Final answer:
To convert the energy absorbed by water from calories to joules, multiply the given energy in calories (3.4 cal) by the conversion factor 4.184 J/cal, resulting in 14.2 J.
Step-by-step explanation:
When a container of water absorbs 3.4 calories (cal) of heat, we can convert this energy to joules (J) using the conversion factor that 1 calorie is approximately equal to 4.184 joules. The calculation is as follows:
Energy absorbed in joules = 3.4 cal × 4.184 J/cal = 14.2256 J.
When rounded to the nearest tenth, the energy absorbed is 14.2 J, which corresponds to answer option (a).
The amount of energy absorbed (in joules) is 2.67 × 10^7 J or 2.67 × 10^4 kJ.
The specific heat of water is 4.184 J/(g•°C), and the temperature change is 16.0°C. Using the equation q=mc∆T, where q is the heat absorbed, m is the mass of water, and ∆T is the temperature change, we can calculate the amount of energy absorbed by the water.
Plugging in the values, we get q = (3.99 × 10^3 g) (16.0°C) = 2.67 × 10^7 J = 2.67 × 10^4 kJ.