Thermodynamics

Do molecules generally move faster at 45 C or 106 C?

• 45 C because molecules have more energy than in 106C

• 106 C because molecules have more energy than in 45C

• 106 C because molecules have less energy than in 45C

• 45C because molecules have less energy than in 106 C

Tags

NGSS.HS-PS1-5

When you place the metal in boiling water, heat flows from the _________ to the _______.

• metal to the boiling water

• bottom of the metal to the top half of the metal

• bottom of the water to the top of the water

• boiling water to the metal

Tags

NGSS.HS-PS3-4

DON'T RUSH, YOU HAVE TIME.

Water droplets condensing on the inside of a window on a cold day. Is this process exothermic or endothermic?

• Gases condense to form liquids. Gases are moving faster than liquids, the air around the window has a higher temperature/kinetic energy. Releasing energy to get water droplets, which is is Exothermic

• Gases condense to form liquids. Gases are moving faster than liquids, the air around the window has a higher temperature/kinetic energy. Releasing energy to get water droplets, which is is Endothermic

• Gases condense to form liquids. Gases particles are moving slower than liquids. Releasing energy to get water droplets, which is is Endothermic

• Gases condense to form liquids. Gases particles are moving slower than liquids. Releasing energy to get water droplets, which is is Exothermic

Tags

NGSS.HS-PS1-4

DON'T RUSH, YOU HAVE TIME.

Frying an egg on a skillet. Referring to the egg, would the Enthalpy change be positive or negative?

• Skillet is absorbing heat energy from the egg. Absorbing energy is Endothermic. Endothermic has a positive Enthalpy

• Egg absorbing heat energy from the skillet. Absorbing energy is Endothermic. Endothermic has a positive Enthalpy

• Egg absorbing heat energy from the skillet. Releasing energy is Exothermic. Exothermic has a positive Enthalpy

• Egg absorbing heat energy from the skillet. Releasing energy is Exothermic. Exothermic has a negative Enthalpy

Tags

NGSS.HS-PS3-4

Define ΔH

• Change in Specific Heat; Heat by one Degree Celsius

• Change in Temperature; the energy we calculate; Degree Celsius

• Change in Enthalpy; the energy/heat we calculate

• Change in Time; time travel

Tags

NGSS.HS-PS3-1

Define Exothermic

• Energy is released; ΔH is negative; Going from Gas to Liquid, Liquid to Solid

• Energy is absorbed; ΔH is positive; Going from Gas to Liquid, Liquid to Solid

• Energy is released; ΔH is positive; Going from Solid to Liquid, Liquid to Gas

• Energy is absorbed; ΔH is negative; Going from Gas to Liquid, Liquid to Solid

Tags

NGSS.HS-PS1-4

Define Endothermic

• Energy is absorbed; ΔH is negative; Going from Liquid to Gas, and Gas to Liquid

• Energy is released; ΔH is negative; Going from Solid to Liquid, and Liquid to Gas

• Energy is released; ΔH is positive; Going from Solid to Liquid, and Liquid to Gas

• Energy is absorbed; ΔH is positive; Going from Solid to Liquid, and Liquid to Gas

Tags

NGSS.HS-PS1-4

Specific Heat is..

• the temperature initial minus temperature final

• the amount of heat/energy required to raise 1 gram of a substance by 1°C (or K) aka "C"

• the temperature final minus temperature initial

• the item in a system with given weight in grams

Tags

NGSS.HS-PS3-4

READ CAREFULLY! YOU HAVE TIME!

A substance with a low specific heat requires less energy to heat up and a substance with high specific heat require more energy to heat up and heats up slower

• TRUE

• FALSE

Tags

NGSS.HS-PS3-4

YOU HAVE TIME!

How much energy is needed to raise the temperature of a 20.0g piece of copper from 15.0 degrees Celsius to 25.0 degrees Celsius? (The specific heat of copper is 0.385 J/g C)

• 20 X (25-15) =70 J

• 20 X .385 X (25-15)= 77 J

• 20 X .385 X (15-25)= 62 J

• 20 X .385 X (15-0)= 77 J

Tags

NGSS.HS-PS3-4

NGSS.HS-PS3-1