Factors Affecting Reaction Rates

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Factors Affecting Reaction Rates

Objective:

To determine the affect that concentration, nature of reactants, temperature and the use of a catalyst can have on reaction rates.

Materials:

See each part of procedure in lab text pg.1

Procedure:

As in lab text pg.1

Data and Observations:

Table 1: Concentration

 [HCl] Volume H2 produced (mL) Time (s) Rate (mL H2/s) 2.0 54.8 91 0.60 3.0 49.8 35 1.4 6.0 51.4 15 3.4

Table 2: Nature of Reactants

 Metal Mass Loss(g) Time (s) Rate (g/s) Mg 0.12 36 0.0033 Zn 0.11 719 0.00015

Table 3: Temperature

 Temperature of HCl Mass of Alkaseltzer(g) Time (s) Rate (g/s) Hot 3.25 69.67 0.0466 Warm 3.23 59.92 0.0539 Cold 3.24 53.07 0.0611

Table 4: Catalyst

 Reaction Before During After H2O2 solution Transparent and nothing happened. Transparent and nothing happened. Transparent and nothing happened. H2O2 solution with MnO2 Transparent and nothing happened. It began to bubble with increased temperature and get darker. It turned to black and opaque.

Sample calculations:

Part1: For [HCl]2.0

[pic 1]

Part2: For Metal Mg

[pic 2]

Part3: For cold temperature

[pic 3]

Questions:

1. Concentration:

a) The reaction rate increases as the concentration of the reaction increases, same as lab result. Because particles have to collide to react successfully, so an increase in concentration of produces makes more collisions. Therefore The chances of an effective collision goes up with the increase in concentration.

b)

 0.60mLH2 1 mol H2 1 mol Mg 24.3g Mg 91s 1s 22400mL H2 1 mol H2 1 mol Mg

=0.059g Mg

So, 0.059g of Mg was used.

2. Nature of Reactants:

a) The independent variable in the reaction was the type of metal used.

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