Work of 700 J is done by stirring an insulated beaker containing 110 g of water.

(a) What is the change in the internal energy of the system?
J
(b) What is the change in the temperature of the water?
°C

(a) 700 J

(b) (Internal Energy Increase)/[(Specific Heat)*Mass]
= (700J/4.184 J/cal)/(110g*1.00 cal/g*C)
= 1.5 C

To answer these questions, we need to understand the concept of the specific heat capacity of water. The specific heat capacity (C) of a substance is the amount of heat energy required to raise the temperature of a unit mass of the substance by one degree Celsius.

For water, the specific heat capacity is approximately 4.18 J/g°C.

(a) The change in internal energy (ΔU) of the system can be calculated using the formula:
ΔU = q - w
Where q is the heat energy transferred to the system and w is the work done. In this case, since the system is insulated, there is no heat transfer (q = 0). Therefore, the change in internal energy is equal to the work done (ΔU = 700 J).

(b) The change in temperature (ΔT) of the water can be calculated using the formula:
q = m * C * ΔT
Where q is the heat energy transferred to the water, m is the mass of the water, C is the specific heat capacity of water, and ΔT is the change in temperature. Rearranging the formula, we have:
ΔT = q / (m * C)

Now we can substitute the given values:
q = 700 J (as calculated in part (a))
m = 110 g
C = 4.18 J/g°C

Substituting these values into the formula, we get:
ΔT = 700 J / (110 g * 4.18 J/g°C)
ΔT ≈ 1.5 °C

Therefore, the change in the temperature of the water is approximately 1.5 °C.