Question

Please help i don't understand how to do this ill give medal for best answer :)

1.Calculate the energy change (q) of the surroundings (water) using the enthalpy equation

qwater = m × c × ΔT.

We can assume that the specific heat capacity of water is 4.18 J / (g × °C) and the density of water is 1.00 g/mL.

The water has absorbed the heat of the metal. So, qwater = qmetal

my data
Measured mass metal (Zinc) 41.664g
Distilled water measurement 26mL
Distilled water temperature 25oC
Temperature of metal 100.8oC
Temperature of mixture 34.8oC

Answer 1

Okay weird question they want enthalpy in the question, but just to please your teacher(s) we can integrate enthalpy into our equations:

First law of thermodynamics:
\[\Large \Delta U = q+w\]
Lets assume constant volume and no additional work happens:
\[\Large \Delta U=q\]
Lets assume constant pressure too:
\[\Large \Delta H = \Delta U = q\]
We assume that the only think working on the surroundings is the heat transfer from the system, so we can write:
\[\Large \Delta H=\Delta U=q=c \times m \times \Delta T\]
Use the equation above and calculate the, internal energy chance / enthalpy / heat process.

Answer 2

that the only thing working*