How much energy is gained by a 40.8g sample of water whose temperature increases from 22 degrees celsius to 35 degrees celsius when left in the sun?
To calculate the energy gained by the water sample, we need to use the formula for calculating heat energy:
Q = m * c * ΔT
Where:
Q is the heat energy gained or lost by the sample
m is the mass of the sample
c is the specific heat capacity of water
ΔT is the change in temperature (final temperature - initial temperature)
Let's break this down step by step using the given information:
1. Determine the mass of the water sample:
The given mass is 40.8g.
2. Find the specific heat capacity of water:
The specific heat capacity of water is approximately 4.184 J/g°C.
3. Calculate the change in temperature:
ΔT = 35°C - 22°C = 13°C
4. Substitute the values into the formula and calculate the energy gained:
Q = (mass) * (specific heat capacity) * (change in temperature)
= 40.8g * 4.184 J/g°C * 13°C
To get the final answer, you'll need to multiply these numbers together. In this case, I'll do the calculation for you:
Q ≈ 2198.19 J
Therefore, the water sample gains approximately 2198.19 Joules (J) of energy when its temperature increases from 22 degrees Celsius to 35 degrees Celsius in the sun.