What is specific heat capacity?

Which factor does NOT affect the temperature change of a substance?

What is specific latent heat?

Which process occurs when water turns into vapor?

Why does land heat up faster than water?

In a heating graph of water, where does the temperature remain constant?

How much heat is needed to raise 200 g of water from 20°C to 60°C? (Use c=4186 J/kg⋅Kc = 4186 \, J/kg \cdot Kc=4186J/kg⋅K)

If 10,000 J of heat is applied to increase the temperature of water by 5°C, what is the mass of the water? (Use c=4186 J/kg⋅Kc = 4186 \, J/kg \cdot Kc=4186J/kg⋅K)

500 g of a substance with a specific heat capacity of 2000 J/kg·K is heated with 5,000 J. What is the temperature change?

How much heat is required to melt 50 g of ice at 0°C? (Use L=333×103 J/kgL = 333 \times 10^3 \, J/kgL=333×103J/kg)

Calculate the total heat needed to heat 100 g of ice from -10°C to 0°C, then completely melt it. (Use c=2100 J/kg⋅Kc = 2100 \, J/kg \cdot Kc=2100J/kg⋅K for ice and L=333×103 J/kgL = 333 \times 10^3 \, J/kgL=333×103J/kg)

What is the amount of heat needed to heat 150 g of ice from -5°C to 100°C and completely vaporize it? (Use c=2100 J/kg⋅Kc = 2100 \, J/kg \cdot Kc=2100J/kg⋅K for ice, c=4186 J/kg⋅Kc = 4186 \, J/kg \cdot Kc=4186J/kg⋅K for water, and Lvaporization=2.3×106 J/kgL_{vaporization} = 2.3 \times 10^6 \, J/kgLvaporization​=2.3×106J/kg)

How much heat is needed to raise 250 g of water from 10°C to 30°C? (Use c=4186 J/kg⋅Kc = 4186 \, J/kg \cdot Kc=4186J/kg⋅K)

If 15,000 J is used to heat a substance by 10°C, and its specific heat is 1500 J/kg·K, what is its mass?

What is the temperature increase when 400 J is applied to 100 g of a substance with a specific heat of 400 J/kg·K?

How much energy is required to vaporize 100 g of water at 100°C? (Use L=2.3×106 J/kgL = 2.3 \times 10^6 \, J/kgL=2.3×106J/kg)

Calculate the heat needed to turn 80 g of ice from -10°C to steam at 100°C. (Use c=2100 J/kg⋅Kc = 2100 \, J/kg \cdot Kc=2100J/kg⋅K for ice, c=4186 J/kg⋅Kc = 4186 \, J/kg \cdot Kc=4186J/kg⋅K for water, Lfusion=333×103 J/kgL_{fusion} = 333 \times 10^3 \, J/kgLfusion​=333×103J/kg, and Lvaporization=2.3×106 J/kgL_{vaporization} = 2.3 \times 10^6 \, J/kgLvaporization​=2.3×106J/kg)

How much energy is needed to heat 1 kg of water in a kettle from 20°C to 100°C and then boil it completely? (Use c=4186 J/kg⋅Kc = 4186 \, J/kg \cdot Kc=4186J/kg⋅K and Lvaporization=2.3×106 J/kgL_{vaporization} = 2.3 \times 10^6 \, J/kgLvaporization​=2.3×106J/kg)

Determine the heat needed to change 150 g of ice from -15°C to water at 10°C. (Use c=2100 J/kg⋅Kc = 2100 \, J/kg \cdot Kc=2100J/kg⋅K for ice, c=4186 J/kg⋅Kc = 4186 \, J/kg \cdot Kc=4186J/kg⋅K for water, and L=333×103 J/kgL = 333 \times 10^3 \, J/kgL=333×103J/kg)

If 8,000 J is used to heat 500 g of a substance by 4°C, what is its specific heat capacity?