The temperature change of water depends on its specific heat capacity, which is 4.184 J/(g·°C) at room temperature and standard pressure. This means that it takes 4.184 Joules of energy to raise the temperature of 1 gram of water by 1 degree Celsius.
Using this information, we can calculate the temperature change of 25 g of water when it absorbs 840 J of energy:
Q = m * c * deltaT
where Q is the amount of energy absorbed, m is the mass of the water, c is the specific heat capacity of water, and deltaT is the change in temperature.
Rearranging this equation to solve for deltaT, we get:
deltaT = Q / (m * c)
Substituting the given values, we get:
deltaT = 840 J / (25 g * 4.184 J/(g·°C))
deltaT = 8.0 °C
Therefore, the temperature of 25 g of water will increase by 8.0 degrees Celsius if it absorbs 840 J of energy.