Step-by-step explanation:
To calculate the amount of water that was heated, we can use the formula:
q = m * c * ΔT
where q is the amount of heat absorbed by the water, m is the mass of the water, c is the specific heat capacity of water (4.18 J/(g * °C)), and ΔT is the temperature change.
In this case, we know that 2.71 grams of fuel released 4.10 kJ of energy into some amount of water, causing its temperature to change from 22.2 C to 53.1 C. Let's first convert the energy released to joules:
4.10 kJ = 4,100 J
Next, we can calculate the amount of heat absorbed by the water using the formula above:
4,100 J = m * 4.18 J/(g * °C) * (53.1 C - 22.2 C)
Simplifying and solving for m, we get:
m = 152.3 g
Therefore, approximately 152.3 grams of water were heated by the combustion of 2.71 grams of the fuel.