Question

A burning candle is placed under a can of water. The mass of the water is 125.30 g and the heat energy the water absorbed from the burning candle is 5.75 kJ. What is the change in temperature of the water?

Multiple Choice Answers:
A. 0.010967940804402129 °C
B. 0.10967940804402129 °C
C. 1.0967940804402129 °C
D. 10.967940804402129 °C

Answer 1

The change in temperature of the water when 5.75 kJ of heat is absorbed is about 10.97 °C. This calculation is done by using the specific heat capacity of water and the mass of the water to find the temperature change.

Step-by-step explanation:

To calculate the change in temperature of the water, we will use the formula:

q = m × c × ΔT

Where:

• q is the heat energy absorbed (in joules or J)
• m is the mass of the water (in grams or g)
• c is the specific heat capacity of water (4.184 J/g°C)
• ΔT is the change in temperature (°C)

Since we are given the heat energy in kilojoules (kJ), we first need to convert it to joules (1 kJ = 1000 J):

q = 5.75 kJ × 1000 = 5750 J

Now, we can rearrange the formula to solve for ΔT:

ΔT = q / (m × c)

ΔT = 5750 J / (125.30 g × 4.184 J/g°C)

ΔT = 5750 / (125.30 × 4.184)

ΔT = 5750 / 524.2272

ΔT ≈ 10.967940804402129 °C

The correct answer is D. 10.967940804402129 °C.