Chemistry Chapter 1 Quiz
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Kinetic Energy

Energy of motion. Objects in motion possess kinetic energy.

First Law of Thermodynamics

Energy cannot be created or destroyed, only transformed from one form to another.

State Function

A property that depends only on the current state of a system, not on the path taken to reach that state.

Enthalpy Change (ΔH)

Heat absorbed or released by a system at constant pressure.

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Heat Capacity

Amount of heat required to raise the temperature of a substance by 1 degree Celsius.

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Potential Energy

Energy stored in an object due to its position or configuration.

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Specific Heat Capacity

Amount of heat needed to raise the temperature of 1 gram of a substance by 1 degree Celsius.

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Hess's Law

The enthalpy change for a reaction is the same whether it occurs in one step or multiple steps.

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Boyle's Law

For a fixed amount of gas at a constant temperature, pressure and volume are inversely proportional.

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Dalton's Law of Partial Pressures

The total pressure of a mixture of gases is equal to the sum of the partial pressures of the individual gases.

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Kinetic Molecular Theory (gases)

Theory about the behavior of gas particles, explaining their motion and interactions.

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Effusion

The escape of gas particles through a small opening.

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Ideal Gas vs. Real Gas

Ideal gases follow gas laws perfectly, while real gases deviate due to particle interactions.

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Kinetic Energy Example

Energy of motion, a rolling ball is an example

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1st Law Thermodynamics

Energy can't be created or destroyed, only changed

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State Function Example

Property only depends on current state, not the path taken

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Enthalpy Change (ΔH)

Heat absorbed or released at constant pressure

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Heat Capacity

Heat needed to raise the temperature by 1°C

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Potential vs Kinetic energy

Potential is stored energy. Kinetic is energy of movement

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Specific Heat Capacity

Heat needed to change 1 gram of substance by 1°C

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Hess's Law

Enthalpy change for a reaction is same whether it happens over multiple steps or not

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Boyle's Law

Constant temp, pressure & volume inversely proportional

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Dalton's Law Partial Pressures

Total pressure is sum of partial pressures of gases

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Kinetic Molecular Theory (gases)

Gas particles are in constant motion

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Effusion

Gas particles escaping through an opening

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Ideal vs. Real Gases

Ideal gases follow gas laws perfectly, while real deviate due to particle interactions

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Kinetic Energy Example

Energy of motion; a rolling ball.

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First Law of Thermodynamics

Energy cannot be created or destroyed, only transformed.

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State Function

Property depending only on the system's current state, not path taken.

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Enthalpy Change (ΔH)

Heat absorbed or released at constant pressure.

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Heat Capacity

Amount of heat needed to raise the temperature of a substance by 1 °C.

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Potential vs Kinetic energy

Potential = stored energy; Kinetic = energy of motion.

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Specific Heat Capacity

Heat needed to change 1 gram of substance by 1°C.

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Hess's Law

Enthalpy change for a reaction is same, whether one or many steps.

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Boyle's Law

Constant Temperature: pressure and volume inversely proportional.

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Dalton's Law Partial Pressures

Total pressure = sum of partial pressures of gases.

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Kinetic Molecular Theory (gases)

Gas particles in constant, random motion.

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Effusion

Gas particles escaping through a small opening

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Ideal vs. Real Gases

Ideal gases follow gas laws perfectly, real gases have deviations due to particle interactions.

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Kinetic Energy

Energy of motion. Objects in movement possess kinetic energy.

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Study Notes

Quiz 1: Chemistry 1

  • Instructions: Answer all questions, show work for calculations, and use appropriate units.

Multiple Choice Questions

  • Question 1: A rolling ball is an example of kinetic energy.
  • Question 2: The First Law of Thermodynamics states energy cannot be created or destroyed, only transformed.
  • Question 3: Enthalpy is a state function.
  • Question 4: Enthalpy change (ΔH) is defined as the heat absorbed or released at constant pressure.
  • Question 5: Heat capacity is the amount of heat required to raise the temperature of a substance by 1 degree Celsius, and it is independent of the mass of the substance.

Short Answer Questions

  • Question 6: Potential energy is stored energy due to position or composition (e.g., water behind a dam, a compressed spring). Kinetic energy is energy of motion (e.g., a moving car, a rolling ball).
  • Question 7: Enthalpy is a state function because its value only depends on the initial and final states of the system, not the path taken.
  • Question 8: Calculation for specific heat capacity of a metal.
    • Heat gained by water (using q = mcΔT)
    • Heat lost by metal (is equal in magnitude but opposite in sign to heat gained by water)
    • Calculate specific heat capacity of a metal (using equation)

Calculations and Conceptual Questions

  • Question 9: Hess's Law calculation for enthalpy change for a reaction. (involves manipulating chemical equations).
  • Question 10: Caloric content of food relates to thermochemistry via energy changes during the metabolic process, which is similar to combustion reactions in terms of energy released (heat/energy from bonds).
  • Question 11: Gases exert pressure on container walls due to their constant, rapid and random motion and collisions.
  • Question 12: Boyle's Law states that for a given mass of gas at constant temperature, volume and pressure are inversely related (PV=constant).
  • Question 13: Calculation of volume of a gas when pressure and temperature are changing based on Combined Gas Law.
  • Question 14: Calculation of moles of a gas using Ideal Gas Law.
  • Question 15: Dalton's Law of Partial Pressures: Total pressure in a mixture of non-reacting gases equals the sum of the partial pressures of each individual gas.

Additional Questions

  • Question 16: Kinetic-Molecular Theory describes gas particles as small, hard spheres in constant, random motion, and collisions are perfectly elastic.
  • Question 17: Graham's Law of Effusion: The rate of effusion of a gas is inversely proportional to the square root of its molar mass. Compare the effusion rates of helium and oxygen.
  • Question 18: Ideal gases vs. Real Gases: Ideal gases assume no intermolecular forces and negligible volume of gas particles. Real gases have intermolecular forces and a finite volume

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Chemistry 1 Practice Exam 4 (PDF)

Description

Test your knowledge on fundamental concepts in chemistry, including kinetic and potential energy, the First Law of Thermodynamics, and enthalpy. This quiz includes both multiple choice and short answer questions, ensuring a comprehensive assessment of your understanding.

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