A chemical reaction takes place inside a flask submerged in a water bath. The water bath contains 3.70kg of water at 30.5 C. During the reaction 97.1 kJ of heat flows out of the flask and into the bath.

Calculate the new temperature of the water bath. You can assume that the specific heat capacity of water under these conditions is 4.18J / g*K. Round to the 3 significant digit.

The new temperature of the water bath is 36.8°C

Explanation:

A Calorimety problem to apply this formula:

Q = m. C. ΔT

Where Q is heat

m is mass

C is specific heat capacity

ΔT = T° final - T° initial

Let's make some conversion before

97.1 kJ. 1000 = 97100 Joules

3.70 kg. 1000 = 3700 g

This because the specific heat capacity units

ΔT it's a difference and mathematically, in numbers, it is the same value in °C as in K

97100 J = 3700 g. 4.18J / g°C (T°final - 30.5°C)

97100 J = 15466 J/°C (T°final - 30.5°C)

97100 J / 15466 °C/J = (T°final - 30.5°C)

6.28°C = T °final - 30.5°C

6.28° C + 30.5°C = T°final

36.8°C = T° final