The weight of Iron is $24\mathrm{.}9$ g

Volume of water with a mass equivalent of $1$ mL $=1$ g is $46$ mL

The temperature change is $6\mathrm{.}90$ C

$1$ a$)$ Calculate the heat change $($q$)$ experienced by the water. $(3$ sig figs$)$

b$)$ Report the enthalpy change $($H$)$ experienced by the water, using the correct sign.

c$)$Determine the moles of iron used in this experiment. Calculate the molar enthalpy change of this

reaction with respect to iron. $(3$ sig figs$)$

d$)$ Oxygen was in excess in this lab. Assuming that the iron we used completely reacted, use molar

ratios to calculate the moles of oxygen that would have also reacted. Calculate the molar enthalpy

change of this reaction with respect to oxygen. $(3$ sig figs$)$

e$)$Iron $($III$)$ oxide was produced in this lab. Assuming all the iron reacted, use molar ratios to calculate

the moles of iron $($III$)$ oxide that would be expected to form. Calculate the molar enthalpy change of

this reaction with respect to iron $($III$)$ oxide. $(3$ sig figs$)$