Another equation used in this lab was the rate equation, which is rate=mol/s. This is rate, which is equal to moles over seconds. The average rate looks at how fast the reactant disappears and how fast the product appears. These equations are able to show comparisons, as to which substance reacted the fastest. This lab involved us using lab safety equipment such as safety goggles. In addition, we used our electronic devices (timer on phone) to determine the time. However, the only discrepancy with this was that the timing of the reaction might have not been precise. …show more content…
Rate ∆ = ( concentration of ∆ at time (t2)-concentration of ∆ at time (t1))/(t1 -t2)
Results
Magnesium with Hydrochloric acid (HCl (aq))
Mg (s) + HCl (aq) → H2 (g) + MgCl2 (aq) + heat
Mass (g) Moles (n) Time (s) Rate (mol/s)
0.02 (g) n=m/M = 0.02 (g) / 24.31 g ● mol
= 8.2 × 10-4 mol 1612.58