Final answer:
The change in internal energy of the system is 0 J because no work is done. The change in temperature of the water is 47.45°C.
Step-by-step explanation:
(a) The change in internal energy of the system can be calculated using the First Law of Thermodynamics, which states that the change in internal energy of a system is equal to the heat added to the system minus the work done by the system. In this case, the work done by stirring the beaker is 133400 J, which is positive because work is done on the system. Therefore, the change in internal energy is given by:
ΔU = Q - W = 133400 J - 133400 J = 0 J
So, there is no change in the internal energy of the system.
(b) The change in temperature of the water can be calculated using the specific heat capacity equation:
Q = mcΔT
Where Q is the heat added, m is the mass of the water, c is the specific heat capacity of water, and ΔT is the change in temperature. Rearranging the equation to solve for ΔT:
ΔT = Q / (mc)
Plugging in the values:
ΔT = 133400 J / (708 g * 4.18 J/g°C) = 47.45°C
Therefore, the change in temperature of the water is 47.45°C.