Question

How much heat (in kj) must be absorbed by a 15.0 g sample of water to raise its temperature from 25.0 °c to 55.0 °c? note: the specific heat capacity for water is 4.184j/(g °c)

A. 1.88 kj
B. 0.107 kj
C. 1.57 kj
D. 3.45 kj

Answer 1

The amount of heat required to raise the temperature of the water from 25.0°C to 55.0°C is approximately 1.88 KJ.

Step-by-step explanation:

To calculate the amount of heat (in KJ) required to raise the temperature of water from 25.0°C to 55.0°C, we can use the formula:

q = mcΔT

Where:

• q is the amount of heat in KJ
• m is the mass of the water in grams (15.0 g)
• c is the specific heat capacity of water (4.184 J/(g °C))
• ΔT is the change in temperature (55.0°C - 25.0°C = 30.0°C)

Substituting the values into the formula, we get:

q = (15.0 g) * (4.184 J/(g °C)) * (30.0°C)

q = 1881.6 J

Since we need the answer in KJ, we divide the result by 1000:

q = 1.8816 KJ

Therefore, the amount of heat required to raise the temperature of the water from 25.0°C to 55.0°C is approximately 1.88 KJ.