Unknown Rate Law Equation Lab Report

Prepare timer to start at the exact time the Alka Seltzer is dropped into the beaker of water.

We took the plastic cup and added the stir bar into it, then we inserted the plastic cup and the stir bar into the styrofoam cup. Next, we secured the clamp on the ring stand rod, and then added the solution calorimeter to the other end of the clamp. Following that, we took the beaker and filled it with distilled water and transferred it to the graduated cylinder. Then we poured it into the plastic cup with the stir bar in it. We turned the stir plate to number 6 and let the water stir around for 10 seconds, then we added in our first effervescent tablet and let it for about a minute or until it was fully dissolved. We added an extra tablet to every test until we reached the total number of tablets we could insert which was 5. After we were finished with each test, we washed out plastic cup, the solution calorimeter, and the stir

The first step that needed to be done in this experiment was adding hydrochloric acid (HCl)

After added, pick up the beaker and swirl it around lightly for a short period of time.

Three factors that can affect the rate of reaction are temperature, pH and the salinity.

Many factors effect reaction rates, two shown above include temperature and concentration. Concentration affects the rate of reactions because the more concentrated a solution the more likely collisions between particles will be. This is simply because there are more particles present to collide with each other. When the temperature is higher, particles will

mL cylinder to the beaker on the stir plate and empty it into the beaker. Place the pH probe in the beaker and record the pH in the data table. Drag the beaker to the red disposal bucket. Double-click the bottle of NaHCO3 to move it to the Stockroom counter. Repeat steps 5 and 6 for KNO3.

After the 5-minute period, take the Elodea and thermometer out of the beaker, pour the mixture into the beaker down the drain and rinse.

7. Using the slider on the right hand side, add NaOH to the HCl in the Erlenmeyer flask (This action is known as titrate). Add the indicator until the color of the indicator turns a light shade of pink.

To determine what factors influence the rate of a chemical reaction and to make predictions based on these

Submerge the graduated cylinder in the plastic tub so that it is completely filled with water. Hold the open end of the graduated cylinder and move it vertically upside-down where the open end of the graduated cylinder is still submerged in the plastic tub. Clamp the graduated cylinder the ring stand of the lab table to keep it in place. perforate a hole in the top of the rubber cork for the solution container. Cut a straw the length of about four inches. place the straw inside of the rubber cork hole. Set up your timer for two minutes.

Since the wells were already labeled I rinsed out the ceramic plate and filled each well with it corresponding substance 1-5 and one for water. Then I added 10 drops of NaOH to each well and then 4 drops of CuSO4 and mixed it. I waited five minutes before recording the color change in Table 1.3.

Another run 2 was made and the set-up where the reaction will take place was ensured to be at room temperature. 4 drops of CuSo4 was added immediately after Beaker A was poured to Beaker B. The reaction was timed until it turned to blue.

The overall aim of this experimental investigation is to further research and investigate the factors of temperature and concentration and how these two elements can alter or change the speed or rate of a reaction. The aim will be investigated thoroughly, with multiple experiments being conducted to ultimately fulfil this aim, with as much detail and data as possible so an in-depth conclusion can be delivered.

Kinetics of chemical reactions is how fast a reaction occurs and determining how the presence of reactants affects reaction rates. In this experiment the rate of reaction for Fe+3 and I- is determined. Because the rate of chemical reactions relates directly to concentration of reactants, the rate law is used to find the rate constant, and calculated with specified temperatures.