Heat

Calculate the amount of energy needed to convert 250. g of ice at - 8.0 °C to steam at 150.°C. 

• 833 kJ
• 165 kJ
• 782 kJ
• 251 kJ

In an exothermic reaction:

• ΔH is positive because energy is gained
• ΔH is negative because energy is gained
• ΔH is positive because energy is lost
• ΔH is negative because energy is lost

How much heat is required to raise the temperature of a sample of copper from 10.0°C to 55.0°C, if its mass is 10.00 g?

• 1881 J
• 250. J
• 173 J
• 359 J

Tags

NGSS.HS-PS3-1

Heat flows from

• cold to hot
• upstream
• freezing to boiling
• hot to cold

Tags

NGSS.HS-PS3-4

 A 16.0 g metallic sample was heated from 0°C to 35.0°C. It absorbed 248.7 J of energy. What is the identity of the metal?

• Magnesium
• Nickle
• Zinc
• Aluminium

Tags

NGSS.HS-PS3-4

Consider the reaction:
2 H₂O + energy → 2H₂ + O₂

• exothermic, releasing energy
• exothemic, absorbing energy
• endothermic, absorbing energy
• endothermic, releasing energy

Tags

NGSS.HS-PS1-4

H₂ + Cl₂ → 2 HCl + 1845 kJ
Is this reaction endothermic or exothermic?

• Endothermic 
• Exothermic

Tags

NGSS.HS-PS1-4

What letter represents boiling?

• B
• C
• D
• E

Tags

NGSS.MS-PS1-4

NGSS.MS-PS3-4

What letter represents a liquid being heated?

• A
• B
• C
• D

Tags

NGSS.HS-PS3-4

Calorimetry Question:
A piece of metal with a mass of 82.9 g is heated to 100.5°C and dropped into 71.4 g of water at 20.0°C.  The final temperature of the system is 30.2°C.  What is the identity of the metal?

• Iron
• Copper
• Gold
• Titanium

Tags

NGSS.HS-PS3-4