How much heat is required to warm 1.50L of water from 25.0C to 100.0C? (Assume a density of 1.0g/mL for the water.)

My brain wants to just start with 1.5L and use density as a conversion factor but I seriously think I'm missing something. I don't really understand the heat equation, but I'm thinking I might need to use q = mCAT?

The amount of heat required to warm given amount of water is 470.9 kJ

Explanation:

To calculate the mass of water, we use the equation:

Density of water = 1 g/mL

Volume of water = 1.50 L = 1500 mL    (Conversion factor:  1 L = 1000 mL)

Putting values in above equation, we get:

To calculate the heat absorbed by the water, we use the equation:

where,

q = heat absorbed

m = mass of water = 1500 g

c = heat capacity of water = 4.186 J/g°C

= change in temperature =

Putting values in above equation, we get:

Hence, the amount of heat required to warm given amount of water is 470.9 kJ

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