Heating Curve and Phase Changes Quiz

True (A)

100°C

<p>120, 125</p> Signup and view all the answers

<p>Common salt (NaCl) = Increases boiling point High altitude = Decreases boiling point Pressure cooker = Increases boiling point Water at standard pressure = Boiling point of 100°C</p> Signup and view all the answers

<p>336000 J/kg (D)</p> Signup and view all the answers

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

<p>latent heat</p> Signup and view all the answers

<p>80</p> Signup and view all the answers

<p>Ice = 80 cal/g Mercury = 3 cal/g Copper = 43 cal/g Silver = 21 cal/g</p> Signup and view all the answers

The temperature at which a liquid changes to a gas. For water, this is 100°C at standard atmospheric pressure.

A graph plotting the temperature of a substance against time as it is heated. It shows different phases of the substance (solid, liquid, gas) and the energy changes involved.

The boiling point of a liquid can be affected by changes in pressure. Higher pressure increases the boiling point, while lower pressure decreases it.

Adding impurities to a liquid, like salt to water, increases its boiling point.

The process where a liquid changes into a gas. This occurs when the vapor pressure of the liquid equals the surrounding atmospheric pressure.

The amount of heat energy absorbed or released during a phase change of a substance, at a constant temperature. It's measured per unit mass and is different for different substances.

The specific latent heat of fusion is the amount of heat energy required to melt a unit mass of a solid substance at its melting point without changing its temperature. It also represents the heat energy released during freezing.

The amount of heat absorbed by 1 kg of ice at 0°C to convert it into water at 0°C. Conversely, 1 kg of water at 0°C releases the same amount of heat to turn into ice at 0°C.

Kinetic model describes the motion of particles within a substance. When a substance melts, the energy absorbed (latent heat) increases the kinetic energy of the molecules, allowing them to overcome the attractive forces holding them in a fixed position, thus causing them to move more freely and change into a liquid.

A table comparing the specific latent heat of fusion, in both calories/gram and Joules/kilogram, for common substances like mercury, sulfur, silver, paraffin wax, copper, and ice.