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

aquifers are bounded above and below by impermeable rock. the driving force of groundwater movement in confined aquifers is pressure, rather than gravity.