closed system where the rates of the forward and reverse reactions are equal, and concentrations of reactants and products remain constant.

A

Dynamic Equilibrium

31
Q

A reaction that can proceed in both forward and reverse directions under certain conditions.

A

Reversible Reaction

32
Q

A technique used to separate and identify components in a mixture based on differences in polarity or molecular size.

A

Chromatography

33
Q

The time taken for a component to travel through the chromatography apparatus to the detector.

A

Retention Time

34
Q

A quantitative analysis method involving the measurement of the volume of a solution required to react with a known quantity of a substance.

A

Volumetric Analysis

35
Q

A technique where a solution of known concentration is used to determine the concentration of an unknown solution.

A

Titration

36
Q

Titre volumes that are within 0.2 cm³ of each other, indicating consistent results in titration.

A

Concordant Titres

37
Q

A solution of known concentration used in titrations.

A

Standard Solution

38
Q

A titration based on a redox reaction, often involving permanganate or dichromate as an oxidizing agent.

A

Redox Titration

39
Q

A substance that changes color at the endpoint of a titration, indicating the completion of the reaction.

A

Indicator

higher CHEMISTRY (3 decks)

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