Calorimetry and Enthalpy Concepts

The video tutorial explains the use of calorimetry in chemistry to determine enthalpy changes, focusing on coffee cup calorimetry. It covers the q=mcΔT equation, specific heat capacity, and the process of measuring heat transfer. The tutorial includes a practical experiment to find the enthalpy of solution for sodium hydroxide, detailing the setup, data collection, and analysis, including calculating percent error.

What is a common use of calorimetry in chemistry?

• To find the enthalpy of a solution, reaction, or neutralization

• To calculate the pressure of a gas

• To measure the speed of a reaction

• To determine the color change in a reaction

What is the purpose of using a coffee cup calorimeter?

• To maintain constant pressure

• To measure the volume of gases

• To increase the reaction rate

• To decrease the temperature

In a calorimetry experiment, what is typically used as the surroundings?

• The reactants

• The calorimeter

• The water

• The air

How is the specific heat capacity of water typically expressed?

• 3.00 joules per gram per Celsius

• 4.18 joules per gram per Celsius

• 2.00 joules per gram per Celsius

• 1.00 joules per gram per Celsius

What does a negative enthalpy change indicate about a reaction?

• The reaction is non-spontaneous

• The reaction is endothermic

• The reaction is exothermic

• The reaction is at equilibrium

What is the first step in calculating the enthalpy of a reaction?

• Find the heat gained or lost by water

• Measure the final temperature

• Determine the moles of reactants

• Convert joules to kilojoules

What is the significance of the sign of enthalpy in a reaction?

• It determines the color change in the reaction

• It measures the pressure change in the reaction

• It shows whether the reaction is endothermic or exothermic

• It indicates the speed of the reaction

What is the enthalpy of solution for sodium hydroxide when 2.55 grams are dissolved?

• -38 kilojoules per mole

• -44.2 kilojoules per mole

• -24 kilojoules per mole

• -30 kilojoules per mole

What is the accepted value for the enthalpy of solution of sodium hydroxide?

• -44.2 kilojoules per mole

• -40 kilojoules per mole

• -38 kilojoules per mole

• -42 kilojoules per mole

What could be a potential source of error in a calorimetry experiment?

• Using water as the solvent

• Using a balance to measure mass

• Not accounting for heat loss to the surroundings

• Using a thermometer to measure temperature