Question

extract catalase from the lettuce/spinach/cabbage (no organic solvents). things to consider: a) how will you extract it? b) how much of it do you need? (hint: you might want to try starting with 10 ml of catalase for 2 ml of peroxide and then adjusting based on how much oxygen is produced) c) how will you keep it stable? d) if you run out, can you make more? will it affect your results? 2. determine the partial order with respect to the peroxide, in the presence of the catalyst catalase, in the rate law. things to consider: a) what variables do you need to determine the partial order? b) which variable(s) would be dependent? which would be independent? c) how will you measure them? d) how many measurements do you need? e) how can you distribute the measurements among the group? 3. determine the activation energy for the catalase-catalysed decomposition of hydrogen peroxide.

Answer 1

Catalase can be extracted from plant tissues by homogenization and centrifugation. Partial order is determined by varying hydrogen peroxide concentrations and measuring the rate of oxygen production. Activation energy is calculated using the Arrhenius equation from rates measured at different temperatures.

Step-by-step explanation:

To extract catalase from lettuce, spinach, or cabbage, you can homogenize the plant tissue in a buffer, strain the mixture, and then centrifuge it to obtain the crude enzyme extract. You might start by trying 10ml of catalase extract to react with 2ml of hydrogen peroxide. To keep the catalase extract stable, it should be kept on ice or stored at a low temperature until use. If you run out of catalase, you can extract more, but be aware that differences in preparation could affect your results.

When determining the partial order with respect to hydrogen peroxide in the catalase-catalyzed reaction, consider the concentrations of reactants and the rate of reaction. The concentration of hydrogen peroxide is the independent variable, while the rate of oxygen production is the dependent variable. You can measure the volume of oxygen produced using a gas syringe or by displacement of water. Multiple measurements should be taken to calculate the reaction rate, and these measurements can be distributed among group members to streamline the process.

Lastly, to determine the activation energy for the decomposition of hydrogen peroxide by catalase, record the rate of reaction at various temperatures and apply the Arrhenius equation to calculate activation energy from the temperature dependence of the reaction rate.