Question

What is the final temperature of a water sample if 12.15 kJ of energy is added to 475 g of water at an initial temperature of 2.5°C?

Answer 1

To calculate the final temperature of the water, use the specific heat capacity formula and rearrange it to solve for the change in temperature (ΔT), then add ΔT to the initial temperature.

Step-by-step explanation:

To find the final temperature of a sample of water after adding energy, we need to use the specific heat capacity of water. The specific heat capacity of water is approximately 4.18 J/g°C, which tells us how much heat is needed to raise the temperature of 1 gram of water by 1°C.
To solve this problem, we will use the formula:
Q = mcΔT, where:
Q = heat energy added (in joules),
m = mass of the water (in grams),
c = specific heat capacity (in J/g°C),
ΔT = change in temperature (in °C).

First, convert the energy from kilojoules to joules:
12.15 kJ = 12,150 J.

Then, rearrange the formula to solve for ΔT:
ΔT = Q / (mc).

Now, plug in the values:
ΔT = 12150 J / (475 g × 4.18 J/g°C).

After calculating ΔT, add it to the initial temperature to get the final temperature.