What is the SI unit of specific heat capacity?

Why do materials with high specific heat capacity take longer to heat?

What happens to the temperature of a substance during melting?

What is the main difference between latent heat of fusion and vaporization?

Why is steaming food an efficient cooking method?

Which state of matter generally expands the most with heat?

How much heat is needed to raise 250 g of water from 20°C to 80°C? (Use c=4186 J/kg⋅Kc = 4186 \, J/kg \cdot Kc=4186J/kg⋅K)

If 12,000 J is used to heat 400 g of water, what is the temperature increase? (Use c=4186 J/kg⋅Kc = 4186 \, J/kg \cdot Kc=4186J/kg⋅K)

How much heat is required to melt 100 g of ice at 0°C? (Use L=333×103 J/kgL = 333 \times 10^3 \, J/kgL=333×103J/kg)

What is the temperature change when 5,000 J is applied to 250 g of a substance with a specific heat of 2,000 J/kg·K?

How much energy is needed to vaporize 75 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 100 g of ice from -5°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 heat is needed to raise 150 g of water from 25°C to 75°C? (Use c=4186 J/kg⋅Kc = 4186 \, J/kg \cdot Kc=4186J/kg⋅K)

If 5,000 J of heat is applied to increase the temperature of a 1 kg metal by 10°C, what is the specific heat capacity of the metal?

What is the mass of a substance if 10,000 J of heat is needed to increase its temperature by 20°C, and it has a specific heat of 2,500 J/kg·K?

How much energy is required to heat 1 kg of water from 0°C to 100°C and then boil it completely? (Use c=4186 J/kg⋅Kc = 4186 \, J/kg \cdot Kc=4186J/kg⋅K and L=2.3×106 J/kgL = 2.3 \times 10^6 \, J/kgL=2.3×106J/kg)

What is the final temperature if 10,000 J of heat is applied to 500 g of a substance with a specific heat of 1,000 J/kg·K and an initial temperature of 25°C?

How much heat is needed to raise 300 g of a liquid from 10°C to 50°C, if its specific heat is 2,000 J/kg·K?

Calculate the energy required to melt 200 g of ice at 0°C and then raise the temperature of the water to 25°C. (Use c=4186 J/kg⋅Kc = 4186 \, J/kg \cdot Kc=4186J/kg⋅K and L=333×103 J/kgL = 333 \times 10^3 \, J/kgL=333×103J/kg)

If 8,000 J of energy is needed to heat 500 g of a substance by 5°C, what is its specific heat capacity?