4. 1000.0 mL of 14.0°C water is heated until its temperature is 37°C. If the specific heat of water is 4.18 J'g°C. calculate the amount of heat energy needed
to cause this rise in temperature.

Hello!

For this, first, we have to convert mL to g, for this:

1000 mL = 1000 g

Then, for calculate heat energy:

Q = m * Sh * ΔT

Data:

Q = Heat energy = ?

m = Mass = 1000 g

Sh = Specfic heat = 4,18 J/g.°C

ΔT = Variation of temperature = (37 °C - 14 °C)

Replacing:

Q = 1000 g * 4,18 J/g.°C * (37 °C - 14 °C)

Resolving:

Q = 96140 J

Result:

The heat energy needed is 96140 Joules.

= initial pressure

= final pressure = 2

= initial volume

= final volume = /4

= initial temperature = 20 c = 20 + 273 = 293 k

= final temperature = ?

using the equation