Observing A Chemical Reaction Lab
Introduction The purpose of this lab is to be able to observe the reaction rates of different chemical substances, by looking at which substance is the fastest reactant. This is what chemical kinetics is. Reaction rate is the change in the concentration of a reactant or product in a chemical reaction per unit time. In this lab the requirement was to be able to calculate each Average reaction rate which is the change in reactant or product concentration at a given time interval. Some equations that were required for this lab is the basic equation to determine the moles of magnesium for each piece in the lab. This formula is n=m/M. This is moles, which is equal to mass over Molar mass.
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
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