100.0g of 4.0c water is heated until its temperature is 37c. 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.

m = 100g

c = 4.18
∆T = 33°C

Q = mc∆T
Q = 100g * 4.18 * 33°C
= 13794J

Compare the energy needed to raise the temperature of 1kg of water from 20°C to 100°C and the energy needed to boil 1 kg of water at 100°C

13,794

To calculate the amount of heat energy needed to cause this rise in temperature, you can use the formula:

Q = m * c * ΔT

Where:
Q = heat energy (in joules)
m = mass of the water (in grams)
c = specific heat capacity of water (in joules/gram Celsius)
ΔT = change in temperature (in Celsius)

Given values:
m = 100.0 g
c = 4.18 J/g°C
ΔT = 37°C - 4.0°C = 33°C

Now, substitute the given values into the formula:

Q = 100.0 g * 4.18 J/g°C * 33°C
Q = 13,734 J

Therefore, the amount of heat energy needed to cause this rise in temperature is 13,734 joules.

q = mass H2O x specific heat x (Tfinal-Tinitial)

YOu know mass, specific heat, Tfinal and Tinitial. Solve for q.