Figure 4a shows data on REACTION RATE vs. the effects of enzyme inhibition experiment. The enzyme did not work with the inhibitor. 5) DISSCUSION Our hypothesis was that while trying to determine the optimum temperature for peroxidase the enzyme was going to denature or that the enzyme activity was going to increase at 60°C. Based on our results we concluded that it was a moderate inhibitor because as the temperature increased the reaction rate (absorbance) also increased instead of decreasing. For the effect of the pH on the peroxidase we did think that the pH5 was going to have the greatest amount of absorbance because it reacted well and it had the most enzyme.
This explanation can be demonstrated in table 3 also because the results of the reactions demonstrates that chloride reacted more by the color of the product compared to the color of chloride in the mineral oil. Also it also demonstrates that iodine is the weakest oxidizing agent because the results show that iodide didn’t change much from the color that it showed in the mineral oil. In example 6 we have shown the activity series for the halogens used in this
is a method that was developed to help a person target which substrate of energy they are using, whether it is carbohydrates, proteins, or fats. It is useful in determining fat catabolism and ATP expenditure because the amount of the O2 used will be different for fat versus other macronutrients. Fat has a lower value than other macronutrients since fatty acids require O2 for catabolism. (Kent, 2011). In the case of COPD patients, proper nutrition can help reduce carbon dioxide levels and improve breathing.
The half reactions for this system are: Oxidation of 〖Fe〗^(2+): 〖Fe〗^(2+)→ 〖Fe〗^(3+)+1e^- Reduction of 〖MnO〗_4^-: 〖MnO〗_4^-+8H_3 O^++5e^-→ 〖Mn〗^(2+)+12H_2 O Which produces the following overall equation: 〖MnO〗_4^-+8H_3 O^++5〖Fe〗^(2+)→5〖Fe〗^(3+)+〖Mn〗^(2+)+12H_2 O Equilibrium is initially obtained at a very slow rate, therefore the titration is carried out in the presence of excess sulphuric acid (H_2 〖SO〗_4) at a high temperature; in order to drastically increase the rate at which equilibrium is attained. Potassium permanganate acts as its own satisfactory indicator since the reagent 〖MnO〗_4^- anion appears to be an intense purple colour while the product 〖Mn〗^(2+) cation has a colourless appearance. However, the end point must be read quickly as the permanganate end point gradually fades due to the 〖MnO〗_4^- reacting with the 〖Mn〗^(2+) that was formed during the titration. When performing the titration, one must be cautious as side reactions can occur and these side reactions must be prevented using appropriate chemical measures. If an insufficient amount of acid was
The only variable that is changing is the temperature meaning that the temperature and the heat of reaction have a positive correlation. If the temperature increases then the value for the enthalpy change will increase, and vice versa. All measurements, observations and calculations were carefully checked and are therefore not a source of error. One source of error could be that the calorimeter (Styrofoam cup) was uncapped and not a perfect insulator for keeping the heat from escaping. As it was uncapped some of the heat would have been lost to the air and as one of our assumptions was that the heat released by the reactions was used only to heat the water the value calculated will be off.
Purpose: Establish which salt solution would prove to be the most cost effective for the company to produce hot and cold packs that reach temperatures of 65° C and 0° C, respectively, as well as their relevant prices of production. Introduction: The Dystan Medical Supply Company is searching for a salt solution for their hot and cold packs that will be most cost effective. The cost of production per pack must be less than $5.00 for the company to make a profit. Four salts: ammonium nitrate, calcium chloride, lithium chloride, and potassium chloride will be tested to find to most cost effective solution. The salts will be dissolved in distilled water by small quantities until the reaction reaches When ionic compounds dissolve in water, they either absorb energy from or release energy to the surroundings.
The ideal gas constant value is 0.082057 (L x atm)÷(mol x K). The purpose of the experiment was to be able to measure the temperature and the mass of each gas tested, to configure a constant and determine which gas is the most “ideal”. To configure “R” the equation will be, R= PV ÷ nT. Based on our knowledge of an ideal gas, we hypothesized Pentane will have the most ideal behavior to real gas and Cyclohexane to be the least ideal. We expect Pentane to be the most ideal because it’s boiling point is the furthest away from the boiling point of water.
___T____ Enzyme reactions can be slowed or halted using inhibitors. 3. Circle the correct effect. Raising the temperature slightly will [ increase | decrease | not change ] the rate of reaction Boiling temperature will [ increase | decrease | not change ] the rate of reaction. Changing the pH toward the optimal pH will [ increase | decrease | not change ] the rate of reaction.
LABORATORY REPORT (Click on the Save a Copy button on the panel above to save your report) Activity: Name: Instructor: Date: Enzyme Activity Khadija Mohamed Dr Smith December 10, 2011 Predictions 1. Sucrase will have the greatest activity at pH 6 2. Sucrase will have the greatest activity at 40 °C (104 °F) 3. Sucrase activity increases with increasing sucrose concentration until a plateau is reached. Materials and Methods Effect of pH on Enzyme Activity.
They have a relatively high level of hydrophilicity. Conversely, cationic surfactants such as cetyltrimethyl ammonium bromide (CTAB) release a positive charge in an aqueous solution. On the other hand, in alkali pH, amphoteric surfactants act as anionic while in acid pH, it act as cationic. Non-ionic surfactants such as partially hydrolyzed PVA (polyvinyl alcohol) have no charge (Li et al, 2008). Among four types of surfactants, partially hydrolyzed PVA is most frequent used because it gives the smallest microsheres (Jeffrey et al, 1991).