Question

If you are too vigorous in your stirring/swirling of the calorimeter, some of the contents of the plastic beaker will spill out into the Styrofoam cup.  Would making this have caused your calculated result in part A to be too high or too low.  Give a detailed explanation

Part A trial 1iial 3 Masof Calm 41, Gz1e 4211.631 clone tr t HC 1 | 6766R9| 62.34%| 61-5566g tempof aard 3.523 mes of diy22 beapir 2.2 766 2.2773 2.27165 mas or My 0.03 6 hight kemp 24.72 343 6 1o6o6 62.315, 1 5518 clsmeder 4

Answer 1

The enthalpy change of the reaction is calculated by heat released per mole of Mg.

If some of the contents from the beaker spills out; then both Mg and HCl solution are lost. As the amount of the reactsnts decreases; less heat will be produced.

But you have calculated the moles of the Mg accordong to your weight before putting it in the calorimeter.

Hence moles of Mg remains fixed and calculated enthalpy change is lower than actual.